A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What is the pressure of the sample if the volume changes to 268 mL while the temperature is increased to 815 K?
A. 9.83 atm
B. 1.05 atm
C. 15.3 atm
D. 6.53 atm
E. 10.2 atm

A gas has a volume of 9.0 liters at a pressure of 1520 torr. If the pressure is decreased to 380 torr, what will be its new volume? (Assume the temperature remains constant.)
A. 36 liters
B. 4.6 liters
C. 2.3 liters
D. 0.28 liters

A certain quantity of a gas occupies 61.3 mL at 68°C. If the pressure remains constant, what would the volume of the gas be at 17°C?
A. 52 mL
B. 72 mL
C. 32 mL
D. 92 mL

Consider the process of 2 H(g) → H2(g) where ΔH = −436 kJ/mol
Determine if the sentence below is true or false.
When this reaction occurs in a sealed container at constant temperature, the pressure in the container should decrease.

If you have 2.00 L of a gas initially at 1.00 atm and 27 °C, what temperature will it have at 3.00 L and 1.25 atm?

The law of Gay-Lussac describes the relationship of P and T (n and V being constant) for an ideal gas. From what you have learned about the other gas laws, which of the following expressions would be a description of Gay-Lussac law (ideal gases)?
a) P ∝ k/T
b) P ∝ T
c P = T
d) PT = constant
e) None of these

Which is a true statement about ideal gas in a container?
a) At constant temperature and a fixed amount of gas, when the pressure changes from P to 2P, the volume doubles.
b) At constant pressure and a fixed amount of gas, when the temperature increases from 20°C to 40°C, the volume doubles.
c) At constant pressure and constant volume, when the temperature changes from 100°C to 200°C, the number of gas molecules decreases by 50%.
d) At constant pressure and a fixed amount of gas, the volume is 0 L at 0 K.
e) All of the above are false statements.

If 0.300 moles of nitrogen gas occupies 0.600 L under certain conditions, what number of moles occupies 1.500 L under the same conditions?

The gas in a gas thermometer that has been placed in an oven has a volume that is 5.42 times larger than the volume that it occupies at 125°C. Determine the temperature of the oven (in degrees Celsius).
a) none of the given answers
b) 1884
c) 2430
d) 2157
e) 73.4

A 4.0 L flask containing N2 at 15 atm is connected to a 4.0 L flask containing H 2 at 7.0 atm and the gases are allowed to mix. What is the mole fraction of N2?
1. 0.75
2. Cannot be determined
3. 0.93
4. 0.26
5. 0.32
6. 0.68

1 mole of an ideal gas is kept at constant pressure but its temperature is lowered. What is the value of T when the volume of the gas reaches zero (extrapolation)?
a. 0.0°C
b. 100.00°C
c. - 273.15K
d. - 273.15°C
e. 373.15K

The gas in a gas thermometer that has been placed in an oven has a volume that is 3.68 times larger than the volume that it occupies at 158°C. Determine the temperature in the oven (in degrees Celsius).
a. 1313
b. 1586
c. 581
d. 43
e. 117

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of ___________ Law.
a. Gay-Lussac's
b. Boyle's
c. Amontons's
d. Charles's
e. Avogadro's

A gas is isothermally expanded. Which plot best shows this type of expansion?

A gas has a volume of 2.00 liters at a temperature of 127ºC. What will be the volume of the gas if the temperature is increased to 327ºC? (Assume the pressure remains constant.)
1. 2.00 liters
2. 3.00 liters
3. 4.00 liters
4. 6.00 liters

A sample of a gas occupies 460 mL at 70.0ºC and 1.00 atmosphere. At what temperature would the gas occupy 650 mL at the same pressure?
1. 99ºC
2. 111ºC
3. 188ºC
4. 212ºC
5. 435ºC
6. 154 ºC
7. -30.0ºC

What is the definition of Boyle's Law?
a) Equal volumes of different gases at the same temperature and pressure have equal numbers of molecules.
b) The pressure of a confined gas at constant volume is directly proportional to its temperature in degrees Celsius.
c) The volume of a confined gas at constant pressure is directly proportional to its absolute temperature.
d) The volume of a confined gas at constant temperature is directly proportional to its gas pressure.
e) The volume of a confined gas at constant temperature is inversely proportional to its gas pressure.

Assume that you have a cylinder with a moveable piston. What would happen to the gas volume inside the cylinder if you decrease the pressure to one quarter the original pressure while holding the temperature constant?
a. V1= 4 V2
b. No change in volume
c. V2= ¼ V1
d. V1= ¾ V2
e. V2= 4 V1

Select the expression that is a correct statement of Boyles law
a. PV = constant
b. P/V = constant
c. V/P = constant
d. V/T = constant
e. N/P = constant

What do you expect the temperature change to be for a rapid, adiabatic compression of a gas from 1.0 atm to 3.0 atm?
a. -10K
b. 100K
c. 0.001K
d. -100K
e. -0.001K

A cylinder with a moveable piston contains 0.553 mol of gas and has a volume of 253 mL. What will its volume be if an additional 0.365 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)

A sample of propane gas is placed in a 10.0 L container at 25.0°C and 725 mmHg. The gas sample is then transferred from the 10.0 L container to a 7.50 L container at 25.0°C for shipping. What is the gas pressure in the second container?
a) 760 torr
b) 0.95 atm
c) 1062 mmHg
d) 1.40 atm
e) 967 mmHg

The volume of a gas is proportional to the temperature of a gas is known as
A) Boyle’s Law
B) Charles’s Law
C) Avogadro’s Law
D) Ideal Gas Law
E) Dalton's Law

What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F 2 has a volume of 25.0 mL at 1.2 atm?
A) 7.6 mL
B) 11 mL
C) 5.5 mL
D) 3.8 mL
E) 17 mL

Which diagram best represents the final system, if the pressure of the gas in this cylinder were doubled and the temperature increased from 200 K to 400 K?

Suppose you have a fixed amount of an ideal gas at a constant volume.If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature? [Section 10.4]

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 760 mmHg and a temperature of 30 oC.What would the pressure be if the can were heated to 1155 oC?

A sample of N2O3(g) has a pressure of 0.018 atm . The temperature (in K) is then doubled and the N2O3 undergoes complete decomposition to NO2(g) and NO(g).Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.

Amontons law expresses the relationship between pressure
and temperature. Use Charless law and Boyles law to
derive the proportionality relationship between P and T.

Explain how the ideal gas law contains within it the simple gas laws (show an example).

Avogadros hypothesis. At the same volume, pressure, and temperature, samples of different gases have the same number of molecules but different masses.How many moles of gas are in each vessel?

A balloon contains 0.136 mol of gas and has a volume of 2.71 L .If an additional 0.151 mol of gas is added to the balloon (at the same temperature and pressure), what will its final volume be?

Two identical balloons are filled to the same volume, one with air and one with helium. The next day, the volume of the air-filled balloon has decreased by 5.1 % .By what percent has the volume of the helium-filled balloon decreased? (Assume that the air is four-fifths nitrogen and one-fifth oxygen, and that the temperature did not change.)

The pressure exerted on a sample of a fixed amount of gas is doubled at constant temperature,
and then the temperature of the gas in kelvins is doubled at constant pressure.What is the final volume of the gas?

A quantity of N2 gas originally held at 5.24 atm pressure in a 1.20 -L container at 26 oC is transferred to a 14.5 -L container at 20 oC. A quantity of O2 gas originally at 5.26 atm and 26 oC in a 5.20 -L container is transferred to this same container.What is the total pressure in the new container?

