Ch.5 - GasesSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Jules Bruno

The Simple Gas Laws represent theories and equations that try to relate together pressure, temperature, volume and the amount of a gas when discussing their chemical properties and behaviors. 


Boyle’s Law

Boyle’s Law, also known as Mariotte’s Law, the Boyle-Mariotte Law or Pressure-Volume Law, states that pressure (P) and volume (V) are inversely proportionally, which basically means they are opposites of one another, at constant moles (n) and temperature (T).

This pressure-volume relationship is commonly displayed in the following example of a closed container. Pressure represents the downward force applied to the container while volume represents the free space within it.

Robert-Boyle-Inverse-RelationshipBoyle's Law (Volume & Pressure)

When plotting this inverse pressure-volume relationship onto a chart you obtain the following: 

PV-Plot-Isothermal-ProcessPressure-Volume Plot

The inverse relationship between pressure and volume at a constant mass for a gas at a fixed temperature is illustrated by the expression: 

Volume-Pressure-Inverse-relationshipVolume & Pressure (Inverse Relationship)

Boyle’s Law Formula

The Ideal Gas Law is presented as: 

Ideal-Gas-Law-universal-gas-constant-0.0821-PV/T-P1V1/T1-P2V2/T2Ideal Gas Law

If moles (n) and temperature (T) are held constant then the formula simplifies into: 

Pressure-Volume-ConstantBoyle's Law (PV = Constant)

When dealing with two sets of data (2 pressures and 2 volumes) the Boyle’s Law formula becomes: 

P1V1-P2V2-Boyles-Law-FormulaBoyle's Law Formula (P1V1 = P2V2)

Now let’s use it in a practice problem. 

PRACTICE: If an unknown gas were confined within a 5.15 L container at 3.20 atm, what would be the pressure if the volume were expanded to 11.23 L? 

STEP 1: Identify the variables given. 

Boyles-Law-VariablesBoyle's Law (Identifying Variables)

STEP 2: Isolate the missing variable for the second pressure (P2). 

Boyle's-Law-P2Boyle's Law (Solving for P2)

Charles’ Law

Charles Law, also known as the Temperature-Volume Law, states that volume (V) and temperature (T) are directly proportionally as long as pressure (P) and moles (n) are held constant. This temperature-volume relationship is commonly displayed by the application and removal of heat from a closed container with a moveable piston. 

Charles-Law-Volume-Temperature-Jacques-CharlesCharles' Law (Volume & Temperature)

Being directly proportional means that as the temperature increases then the volume would also increase. This direct temperature-volume relationship can be plotted onto a chart and provide the following: 

Volume-Temperature-PlotTemperature-Volume Plot

The direct relationship between temperature and volume at constant moles and pressure is illustrated by the expression: 

Volume-Temperature-Direct-RelationshipVolume & Temperature (Direct Relationship)

Charles’ Law Formula

By rearranging the Ideal Gas Law we can isolate V and T: 

Derived-Charles-LawDerived Formula (Charles' Law)

If moles (n) and pressure (P) are held constant then the formula simplifies into: 

V/T-C-Charles-LawCharles' Law (V/T = Constant)

Incorporating the two sets of data (2 volumes, 2 temperatures) produces the Charles’ Law formula as: 

Charles' Law Formula (V1 / T1 = V2 / T2)

PRACTICE: If a 2.2 L container filled with gas at a temperature of 18.0 °C is heated to a temperature of 38.0 °C, what is the new volume of the container (in liters)?

STEP 1: Identify the variables given. 

Charles-Law-VariablesCharles' Law (Identifying Variables)

STEP 2: Gas behavior is examined under absolute temperature conditions and so we must convert all temperatures from Celsius to Kelvin. 

Charles-Law-Temperature-ConversionsTemperature Conversions (T1 & T2)

STEP 3: Plug the given values into Charles’ Law formula.

Charles-Law-Solving-V2Charles' Law (Plugging in values)

STEP 4: Perform cross-multiplication between the two ratios. 