An automobile tire has a maximum rating of 38.0 psi (gauge pressure).The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.) at a temperature of 12.0 oC. While driving on a hot day, the tire warms to 65.0 oC and its volume expands to 12.2 L.
What is the total pressure (gauge pressure + atmospheric pressure) in the tire after warming on a hot day?

The following picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 oC. What would happen to the pressure if the volume were reduced to 0.5 L and the temperature increased to 260 oC?

In a common classroom demonstration, a balloon is filled with air and submerged in liquid nitrogen. The balloon contracts as the gases within the balloon cool. Suppose the balloon initially contains 2.96 L of air at a temperature of 25.5 oC and a pressure of 0.995 atm .Calculate the expected volume of the balloon upon cooling to -196 oC (the boiling point of liquid nitrogen). When the demonstration is carried out, the actual volume of the balloon decreases to 0.62 L .

A 160.0 -L helium tank contains pure helium at a pressure of 1860 psi and a temperature of 298 K.How many 3.5-L helium balloons can be filled from the helium in the tank? (Assume an atmospheric pressure of 1.0 atm and a temperature of 298 K.)

A particular balloon can be stretched to a maximum surface area of 1257 cm2. The balloon is filled with 3.1 L of helium gas at a pressure of 756 torr and a temperature of 298 K . The balloon is then allowed to rise in the atmosphere. Assume an atmospheric temperature of 273 K and determine at what pressure the balloon will burst. (Assume the balloon to be in the shape of a sphere.)

The volume of a sample of a fixed amount of gas is decreased from 2.0 L to 1.0 L. The temperature of the gas in Kelvins is then doubled.What is the final pressure of the gas in terms of the initial pressure?

An ideal gas at a pressure of 1.60 atm is contained in a bulb
of unknown volume. A stopcock is used to connect this
bulb with a previously evacuated bulb that has a volume
of 0.810 L as shown here. When the stopcock is opened
the gas expands into the empty bulb. If the temperature is
held constant during this process and the final pressure is
695 torr , what is the volume of the bulb that was originally
filled with gas?

Consider the apparatus shown in the drawing.When the valve between the two containers is opened and the gases allowed to mix, how does the volume occupied by the N2 gas change?

Consider the apparatus shown in the drawing.How does the volume of the O2 gas change when the gases mix?

Consider the apparatus shown in the drawing.What is the total pressure in the container after the gases mix?

Consider the apparatus shown in the drawing.What is the partial pressure of N2 after mixing?

Consider the apparatus shown in the drawing.What is the partial pressure of O2 in the mixture?

Expansion of a gas into an evacuated space is a spontaneous process.The reverse process-gas molecules initially distributed evenly in two flasks all moving into one flask-is not spontaneous.If flask B were smaller than flask A, would the final pressure after the stopcock is opened be greater than, equal to, or less than 0.5 atm?

A 16.0 -L tank is filled with helium gas at a pressure of 105 atm .How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm, assuming that the temperature remains constant and that the tank cannot be emptied below 1.00 atm?

A sample of gas has an initial volume of 5.1 L at a pressure of 748 mmHg .If the volume of the gas is increased to 9.0 L , what will the pressure be?

Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown.What is the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant? (We can neglect the volume of the capillary tubing connecting the bulbs.)

A wine-dispensing system uses argon canisters to pressurize and preserve wine in the bottle. An argon canister for the system has a volume of 59.6 mL and contains 30.1 g of argon.When the argon is released from the canister it expands to fill the wine bottle. How many 750.0-mL wine bottles can be purged with the argon in the canister at a pressure of 1.26 atm and a temperature of 297 K ?

A scuba diver creates a spherical bubble with a radius of 3.5 cm at a depth of 30.0 m where the total pressure (including atmospheric pressure) is 4.00 atm.What is the radius of the bubble when it reaches the surface of the water? (Assume atmospheric pressure to be 1.00 atm and the temperature to be 298 K.)

What happens to the pressure of a gas in a closed container if you double its
volume while its temperature is held constant?

You have a sample of gas in a container with a movable piston,
such as the one in the drawing.
Redraw the container to show what it might look like if the external pressure on the piston is increased from 1.0 atm to 2.0 atm while the temperature is kept constant.

Boyles Law: For a fixed quantity of gas at constant temperature, the volume of the gas is inversely proportional to its pressure.What would a plot of P versus 1/V look like for a fixed quantity of gas at a fixed temperature?

A 47.6-mL sample of gas in a cylinder is warmed from 24 oC to 87 oC.What is its volume at the final temperature? (Assume constant pressure.)

A natural gas storage tank is a cylinder with a moveable top. Its volume can change only as its height changes, and its radius fixed. The height of the cylinder is 22.6 m on a day when the temperature is 23 oC. The next day the height of the cylinder increases to 23.8 m when the gas expands because of a heat wave.Determine the temperature on the second day, assuming that the pressure and amount of gas in the storage tank have not changed.

Does the volume of a fixed quantity of gas decrease to half its original value
when the temperature is lowered from 100 oC to 50 oC ?

You have a sample of gas in a container with a movable piston,
such as the one in the drawing.
Redraw the container to
show what it might look like if the temperature of the gas is increased
from 300 to 500 K while the pressure is kept constant.

You have a sample of gas in a container with a movable piston,
such as the one in the drawing.
Redraw the container to show what it might look like if the temperature of the gas decreases from 300 to 200 K while the pressure is kept constant (assume the gas does not liquefy).

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

At 25.0°C, a sample of Xe gas occupies 106.5 mL in a piston-cylider apparatus when the external pressure is 644.4 torr. At what pressure (torr) will its volume become 215.2 mL if the temperature does not change? Enter your answer with two decimal places and no units.

What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 L at 2888 mmHg?

In a common classroom demonstration, a balloon is filled with air and submerged in liquid nitrogen. The balloon contracts as the gases within the balloon cool. Suppose the balloon initially contains 2.95 L of air at a temperature of 25.0 °C and a pressure of 0.998 atm. Calculate the expected volume of the balloon upon cooling to -196 °C (the boiling point of liquid nitrogen). When the demonstration is carried out, the actual volume of the balloon decreases to 0.61 L. How does the observed volume of the balloon compare to your calculated value? Can you explain the difference?

A particular balloon can be stretched to a maximum surface area of 1257 cm 2. The balloon is filled with 3.0 L of helium gas at a pressure of 755 torr and a temperature of 298 K. The balloon is then allowed to rise in the atmosphere. If the atmospheric temperature is 273 K, at what pressure will the balloon burst? (Assume the balloon to be in the shape of a sphere.)

At constant temperature if the volume of a gas sample is tripled the pressure will
1. be increased by a factor of 6.
2. be tripled.
3. be cut in half
4. be one third the original.
5. remain the same.

What volume will a balloon occupy at 1.0 atm, If the balloon has a volume of 8.8 L at 4.4 atm? a. 2.0 L b. 44 L c. 0.50 L d. 39 L

A sample of carbon dioxide gas as 125 oC and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125 oC? a. 441 torr b. 289 torrc. 356 torrd. 359 torre. 212 torr

The volume of a gas is proportional to the temperature of a gas is known asA) Avogadro's LawB) Ideal Gas LawC) Charles's LawD) Boyle's LawE) Dalton's Law

What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm?
a) 11 mL
b) 17 mL
c) 3.8 mL
d) 5.5 mL
e) 7.6 mL

On a flight to Europe, you notice that the packages of peanuts are puffed up. Why?1. The peanuts have greater velocities at high altitudes, thus causing the peanuts to exert more force on the packaging.2. The jet is over-pressurized at high altitudes, thus causing the gas inside the packages to expand.3. The air in the jet is approximately ten times hotter than on the ground, thus increasing the temperature of the gas in the packages.4. The packages are puffed up on the ground due to overinflation with helium. This type of packaging provides extra buoyancy for aircrafts.5. They were packaged at a higher pressure on the ground, thus causing the gas inside the packages to expand in the sky where the jet is at a lower pressure.

A certain quantity of a gas occupies 61.3 mL at 68°C. If the pressure remains constant, what would the volume of the gas be at 17°C?1. 72 mL2. 92 mL3. 32 mL4. 52 mL

Some students believe that professors are full of hot air. If I inhale 2.2 liters of gas at a temperature of 18.0°C and it heats to a temperature of 38.0°C in my lungs, what is the new volume of the gas (in liters)?
a) 1.04
b) 4.64
c) 0.425
d) 2.35
e) 2.06

A sample of N2O3(g) has a pressure of 0.017 atm. The temperature (in K) is then doubled and the N2O3 undergoes complete decomposition to NO2(g) and NO(g). Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.

The gas in a gas thermometer that has been placed in an oven has a volume that is 3.68 times larger than the volume that it occupies at 158°C. Determine the temperature in the oven (in degress Celsius).a) 1313b) 1586c) 581d) 43e) 117

A gas occupies 4.23 L at 2.25 atm. What is the volume at 3.46 atm?
A) 6.50 L
B) 1.84 L
C) 2.75 L
D) 32.9 L
E) 0.364 L

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant?

A weather balloon filled with hydrogen gas has a volume of 2.5 x 10 4 L at 1.3 atm and 32.0°C. At one point during its ascent, the balloon has the same volume as when it was launched, although its temperature is -8.00°C. Compute the pressure (in atm) at that point.
a) 0.0667
b) 4.5 x 10-3
c) 1.13
d) 1.50
e) 0.885

An oxygen tank of 500 L is 80 atm in a room 25°C and 1.0 atm is used for supplying oxygen to a patient. If the flow rate of oxygen coming out from the tank is set to me 1.00 L/s, about how long will this tank last for this purpose?a. 11 hrb. 5.5 hrc. 2.3 hrd. 16 mine. 8.3 min

What is the final pressure in atmosphere if 100.0 L of gas at 150.0°C and 1.00 atm pressure is compressed to 5.00 L at 642°C? Zincblende, ZnS, is the most important zinc ore. Roasting (strong heating) of ZaS is the first step in the commercial production of zinc.2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) a) no given answer is closeb) 57.1c) 43.3d) 128.4e) 85.6 In the previous question, what volume (in liters) of SO 2(g) forms per liter of O2(g) consumed? Both gases are measured at 25.0°C and 745 mm Hg.a) no given answer is close b) 1.45c) 1.67d) 1.33e) 0.667

A fuel cell car is powered by electrons harvested from the flameless, low-temperature reactionHow many liters of oxygen is needed to react with 42.0 L of hydrogen at STP?1. 21.0 L2. 32.0 L3. 63.0 L4. 84.0 L5. 22.4 L6. 672 L7. 42.0 L8. 2.02 L

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?a. 441 torrb. 289 torrc. 356 torrd. 359 torre. 212 torr

In the ideal gas law P V = n R T, P and V are1. related, but not important.2. independent of each other.3. inversely proportional. 4. lovers.5. never related mathematically.

Summarize each of the simple gas laws (Boyle's law, Charles's law, and Avogadro's law).

A gas is collected and found to fill a volume of 2.85 L at 25.0°C. What will be its volume at standard temperature?a. 1.3 Lb. 2.6 Lc. 4.5 Ld. 2.8 Le. 1.3 L

The gas in a gas thermometer that has been placed in an oven, has a volume that is 3.68 times larger than the volume that it occupied at 86°C. Determine the temperature in the oven (in degrees Celsius)a) 1048b) 316c) 3850d) 25.9e) 1321

A sample of gas has an initial volume of 13.9 L at a pressure of 1.22 atm. If the sample is compressed to a volume of 10.3 L, what is its pressure?

A syringe containing 1.55 mL of oxygen gas is cooled from 95.3°C to 0.0 °C. What is the final volume of oxygen gas?

A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 °C. The balloon rises in the atmosphere to an altitude of approximately 25,000 feet, where the pressure is 385 mmHg and the temperature is -15.0 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Avogadro's Law states that at a given temperature and pressure, what quantity is constant?
a) V + n
b) V x n
c) V/n

A piece of metal, initially at room temperature, is heated. Neither a chemical change nor a physical change takes place. During this process what remains constant? A. The densityB. The massC. The volumeD. All of these properties remain constant.

A 12 liter tank contains helium gas pressurized to 160 atm. What size tank would be needed to contain the same amount of helium at atmospheric pressure (1 atm)?

This picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 °C. Draw a similar picture showing what would happen to the sample if the volume were reduced to 0.5 L and the temperature increased to 250 °C. What would happen to the pressure?

A sample of nitrogen gas in a 1.75-L container exerts a pressure of 1.35 atm at 25 °C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 355 °C?

A sample of ideal gas at room temperature occupies a volume of 34.0 L at a pressure of 782 torr . If the pressure changes to 3910 torr , with no change in the temperature or moles of gas, what is the new volume, V2; and If the volume of the original sample in Part A (P1 = 782 torr , V1 = 34.0 L ) changes to 65.0L , without a change in the temperature or moles of gas molecules, what is the new pressure, P2.

A sample of gas in a balloon has an initial temperature of 9°C and a volume of 1200L . If the temperature changes to 85°C , and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas? What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 9°C , V1= 1200L ) to a volume of 2400L ? Assume no change in pressure or the amount of gas in the balloon.

Oxygen used in respiratory therapy is stored at room temperature under a pressure of 150 atm in a gas cylinder with a volume of 60.0 L. What volume would the oxygen occupy at 0.730 atm? Assume no temperature change; and if the oxygen flow to the patient is adjusted to 6.00 L/min at room temperature and 0.730 atm , how long will the tank of gas last?

What is the mole fraction of oxygen gas in air (see Table 5.3)? What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm?

10.79The temperature of a 5.00-L container of N2 gas is increased from 20 °C to 250 °C. If the volume is held constant, predict qualitatively how this change affects the following:(c) the strength of the impact of an average molecule with the container walls

If a car tire is filled to a pressure of 32.0 lbs/in2 (psi) measured at 76 ˚F, what will be the tire pressure if the tires heat up to 121 ˚F during driving?

10.79The temperature of a 5.00-L container of N2 gas is increased from 20 °C to 250 °C. If the volume is held constant, predict qualitatively how this change affects the following:(d) the total number of collisions of molecules with walls per second

For a given amount of gas showing ideal behavior, draw labeled graphs of:(c) the variation of P with T

If the temperature of a fixed amount of a gas is doubled at constant volume, what happens to the pressure?

If you fill your car tire to a pressure of 32 psi (pounds per square inch) on a hot summer day when the temperature is 35oC (95oF), what is the pressure (in psi) on a cold winter day when the temperature is –15oC (5oF)? Assume no gas leaks out between measurements and the volume of the tire does not change.

A sample of nitrogen gas in a 1.73-L container exerts a pressure of 1.36 atm at 26 oC.What is the pressure if the volume of the container is maintained constant and the temperature is raised to 353 oC?

What is the effect of the following on the volume of 1 mol of an ideal gas?(b) The absolute temperature is increased by a factor of 3.0 (at constant P).

A gas cylinder is filled with argon at a pressure of 177 atm and 25°C. What is the gas pressure when the temperature of the cylinder and its contents are heated to 195°C by exposure to fire?