Charles-Law-Cross-MultiplicationCharles' Law (Cross Multiplication)

STEP 5: Isolate the missing variable for the second volume (V2). 

Charles' Law (Solving for V2)

Avogadro’s Law

Avogadro’s Law, also known as the Mole-Volume Law or Volume Amount Law, states that volume (V) and moles (n) are directly proportional as long as pressure (P) and temperature (T) are held constant. This mole-volume relationship is depicted with the addition or removal of gas molecules from a closed container with a moveable piston. 

Avogadro's Law (Moles & Volume)

As more and more gas molecules are pumped into the container they push up against the moveable piston and thereby increase the volume inside the container. This direct mole-volume relationship can be plotted onto a chart and provide the following:

Moles-Volume-PlotMoles-Volume Plot

The direct relationship between the number of moles and volume at constant temperature and pressure is illustrated by the expression: 

Volume-moles-Direct-RelationshipVolume & moles (Direct Relationship)

Avogadro’s Law Formula

By rearranging the Ideal Gas Law we can isolate V and n: 

Avogadro-Law-Derived-FormulaDerived Formula (Avogadro's Law)

If temperature (T) and pressure (P) are held constant then the formula simplifies into: 

Avogadro-Law-V/n-constantAvogadro's Law (V/n = Constant)

Incorporating the two sets of data (2 volumes, 2 moles) produces the Avogadro’s Law formula as: 

Avogadro-Law-V1n1-V2n2Avogadro's Law (V1/n1 = V2/n2)

PRACTICE: How many moles will a sample of F2 gas occupy in a 2.50 L container, if 3.21 moles of F2 have a volume of 53.2 L?

STEP 1: Identify the variables given. 

Avogadro-Law-VariablesAvogadro's Law (Identifying Variables)

STEP 2: Plug the given values into Avogadro’s Law formula. 

Avogadro-Law-Plugging-in-VariablesAvogadro's Law (Plugging in values)

STEP 3: Perform cross-multiplication between the two ratios. 

Avogadro-Law-Cross-MultiplicationAvogadro's Law (Cross Multiplication)

STEP 4: Isolate the missing variable for the second moles (n2). 

Avogadro's Law (Solving for n2)

Gay-Lussac’s Law

This sometimes overlooked simple gas law, because it doesn’t involve a changing volume like the previous 3, states that pressure (P) and temperature (T) are directly proportional as long as volume (V) and moles (n) are held constant. This pressure-temperature relationship is depicted with the addition or removal of heat from a rigid, non-flexible container. 

Gay-Lussac-Law-Amedeo-AvogadroGay-Lussac's Law (Pressure & Temperature)

By increasing the temperature of a container the gas molecules will absorb the excess thermal energy and convert it into kinetic energy. With higher kinetic energies, the gas molecules will move faster and hit the walls of the container more frequently and with harder force. This in term leads to a higher overall pressure within the container. 


This direct pressure-temperature relationship can be plotted onto a chart and provide the following:

Pressure-Temperature-PlotPressure-Temperature Plot

The direct relationship between the pressure and temperature at constant volume and moles of gas is illustrated by the expression: 

Pressure-Temperature-direct-relationshipPressure & Temperature (Direct Relationship)

Gay-Lussac’s Law Formula

By rearranging the Ideal Gas Law we can isolate P and T: 

Derived-Formula-Gay-LussacDerived Formula (Gay-Lussac's Law)

If volume (V) and moles of gas (n) are held constant then the formula simplifies into: 

Gay-Lussac-ConstantGay-Lussac's Law (P/T = Constant)

Incorporating the two sets of data (2 pressures, 2 temperatures) produces the Gay-Lussac’s Law formula as: 

Gay-Lussac's Law Formula (P1/T1 = P2/T2)

PRACTICE: If an unknown gas possesses a pressure of 800 mmHg when the temperature is 20 °C, what would be its pressure (in mmHg) when the temperature is increased to 110 °C

STEP 1: Identify the variables given. 

Gay-Lussac's Law (Identifying Variables)

STEP 2: Convert the Celsius values into Kelvin. 

Gay-Lussac-Temperature-ConversionsAvogadro's Law (Temperature Conversions)

STEP 3: Plug the given variables into the Gay-Lussac’s Law Formula. 

Gay-Lussac-Plugging-in-VariablesGay-Lussac's Law Formula (Plugging in values)

STEP 4: Perform cross-multiplication between the two ratios. 

Gay-Lussac-Cross-MultiplicationGay-Lussac's Law (Cross Multiplication)

STEP 5: Isolate the missing variable for the second pressure (P2). 

Avogadro's Law (Solving for P2)

By combining the Simple Gas Laws we are able to create the Ideal Gas Law and the Combined Gas Law. Through these equations we can examine gas behaviors as well as their properties dealing with molar masspartial pressure, density, effusionspeed and velocity


Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.


Additional Problems
Into a 500.0 L container at 18°C are placed 0.40 g of H 2, 20.0 g CO 2 and 14.0 g of O2. What is the partial pressure of H 2?
A mixture of He and O 2 is placed in a 4.00 L flask at 32°C. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4atm. What is the mole fraction of O 2? a. 0.224 b. 0.341 c. 0.481 d. 0.518 e. 0.659
What is the pressure in atm exerted by a mixture of 1.00 g H 2 and 5.00 g He when the mixture is contained in a volume of 5.00 L at 20.0°C? a) 8.4 b) 7.84 c) 28.8 d) 0.574 e) 7.71   What is the partial pressure in atm exerted by the H 2 in the gaseous mixture described in the previous question? a) no given answer is close b) 0.115 c) 2.4 d) 5.76 e) 1.54
If the pressure exerted by ozone, O 3, in the stratosphere is 3.0 x 10 -3 atm and the temperature is 255 K, how many ozone molecules are in one liter? a. 6.0 x 1018 b. 6.1 x 10 22 c. 8.6 x 1019 d. 1.4 x 1018 e. 2.7 x 10 20
A 55.0 L gas cylinder containing NO and 3.238 mol of N 2 has a total pressure of 2.14 atm at 303 K. What is the mole fraction of NO? A)  4.729               B) 0.683          C) 0.0467           D) 1.491            E) 0.316
A 355 mL container holds 0.146 g of Ne gas and an unknown amount of Ar gas at 35°C, and a total pressure of 626 mmHg. Calculate the number of moles of Ar gas present. a) 7.24 x 10 –3 mol Ar b) 4.34 x 10 –3 mol Ar c) 4.27 x 10 −3 mol Ar d) 1.00 x 10 −2 mol Ar e) 5.79 x 10 −3 mol Ar
What is the volume occupied by 12.5 g of argon gas at a pressure of 1.05 atm and a temperature of 322 K? Would the volume be different if the sample were 12.5 g of helium (under identical conditions)? 
Assume the ideal gas constant, R, has a value of .08206 (L * atm)/(mol * K). Convert this value into expressions for R in terms of J/(mol* K), (cubic meters * Pa)/(mol * K), (L * bar)/(mol * K), and J/(molecule * K).
A 118-mL flask is evacuated and found to have a mass of 97.129 g. When the flask is filled with 768 torr of helium gas at 35 °C, it has a mass of 97.171 g. Was the helium gas pure? 
Calculate the volume occupied by 0.845 mol of nitrogen gas at a pressure of 1.37 atm and a temperature of 315 K.Given: n = 0.845 mol, P = 1.37 atm, T = 315 KFind: V
A 1.00 L flask is filled with 1.05 g of argon at 25 °C . A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm. What is the partial pressure of argon, PAr , in the flask? What is the partial pressure of ethane, Pethane, in the flask?
Samples containing equal numbers of moles of H 2, N2, O2, and He are placed into separate 1 L containers at the same temperature. Assuming each gas behaves ideally, which container has the highest pressure?a. H2b. N2c. O2d. Hee. All the gases would all exhibit the same pressure.
A 750.0 mL metal bulb is filled with 0.421 g of CH 4 and an unknown mass of NH 3. If the total pressure in the bulb is 3.77 atm at 315°C, then how much NH3 is also in the bulb?1. 2.39 grams2. 0.00713 grams3. 0.549 grams4. 14.5 grams5. 1.17 grams6. 0.996 grams7. 0.0323 grams