A bicycle tire is filled to a pressure of 110 psi at a temperature of 30.0°C. At what temperature will the air pressure in the tire decrease to 105 psi? Assume that the volume of the tire remains constant.

A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the pressure in the hot can?

A truck tire has a volume of 218 L and is filled with air to 35.0 psi at 295 K. After a drive, the air heats up to 318 K. (a) If the tire volume is constant, what is the pressure (in psi)?

Nitrogen and hydrogen react to form ammonia according to the following equation:N2(g) + 3 H2(g) → 2 NH3(g)Consider the following representations of the initial mixture of reactants and the resulting
mixture after the reaction has been allowed to react for some time:If the volume is kept constant, and nothing is added to the reaction mixture, what
happens to the total pressure during the course of the reaction?

Explain how Boyle's law, Charles's law, Avogadro's law, and Dalton's law all follow from kinetic molecular theory.

Which of the following statements is(are) true?a. If the number of moles of a gas is doubled, the volume will double, assuming the pressure and temperature of the gas remain constant.b. If the temperature of a gas increases from 25°C to 50°C, the volume of the gas would double, assuming that the pressure and the number of moles of gas remain constant. c. The device that measures atmospheric pressure is called a barometer.d. If the volume of a gas decreases by one half, then the pressure would double, assuming that the number of moles and the temperature of the gas remain constant.

You have a gas in a container fitted with a piston, and you change one of the conditions of the gas such that a change takes place, as shown below:State two distinct changes you can make to accomplish this, and explain why each would work.

You have a gas in a container fitted with a piston, and you change one of the conditions of the gas such that a change takes place, as shown below:State three distinct changes you can make to accomplish this, and explain why each would work.

One way to state Boyle’s law is “All other things being equal, the pressure of a gas is inversely proportional to its volume.” (a) What is the meaning of the term “inversely proportional?”

One way to state Boyle’s law is “All other things being equal, the pressure of a gas is inversely proportional to its volume.”(b) What are the “other things” that must be equal?

An alternate way to state Avogadro’s law is “All other things being equal, the number of molecules in a gas is directly proportional to the volume of the gas.” (a) What is the meaning of the term “directly proportional?”

An alternate way to state Avogadro’s law is “All other things being equal, the number of molecules in a gas is directly proportional to the volume of the gas.”(b) What are the “other things” that must be equal?

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).a. PV versus V with constant T

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).b. P versus T with constant V

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).c. T versus V with constant P

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).d. P versus V with constant T

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).e. P versus 1/V with constant T

Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvin).f. PV/T versus P

A form of Boyle’s law is PV = k (at constant T and n). Table 8-1 contains actual data from pressure–volume experiments conducted by Robert Boyle. The value of k in most experiments is 14.1 x 102 in Hg • in3. Express k in units of atm • L. In Example 8-3, k was determined for NH3 at various pressures and volumes. Give some reasons why the k values differ so dramatically between Example 8-3 and Table 8-1.

A cylinder with a moveable piston contains 0.551 mol of gas and has a volume of 251 mL .What will its volume be if an additional 0.276 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)

An 11.2-L sample of gas is determined to contain 0.50 mole of N2. At the same temperature and pressure, how many moles of gas would there be in a 20.-L sample?

In A, the picture shows a cylinder with 0.1 mol of a gas that behaves ideally. Choose the cylinder (B, C, or D) that correctly represents the volume of the gas after each of the following changes. If none of the cylinders is correct, specify “none.”(d) 0.1 mol of gas is added at fixed P and T.

A chemical reaction occurring in a cylinder equipped with a moveable piston produces 0.641 mol of a gaseous product. If the cylinder contained 0.220 mol of gas before the reaction and had an initial volume of 2.11 L , what was its volume after the reaction? (Assume that pressure and temperature are constant and that the initial amount of gas completely reacts.)

What is the effect of the following on the volume of 1 mol of an ideal gas?(c) Three more moles of the gas are added (at constant P and T).

What is the effect of the following on the volume of 1 mol of an ideal gas?(b) Half the gas escapes (at constant P and T).

A balloon filled with 1.92 g of helium has a volume of 12.5 L. What is the balloon’s volume after 0.850 g of helium has leaked out through a small hole (assume constant pressure and temperature)?

The average person takes 500 mL of air into the lungs with each normal inhalation, which corresponds to approximately 1×1022 molecules of air. Calculate the number of molecules of air inhaled by a person with a respiratory problem who takes in only 350 mL of air with each breath. Assume constant pressure and temperature.

A balloon inflated with three breaths of air has a volume of 1.7 L. At the same temperature and pressure, what is the volume of the balloon if five more same-sized breaths are added to the balloon?

In the four piston-cylinder assemblies below, the reactant in the left cylinder is about to undergo a reaction at constant T and P:Which of the other three depictions best represents the products of the reaction?

Methanol, CH3OH, is produced industrially by the following reaction:Assuming that the gases behave as ideal gases, find the ratio of the total volume of the reactants to the final volume.

You have a gas at 25 oC confined to a cylinder with a movable piston.Which of the following actions would double the gas pressure?(a) Lifting up on the piston to double the volume while keeping the temperature constant(b) Heating the gas so that its temperature rises from 25 °C to 50 °C, while keeping the volume constant(c) Pushing down on the piston to halve the volume while keeping the temperature constant

A gas occupies a volume of 0.75 L at 20 oC at 720 torr. What volume would the gas occupy at 41 oC and 760 torr?

Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24 oC.At what temperature will the volume be 15.10
L if the pressure is 875
torr?

A weather balloon is inflated to a volume of 27.6 L at a pressure of 743 mmHg and a temperature of 28.1 oC. The balloon rises in the atmosphere to an altitude where the pressure is 385 mmHg and the temperature is -14.9 oC.Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24 oC.At what pressure will the volume equal 6.60 L if the temperature is 57 oC?

Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 55.0 gallons and which contains O2 gas at a pressure of 16,500 kPa at 24 oC.What would be the pressure of the gas, in kPa, if it were transferred to a container at 24 oC whose volume is 55.0 L?

A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25°C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15°C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?

In A, the picture shows a cylinder with 0.1 mol of a gas that behaves ideally. Choose the cylinder (B, C, or D) that correctly represents the volume of the gas after each of the following changes. If none of the cylinders is correct, specify “none.”(e) 0.1 mol of gas is added and P is doubled at fixed T.

What is the effect of the following on the volume of 1 mol of an ideal gas?(a) The pressure changes from 760 torr to 202 kPa, and the temperature changes from 37°C to 155 K.

What is the effect of the following on the volume of 1 mol of an ideal gas?(b) The temperature changes from 305 K to 32°C, and the pressure changes from 2 atm to 101 kPa.

What is the effect of the following on the volume of 1 mol of an ideal gas?(a) The initial pressure is 722 torr, and the final pressure is 0.950 atm; the initial temperature is 32°F, and the final temperature is 273 K.

What is the effect of the following on the volume of 1 mol of an ideal gas?(c) Both the pressure and temperature decrease to one-fourth of their initial values.

A bicycle tire is filled with air to a pressure of 75 psi at a temperature of 19°C. Riding the bike on asphalt on a hot day increases the temperature of the tire to 58°C. The volume of the tire increases by 4.0%. What is the new pressure in the bicycle tire?

Will the volume of a gas increase, decrease, or remain unchanged with each of the following sets of changes?(a) The pressure is decreased from 2 atm to 1 atm, while the temperature is decreased from 200°C to 100°C.