A 1.00 L flask is filled with 1.00 g of argon at 25°C. A sample of ethane vapor is added to the same flask until the total pressure is 1.250atm . Part A What is the partial pressure of argon, PAr, in the flask? Express your answer to three significant figures and include the appropriate units. PAr = _________________ PART B What is the partial pressure of ethane, Pethane, in the flask? Express your answer to three significant figures and include the appropriate UNITS. Pethane =_________________
How many moles of O2 will be present in a 3.00 L sample of the gas collected at 25°C and 0.900 atm?1. 0.110 mol2. 0.134 mol3. 83.9 mol4. 9.06 mol5. 1.32 mol
The chemical reaction N2(g) + 3H2(g) → 2NH3(g) is carried out below:20.0L N2 5.0L H210.0 atm 5.0 atma. When the stopcock between the two reaction vessels is opened, the reaction proceeds. Calculate the partial pressure of NH3 after the reaction is complete. Assume 100% yield for the reaction and that the temperature is constant.b.What will be the effect on the volume of an ideal gas if both the pressure is increased 10 fold and the absolute temperature is doubled?
A 10-liter container is filled with 0.10 mol of H2(g) and heated to 3000 K causing some of the H2(g) to decompose into H(g). The pressure is found to be 3.0 atm. Find the partial pressure of the H(g) that foms from H2 at this temperature. (Assume two significant figures for the temperature.) 
A balloon is filled with SF6 gas at 22°C to a volume of 2.50 liters and has a pressure inside equal to 1.25atm. Molar mass of SF6 is 146.06 g/mol.a. What is the mass of SF6 in the balloon?b. Calculate the density of the SF6 in the balloon?c. How many molecules of SF6 are in the balloon?
What pressure will 14.0 g of CO exert in a 3.5 L container at 75 degrees Celsius?
A sample of sodium azide (NaN 3), a compound used in automobile air bags was thermally decomposed and 15.3 mL of nitrogen gas was collected at 25°C and 755 torr. How many grams of nitrogen were collected? a. 16.85b. 12.8c. 0.0174d. 0.0168e. 6.21 x 10 -4
A 750.0 mL metal bulb is filled with 0.421 g of CH 4 and an unknown mass of NH 3. If the total pressure in the bulb is 3.77 atm at 315ºC, then how much NH3 is also in the bulb?1. 0.0323 grams2. 2.39 grams3. 14.5 grams4. 1.17 grams5. 0.549 grams6. 0.996 grams7. 0.00713 grams
Consider a gas in a container with an initial pressure, temperature and volume. What will happen to the pressure of the gas if the number of moles are quadrupled, the volume is tripled and the temperature is increased 5 times?A. the pressure will increase by 12 timesB. the pressure will increase by 6.7 timesC. the pressure will remain inchangedD. the pressure will increase by 2.4 timesE. the pressure will increase by 3.8 times
A 1.00 L flask is filled with 1.20g of argon at 25°C. A sample of ethane vapor is added to the same flask until the total pressure is 1.400atm .a. What is the partial pressure of argon, PAr, in the flask?b. What is the partial pressure of ethane, Pethane, in the flask?
Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65°C and contains 0.482 g of hydrogen and 4.98 g of oxyen. What is the partial pressure of oxygen in the flask?a. 33.5 atmb. 0.557 atmc. 67 atmd. 1.11 atme. 0.043 atm
A 40.2 L constant volume cylinder containing 2.21 mol He is heated until the pressure reaches 4.20 atm. What is the final temperature?A) 658 KB) 1074 KC) 804 KD) 931 KE) 258 K
Calculate the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg   (R = 0.08206 L•atm•K-1•mol-1, 1 atm = 760 mmHg).a. 0.263 gb. 35.2 gc. 2.46 gd. 3.80 ge. 206 g
What is the pressure in a 15.0-L cylinder filled with 32.7 g of oxygen gas at a temperature of 302 K? 
What is the temperature of 0.52 mol of gas at a pressure of 1.3 atm and a volume of 11.8 L? 
How many moles of CO are contained in a 5.00 L tank at 155 °C and at 2.80 atm?