A sample of carbon monoxide occupies 3.65 L at 298 K and 745 torr. Find its volume at −14°C and 367 torr.

Will the volume of a gas increase, decrease, or remain unchanged with each of the following sets of changes?(b) The pressure is increased from 1 atm to 3 atm, while the temperature is increased from 100°C to 300°C.

Will the volume of a gas increase, decrease, or remain unchanged with each of the following sets of changes?(d) The pressure is increased from 0.2 atm to 0.4 atm, while the temperature is decreased from 300°C to 150°C.

Will the volume of a gas increase, decrease, or remain unchanged with each of the following sets of changes?(c) The pressure is increased from 3 atm to 6 atm, while the temperature is increased from −73°C to 127°C.

What will be the effect on the volume of an ideal gas if the pressure is doubled and the absolute temperature is halved?

A container is filled with an ideal gas to a pressure of 11.0 atm at 0°C.a. What will be the pressure in the container if it is heated to 45°C?

A container is filled with an ideal gas to a pressure of 11.0 atm at 0°C.b. At what temperature would the pressure be 6.50 atm?

A container is filled with an ideal gas to a pressure of 11.0 atm at 0°C.c. At what temperature would the pressure be 25.0 atm?

What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 °C and 744 torr?

An ideal gas is contained in a cylinder with a volume of 5.0 x 102 mL at a temperature of 30.°C and a pressure of710. torr. The gas is then compressed to a volume of 25 mL, and the temperature is raised to 820.°C. What is the new pressure of the gas?

A high altitude balloon is filled with 1.41 × 104 L of hydrogen at a temperature of 21 °C and a pressure of 745 torr. What is the volume of the balloon at a height of 20 km, where the temperature is –48 °C and the pressure is 63.1 torr?

A cylinder of medical oxygen has a volume of 35.4 L, and contains O2 at a pressure of 151 atm and a temperature of 25 °C. What volume of O2 does this correspond to at normal body conditions, that is, 1 atm and 37 °C?

A truck tire has a volume of 218 L and is filled with air to 35.0 psi at 295 K. After a drive, the air heats up to 318 K. (b) If the tire volume increases 2.0%, what is the pressure (in psi)?

A sealed balloon is filled with 1.00 L helium at 23°C and 1.00 atm. The balloon rises to a point in the atmosphere wherethe pressure is 220. torr and the temperature is -31°C. What is the change in volume of the balloon as it ascends from1.00 atm to a pressure of 220. torr?

For a given amount of gas showing ideal behavior, draw labeled graphs of:(a) the variation of P with V

For a given amount of gas showing ideal behavior, draw labeled graphs of:(d) the variation ofwith V

A 15.0-L tank is filled with H2 to a pressure of 2.00 x 102 atm. How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm from the tank? Assume that there is no temperature change and that the tank cannot be emptied below 1.00 atm pressure.

A sample of gas has an initial volume of 13.8 L at a pressure of 1.26 atm .If the sample is compressed to a volume of 10.8 L , what is its pressure?

If the volume of a fixed amount of a gas is tripled at constant temperature, what happens to the pressure?

Consider the flasks in the following diagrams.d. Solve for the final partial pressures of helium and neon in terms of their original pressures. Assume the temperature is constant.

In A, the picture shows a cylinder with 0.1 mol of a gas that behaves ideally. Choose the cylinder (B, C, or D) that correctly represents the volume of the gas after each of the following changes. If none of the cylinders is correct, specify “none.”(a) P is doubled at fixed n and T.

A particular balloon is designed by its manufacturer to be inflated to a volume of no more than 2.5 L. If the balloon is filled with 2.0 L helium at sea level, is released, and rises to an altitude at which the atmospheric pressure is only 500. mm Hg, will the balloon burst? (Assume temperature is constant.)

A 280-mL flask contains pure helium at a pressure of 753 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 723 torr .If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of helium?

A 280-mL flask contains pure helium at a pressure of 753 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 723 torr .If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of argon?

A snorkeler takes a syringe filled with 20 mL of air from the surface, where the pressure is 1.0 atm, to an unknown depth. The volume of the air in the syringe at this depth is 7.6 mL .If the pressure increases by an additional 1 atm for every 10 m of depth, how deep is the snorkeler?

A 280-mL flask contains pure helium at a pressure of 753 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 723 torr .If we connect the two flasks through a stopcock and we open the stopcock, what is the total pressure?

Explain how the volume of the bubbles exhausted by a scuba diver (Figure 9.16) change as they rise to the surface, assuming that they remain intact.

What is the effect of the following on the volume of 1 mol of an ideal gas?(a) The pressure is tripled (at constant T).

What is the effect of the following on the volume of 1 mol of an ideal gas?(c) The pressure is reduced by a factor of 4 (at constant T).

A 1.0-L sample of air is collected at 25°C at sea level (1.00 atm). Estimate the volume this sample of air would have at an altitude of 15 km (see Fig. 8-30). At 15 km, the pressure is about 0.1 atm.

What is the effect of the following on the volume of 1 mol of an ideal gas?(c) Pressure increases from 2 atm to 6 atm (at constant T).

A weather balloon is filled with helium to a volume of 1.61 L at 734 torr. What is the volume of the balloon after it has been released and its pressure has dropped to 0.844 atm? Assume that the temperature remains constant.

A sample of methane is placed in a 10.0-L container at 25°C and 725 mmHg. The gas sample is then moved to a 7.50-L container at 25°C. What is the gas pressure in the second container?

How would the graph in Figure 9.13 change if the number of moles of gas in the sample used to determine the curve were doubled?

In addition to the data found in Figure 9.13, what other information do we need to find the mass of the sample of air used to determine the graph?

Determine the pressure of the gas in the syringe shown in Figure 9.13 when its volume is 12.5 mL, using:(a) the appropriate graph

Determine the pressure of the gas in the syringe shown in Figure 9.13 when its volume is 12.5 mL, using:(b) Boyle’s law

A gas sample has an initial pressure of 571 mmHg and an initial volume of 0.526 L .What is the pressure (in atm) when the volume of the sample is decreased to 226 mL ? (Assume constant temperature and constant number of moles of gas.)

A large scuba tank (Figure 9.16) with a volume of 18 L is rated for a pressure of 220 bar. The tank is filled at 20 °C and contains enough air to supply 1860 L of air to a diver at a pressure of 2.37 atm (a depth of 45 feet). Was the tank filled to capacity at 20 °C?

A fixed quantity of gas at 23 oC exhibits a pressure of 756
torr and occupies a volume of 5.32
L.Calculate the volume the gas will occupy if the pressure is increased to 1.88
atm while the temperature is held constant.

For a given amount of gas showing ideal behavior, draw labeled graphs of:(b) the variation of V with T

A syringe containing 1.56 mL of oxygen gas is cooled from 95.0 oC to 0.6 oC. What is the final volume Vf of oxygen gas? (Assume that the pressure is constant.)

In A, the picture shows a cylinder with 0.1 mol of a gas that behaves ideally. Choose the cylinder (B, C, or D) that correctly represents the volume of the gas after each of the following changes. If none of the cylinders is correct, specify “none.”(b) T is reduced from 400 K to 200 K at fixed n and P.

In A, the picture shows a cylinder with 0.1 mol of a gas that behaves ideally. Choose the cylinder (B, C, or D) that correctly represents the volume of the gas after each of the following changes. If none of the cylinders is correct, specify “none.”(c) T is increased from 100°C to 200°C at fixed n and P.

A balloon is filled to a volume of 7.00 x 102 mL at a temperature of 20.0°C. The balloon is then cooled at constant pressure to a temperature of 1.00 x 102 K. What is the final volume of the balloon?

A gas in a cylinder with a moveable piston has an initial volume of 88.2 mL . If we heat the gas from 36 oC to 156 oC, what is its final volume (in mL)?

A gas sample has a volume of 166 mL at 0.00 oC. The temperature is raised (at constant pressure) until the volume is 221 mL .What is the temperature of the gas sample in oC at this volume?

What is the effect of the following on the volume of 1 mol of an ideal gas?(a) Temperature decreases from 800 K to 400 K (at constant P).

What is the effect of the following on the volume of 1 mol of an ideal gas?(b) Temperature increases from 250°C to 500°C (at constant P).

A sample of sulfur hexafluoride gas occupies 9.10 L at 198°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 2.50 L?

A 93-L sample of dry air cools from 145°C to −22°C while the pressure is maintained at 2.85 atm. What is the final volume?

How would the graph in Figure 9.12 change if the number of moles of gas in the sample used to determine the curve were doubled?

Determine the volume of 1 mol of CH4 gas at 150 K and 1 atm, using Figure 9.12

A 2.50-L volume of hydrogen measured at –196 °C is warmed to 100 °C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

An ideal gas at 7°C is in a spherical flexible container having a radius of 1.00 cm. The gas is heated at constant pressure to 888°C. Determine the radius of the spherical container after the gas is heated. [Volume of a sphere = (4/3)πr3.]

A fixed quantity of gas at 23 oC exhibits a pressure of 756
torr and occupies a volume of 5.32
L.Calculate the volume the gas will occupy if the temperature is increased to 175 oC while the pressure is held constant.

What is the volume occupied by 18.6 g of argon gas at a pressure of 1.19 atm and a temperature of 394 K? Express your answer with the appropriate units. Compare the volume of 18.6 g of helium to 18.6 g of argon gas (under identical conditions). The volume would be greater for helium gas. The volume would be the same for helium gas. The volume would be lower for helium gas.

A sample of gas (24.2 g) initially at 3.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was ____ atm. 4.008.0012.016.02.00

A sample of an ideal gas has a volume of 2.22 L at 279 K and 1.05 atm. Calculate the pressure when the volume is 1.73 L and the temperature is 303 K.

A helium-filled balloon of the type used in long-distance flying contains 420, 000 ft^3 (1.2 times 10^7 L) of helium. Suppose you fill the balloon with helium on the ground, where the pressure is 741 mm Hg and the temperature is 24.4 degree C. When the balloon ascends to a height of 2 miles, where the pressure is only 600. mm Hg and the temperature is -33 degree C, what volume is occupied by the helium gas? Assume the pressure inside the balloon matches the external pressure.

A 36.4 - L volume of methane gas is heated from 22°C to 78°C at constant pressure. What is the final volume of the gas?

A gas evolved during the fermentation of glucose (wine making) has a volume of 2.30 L when measured at 24°C and 1.00 atm. What was the volume of this gas at the fermentation temperature of 37.0 °C and 1.00 atm pressure?

A hot air balloon is filled with 1.51 x 106 L of an ideal gas on a cool morning (11oC). The air is heated to 125oC. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

A flexible container at an initial volume of 7.14 L contains 2.51 mol of gas. More gas is then added to the container until it reaches a final volume of 17.3 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.

A gas sample has a volume of 125 mL at 28°C. What is its volume at 105°C?

A sealed container holding 0.0255 L of an ideal gas at 0.993 atm and 73°C is placed into a refrigerator and cooled to 43°C with no change in volume. Calculate the final pressure of the gas.

The ideal gas law (PV = nRT) describes the relationship among pressure P. volume V, temperature T. and molar amount n. When some of these variables are constant, the ideal gas law can be rearranged in different ways to take the following forms where k is a constant. Part CA cylinder with a movable piston contains 2.00 g of helium. He at room temperature. More helium was added to the a under and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 4.30 L? (The temperature was held constant) Express your answer with the appropriate units.

Enter your answer in the provided box.Under constant-pressure conditions a sample of hydrogen gas initially at 73.00 °C and 9.40 L is cooled until its final volume is 1.70 L. What is its final temperature?

If a fixed amount of a gas is at a pressure of 2.71 atm and has a volume of 85.3 L at a temperature of 173.4 K, what is the final temperature of the gas if the pressure changes to 1.04 atm in a 105.3 L container?a. 82.1 Kb. 49.8 Kc. 75.9 Kd. 557.8 Ke. 366.0 K

A sample of an ideal gas has a volume of 3.15 L at 10.20°C and 1.50 atm. What is the volume of the gas at 20.80°C and 0.987 atm?

What is the change in temperature of a 2.50 L system when it is compressed to 1.75 L. If the initial temperature was 299 K? Select one: a. -89 K b. -98 K c. None of these d. 290 K e. 209 K

Part AA syringe containing 1.63 mL of oxygen gas is cooled from 96.4°C to 0.1°C. What is the final volume Vf of oxygen gas? (Assume that the pressure is constant.)

A sample of an ideal gas at 1.00 atm and a volume of 1.16 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 50.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

A sample of a gas occupies 1.40 L at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg? a. 2.8 L b. 2.10 L c. 1.40 L d. 1.05 L e. 0.700 L

A cylinder with a moveable piston contains 0.507 mol of gas and has a volume of 240 mL. Part AWhat will its volume be if an additional 0.237 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)

A sample of an ideal gas has a volume of 2.34 L at 289 K and 1.03 atm. Calculate the pressure when the volume is 1.63 L and the temperature is 303 K.

A sample of gas in a cylinder as in the example in Part A has an initial volume of 66.0 L, and you have determined that it contains 2.00 moles of gas. The next day you notice that some of the gas has leaked out. The pressure and temperature remain the same, but the volume has changed to 16.5 L. How many moles of gas (n2) remain in the cylinder? Express your answer with the appropriate units.

Under constant-pressure conditions a sample of hydrogen gas initially at 63.00°C and 8.90 L is cooled until its final volume is 4.10 L. What is its final temperature?

A cylinder with a moveable piston contains 0.95 mol of gas and has a volume of 343 mL. Part AWhat will its volume be if an additional 0.17 mol of gas is added to the cylinder? Express your answer using two significant figures.

Consider 4.60 L of a gas at 365 mmHg and 20 °C. If the container is compressed to 2.00 L and the temperature is increased to 39 °C, what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder. Express your answer with the appropriate units.

A sample of a gas in a piston/cylinder apparatus occupies 41.6 mL at 1.1 atm and 18.6°C. If the volume of the sample is increased to 65.4 mL and the temperature changes to 39°C, what is the new pressure, in atm, of the sample? Enter your answer with three decimal places and no units.

A balloon containing methane gas has a volume of 1.38 L at 33.0°C. What volume will the balloon occupy at 66.0°C?

A sample of gas in a balloon has an initial temperature of 37°C and a volume of 1.97 x 103 L. If the temperature changes to 93°C, and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas? Express your answer with the appropriate units.

A sample of O2 gas occupies a volume of 832 mL at 14°C. If pressure remains constant, what would be the new volume if the temperature changed to: New volume (a) -5°C mL (b) 95°F mL (c) 1095 K mL

Part A A sample of gas in a balloon has an initial temperature of 15°C and a volume of 1.52 x 103 L. If the temperature changes to 59°C, and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas? Express your answer with the appropriate units.

A sample of krypton gas occupies a volume of 6.43 L at 53°C and 0.4520 atm. If the volume of the gas sample is increased to 8220.0 mL, while its temperature is decreased to -19°C, the resulting gas pressure, in torr, will be ___ torr.

What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 12 °C, V1 = 1 77 x 103 L) to a volume of 3.54 x 103 L? Assume no change in pressure or the amount of gas in the balloon. Express your answer with the appropriate units.

What pressure would need to be applied to sample of gas with an initial volume of 979.2 mL at a pressure of 588.0 torr to decrease the volume to 325.2 mL?

A sample of an ideal gas at 1.00 atm and a volume of 1.81 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 15.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

The volume of a gas is 4.58 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume if changed to 8.64 L? (The temperature remains constant.) Enter your answer in scientific notation.

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 765 mmHg and a temperature of 25°C.Part AWhat would the pressure be if the can were heated to 1180°C?

If a sample of oxygen gas occupies 30.0 mL at -10°C and 680 mmHg, what is the volume at 10°C and 310 mmHg? Express your answer to two significant figures and include the appropriate units.

A sample of an ideal gas has a volume of 2.26 L at 288 K and 1.11 atm. Calculate the pressure when the volume is 1.04 L and the temperature is 299 K.

Part CA certain gas is present in a 15.0 L atm pressure. If the pressure is increased to 8.0 atm, the volume of the gas decreases to 7.5 L. Find the two constants k1, the initial value of k, and kf, to final volume of k, to verily whether the gas obeys Boyle's law. Express your answers to two significant figures separated by a comma. Part DIf a certain gas occupies a volume of 12 L when the applied pressure is 6.0 atm, find the pressure when the gas occupies a volume of 3.0L. Express your answer to two significant figures, and include the appropriate units.

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and 1.35 atm? a. 19.0 L b. 77.9 L c. 10.9 L d. 38.3 L e. 5.38 L

In this problem, your answers mathematical expressions involving a variable. a) Consider an ideal gas with an absolute temperature of T1. To what temperature would you need to heat the gas to double its pressure? Express your answer in terms of T1. b) Consider an ideal gas with a volume of V1. To what volume would you need to compress the gas to double its pressure? Express your answer in terms of V1.

When the volume of a gas is changed from _________ L to 4.50 L, the temperature will change from 38.1°C to 15.0°C.

A sample of helium gas occupies a volume of 161.0 mL at a pressure of 712.0 mm Hg and a temperature of 306.0 K. What will the volume be at a pressure of 474.0 mm Hg and a temperature of 804.0 K? The combined gas law equation is given below. P1V1/T1 = P2V2/T2 In this equation, P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.

A sample of an ideal gas is contained inside a rigid cylinder with a fixed volume. At 217 K, the pressure of the gas in the cylinder is 1.90 atm. At what temperature will the pressure inside the cylinder be 2.68 atm?

What mass of iron(II) oxide must be used in the reaction given by the equation below to release 28.8 kJ? 6FeO (s) + O2 (g) = > 2Fe3O4 (s) ΔH° = -635 kJ Calculate your answer in g. Enter it with two decimal places and no units.

A hot air balloon is filed with 1.51 x 10 6 L of an Ideal gas on a cool morning (11°C). The air is heated to 101°C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

A 18.0 L sample of hydrogen gas has a pressure of 26.0 atm. What volume would this gas occupy at 4.10 atm? Assume ideal behavior.

A cylinder with a moveable piston contains 0.562 mol of gas and has a volume of 236 mL. Part AWhat will its volume be if an additional 0.224 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)

A balloon filled with helium has a volume of 11.9 L at 283 K. What volume will the balloon occupy at 251 K?

A sample of gas with a volume of 3.25 L and a pressure of 785 torr is compressed to a volume of 1.30 L at constant temperature. What is the new pressure (in torr), assuming the amount remains constant?a. 8290 b. 1960 c. 0.000510 d. 314e. 44.3

What is the final temperature (°C) of a gas? Initial Status: 1 atm, 2L, 30°C Final Status: 2 atm, 4L, ____°C (a) None of the above (b) 1212 Celsius degree (c) 939 Celsius degree (d) 120 Celsius degree

A fixed quantity of gas at 28°C exhibits a pressure of 737 torr and occupies a volume of 5.50 L. (See the table of physical data.) (a) Calculate the volume the gas will occupy if the pressure is increased to 1.87 atm while the temperature is held constant. (b) Calculate the volume the gas will occupy if the temperature is increased to 164°C while the pressure is held constant.

A balloon containing methane gas has a volume of 5.06 L at 95.0°C. What volume will the ballon occupy at 1.90 × 102°C?

A hot air balloon is filled with 1.25 x 106 L of an ideal gas on a cool moming (11°C). The air is heated to 123°C, what is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

A sealed container holding 0.0255 L of an ideal gas at 0.983 atm and 75 cooled to 43°C with no change in is placed into a refrigerator and culate the final pressure of the gas.

A 128 mL bubble of hot gases at 213°C and 1.90 atm is emitted from an active volcano.Part A What is the final temperature in degree Celsius, of the gas in the bubble outside the of the final volume of the bubble is 136 mL and the pressure is 0.600 atm, If the amount of the gas does not change? Express your answer using two significant figures.

A sample of N2 gas has a volume of 15.0 L at a pressure of 1.50 atm and a temperature of 23°C. What volume, in liters, will the gas occupy at 3.50 atm and 281°C? Assume ideal behavior. V =

If the initial temperature of an ideal gas at 2.250 atm is 62.00°C, what final temperature would cause the pressure to be reduced to 1.600 atm?

The temperature of a sample of an ideal gas is doubled. If the pressure and amount of gas remain the same, what will happen to the volume of the gas? The volume of the gas will be _____________.

A sample of xenon gas occupies a volume of 5.03 L at 435 K. If the pressure remains constant, at what temperature will this same xenon gas sample have a volume of 1.85 L?

Part AA syringe containing 1.35 mL of oxygen gas is cooled from 98.4°C to 0.3°C. What is the final volume?(Assume that the pressure is constant.)

A gas is placed in a 5.0-mL syringe. It exerts 141 mm Hg of pressure on the inside walls of the syringe. The syringe's plunger is pressed, reducing the volume of the syringe to 2.9 mL. The cap was not removed from the syringe, so none of the gas escapes. Assuming the temperature of the gas does not change, use Boyle's law (below) to determine the pressure of the compressed gas. P1V1 = P2V2

A 10.5 L balloon contains heim gas at a pressure of 620 mmHg. What is the final pressure, in millimeters of mercury, of the helium gas at each of the following volumes, if there is no mmHg change in temperature and amount of gas? Part B 200 L Part C 3400 mLPart D 1210 mL

A fixed quantity of gas at 24°C exhibits a pressure of 736 torr and occupies a volume of 5.46 L. (See the table of physical data.) (a) Calculate the volume the gas will occupy if the pressure is increased to 1.93 atm while the temperature is held constant. (b) Calculate the volume the gas will occupy if the temperature is increased to 152°C while the pressure is held constant.

An ideal gas in a sealed container has an initial volume of 2.55 L. At constant pressure, it is cooled to 23.00 °C where its final volume is 1.75 L. What was the initial temperature?

A sample of chlorine gas occupies a volume of 873 mL at a pressure of 467 mmHg. Calculate the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 121 mL. Enter your answer in scientific notation.

A balloon contains 413 mL of gas at 20.85 °C. A student places the balloon outside, where it sits for several hours at a temperature of 4.65 °C. Assuming there is no change in pressure for the balloon, use Charles' law (below) to determine the new volume of the gas. v1/T1 = v2/T2

What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 37°C, V1 = 1.97 x 103 L) to a volume of 3.94 x 103 L? Assume no change in pressure or the amount of gas in the balloon. Express your answer with the appropriate units.

A hot air balloon is filled with 1.11 x 106 L of an ideal gas on a cool morning (11oC). The air is heated to 121oC. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

If the initial temperature of an ideal gas at 2.250 atm is 62.00°C, what final temperature would cause the pressure to be reduced to 1.750 atm?

A sample of an ideal gas at 1.00 atm and a volume of 1.77 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 65.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

Part A A syringe containing 1.62 mL oxygen gas is cooled from 92.6°C to .9°C. What is the final volume Vf of oxygen gas (Assume that the pressure is constant.)

A sample of an ideal gas has a volume or 2 25 L at 284 K and 1.13 atm. Calculate the pressure when the volume is 1.83 L and the temperature is 298 K

The pressure of a sample of argon gas was increased from 370 atm to 8.54 atrn at constant term final of the argon sample was what was the initial volume of the sample? Assurne ideal behavior.

A student is experimenting with gases. She finds that 0.13 mol of hydrogen gas (H2) has a volume of 4.6 L. She wants to measure the volume of 0.050 mol of oxygen gas (O2). What volume should she expect the oxygen gas to have? (Use the equation for Avogadro's law.)

A fire extinguisher has a pressure of 10 atm 25°C. Part A What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 80°C if V and n are constant?

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature? a. 22.3 L b. 31.2 L c. 44.9L d. 112 L e. 380 L

A sample of carbon monoxide initially at 49.0 °C was heated to 98.0 °C. If the volume of the carbon monoxide sample at 98.0 °C is 888.7 mL, what was its volume at 49.0 °C?

Part AA sample of gas in a balloon has an initial temperature of 36 °C and a volume of 1640 L. If the temperature changes to 91 °C, and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas? Express your answer with the appropriate units.

A balloon containing 0.146 mol Ne gas has a volume of 1.7 L at 2.1 atm and 28 °C. How many grams of neon should be added to the balloon to increase the volume to 3.1 L at the same pressure and temperature?

An ideal gas is allowed to expand from 9.00 L to 76.5 L at constant temperature. By what factor does the volume increase? The pressure will • increase by that same factor • decrease by that same factor If the intial pressure was 143 atm, what is the final pressure?

Part AA gas has a volume of 36.0 L and a pressure of 750. torr when the temperature is 10°C. What is the pressure if the volume change to 15.0 L and the temperature changes to 78°C, if the amount of gas stays the same? Express your answer using three significant figures.

A 6.9 mL sample of CO2 gas is enclosed in a gas-tight syringe at 20°C. If the syringe is immersed in an ice bath (0°C), what is the gas volume, assuming that pressure is held constant?

An arctic weather balloon is filled with 1.87 L of helium gas inside a prep shed. The temperature inside the shed is 15.°C. The balloon is then taken outside, where the temperature is - 43.°C. Calculate the new volume (L) of the balloon. You may assume the pressure on the balloon stays constant at exactly 1 atm. Round your answer to 3 significant digits.

An ideal gas is allowed to expand from 4.60 L to 34.5 L at constant temperature. By what factor does the volume increase? The pressure will • increase by that same factor. • decrease by that same factor. If the initial pressure was 109 atm, what is the final pressure?

An ideal gas is allowed to expand from 5.60L to 14.0 L at constant temperature. By what factor does the volume increase? The pressure will lf the intial pressure was 117 atm, what is the final pressure?

A sample of an ideal gas has a volume of 2.24 L at 284 K and 1.10 atm. Calculate the pressure when the volume is 1.01 L and the temperature is 302 K.

A 125.0-mL contains a gas at 27°C and 760 mm Hg of pressure. The gas is pumped into an empty 1.50-L flask also at a temperature of 27°C. What is the pressure (in atm) of the gas in the new flask? Show your work for partial credit.P1 V1/T1 = P2V2/T2 1 atm = 760 Torr = 760 mmHg = 101325 Pa = 1.01325 bar

A balloon filled with helium has a volume of 11.7 Lat 287 K. What volume will the balloon occupy at 256 K?

Enter your answer in the provided box.A gas at 693 mmHg and 31 °C occupies a volume of 7.04 L. Calculate its volume at STP.

The following picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25°C. (Figure 1)What would happen to the pressure if the volume were reduced to 0.5 L and the temperature increased to 260°C? Express your answer using one significant figure.

A sample of a gas at room temperature occupies a volume of 20.0 L at a pressure of 472 torr. If the pressure changes to 2360 torr, with no change in the temperature or moles of gas, what is the new V2? Express your answer with the appropriate units. If the volume of the original sample in Part A (P1 = 472 torr, V1 = 20.0 L) changes to 76.0 L, without a change in the temperature or moles of gas molecules, what is the new pressure, P2? Express your answer with the appropriate units.

Which of the following occupies the largest volume at STP?a. 1.00 g H2b. 1.00 g Hec. 1.00 g Ned. 1.00 g N2e. All of them occupy the same volume

An ideal gas is allowed to expand from 5.40 L to 24.3 Lat constant temperature. By what factor does the volume increase? The pressure will increase by that same factor. decrease by that same factor If the initial pressure was 111 atm, what is the final pressure?

Part AA sample of a gas is in a sealed container. The pressure of the gas is 625 torr, and the temperature is 21 °C. If the temperature changes to 75 °C with no change in volume or amount of gas, what is the new pressure, P2, of the gas inside the container? Express your answer with the appropriate units. Part BUsing the same sample of gas (P1 = 625 torr, T1 = 21 °C), we wish to change the pressure to 6250 torr with no accompanying change in volume or amount of gas. What temperature T2, in Celsius, is needed to reach this pressure? Express your answer with the appropriate units.

A balloon that is 100.21 L at 21 °C and 0.981 atm is released and just barely clears the top of Mount Crumpet in British Columbia. If the final volume of the balloon is 144.53 L at a temperature of 5.24 °C, what is the pressure experienced by the balloon as it clears Mount Crumpet?

A 12 Liter tank contains helium gas pressurized to 160 atm.How many 3-liter balloons could the 12 Liter helium tank fill?(Keep in mind that an "exhausted" helium tank is not empty. In other words, once the gas inside the tank reaches atmospheric pressure, it will no longer be able to fill balloons.)

A hot air balloon is filled with 1.19 x 106 L of an ideal gas on a cool morning (11°C). The air is heated to 129°C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

Assuming all gases are at the same temperature and pressure, how many milliliters of nitrogen gas react to give 47.0 mL of ammonia gas? 3H2(g) + N2(g) → 2NH3 (g). Express your answer with the appropriate units.

An ideal gas is allowed to expand from 7.60 L to 72.2 L at constant temperature. By what factor does the volume increase? The pressure will increase by that same factor. decrease by that same factor. If the initial pressure was 107 atm, what is the final pressure?

A certain mass of nitrogen gas occupies a volume of 5.66 L at a pressure of 8.57 atm. At what pressure will the volume of this sample be 8.04 L? Assume constant temperature and ideal behavior.

A sample of an ideal gas has a volume or 2.25 L at 284 K and 1.13 atm. Calculate the pressure when the volume is 1.83 L and the temperature is 298 K.

A sample of an ideal gas has a volume of 3.40 L at 10.80°C and 1.60 atm. What is the volume of the gas at 22.80°C and 0.997 atm?

A sample of neon gas at 305 K and 0.372 atm occupies a volume of 1.89 L. If the pressure of the gas is increased, while at the same time it is heated to a higher temperature, the final gas volume (a) could be larger or smaller than 1.89 L depending on the final pressure and temperature. (b) will be larger than 1.89 L. (c) will be smaller than 1.89 L.