Into a 5.00 L container at 18oC are placed 0.200 mol H2, 20.0 g CO2, and 14.00 g O2. Calculate the total pressure in the container and the partial pressure of each gas.
Pressurized carbon dioxide inflators can be used to inflate a bicycle tire in the event of a flat. These inflators use metal cartridges that contain 16.0 g of carbon dioxide. At 298 K, to what pressure (in psi) can the carbon dioxide in the cartridge inflate a 3.45-L mountain bike tire? (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.) 
What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?A) 1.1 atmB) 2.3 atmC) 4.1 atmD) 6.4 atmE) 5.0 atm
What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K?
A 1.20-g sample of dry ice is added to a 755-mL flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas) and the mixture returns to 25.0 °C. What is the total pressure in the flask? 
The air in a bicycle tire is bubbled through water and collected at 25 °C. If the total volume of gas collected is 5.45 L at a temperature of 25°C and a pressure of 745 torr, how many moles of gas were in the bicycle tire?
The zinc within a copper-plated penny will dissolve in hydrochloric acid if the copper coating is filed down in several spots (so that the hydrochloric acid can get to the zinc). The reaction between the acid and the zinc is 2 H+(aq) + Zn(s) → H2(g)+Zn2+(aq). When the zinc in a certain penny dissolves, the total volume of gas collected over water at 25 °C was 0.951 L at a total pressure of 748 mmHg. What mass of hydrogen gas was collected?   
How many moles of CO are contained in a 5.00 L tank at 155 °C and 2.80 atm? a. 0.399 moles b. 1.10 moles c. 0.455 moles d. 0.289 moles e. 2.51 moles
For each of the items written below, state why it is wrong and write a version that is correct. What’s wrong?Write a correct version.  
What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25oC?
When 5.91 grams of hydrogen gas (H2) is contained in 3.75 liters at a temperature of -10.0°C, the measured pressure will be...
Hyperbaric therapy uses 100% oxygen at pressure to help heal wounds and infections, and to treat carbon monoxide poisoning. A hyperbaric chamber has a volume of 1430 L. How many kilograms of O2 gas are needed to give an oxygen pressure of 3.14 atm at 25°C? 
A 7.35-L container holds a mixture of two gases at 17°C. The partial pressures of gas A and gas B, respectively, are 0.168 atm and 0.630 atm. If 0.170 mol of a third gas is added with no change in volume or temperature, what will the total pressure become? 
A 0.203 g sample of carbon dioxide, CO2, has a volume of 564 mL and a pressure of 453 mmHg.What is the temperature of the gas in kelvins? Express your answer to three significant figures.What is the temperature of the gas in degrees Celsius? Express your answer to three significant figures.
The nitrogen gas in an automobile air bag, with a volume of 60. L, exerts a pressure of 858 mm Hg at 25 degree C. What amount of N_2 gas (in moles) is in the air bag?
A sample of a gas mixture contains the following quantities of three gases. The sample has: volume = 2.50 L temperature = 16.6 degree C. What is the partial pressure for each gas, in mmHg? What is the total pressure in the flask?
A. A balloon is floating around outside your window. The temperature outside is 13 ° C, and the air pressure is 0.700 atm. Your neighbor, who released the balloon, tells you that he filled it with 4.50 moles of gas. What is the volume of gas inside this balloon? Express your answer to three significant figures and include the appropriate units.B. A 18.0 L gas cylinder is filled with 8.00 moles of gas. The tank is stored at 49 ° C. What is the pressure in the tank? Express your answer to three significant figures and include the appropriate units.C. A 240. L kiln is used for vitrifying ceramics. It is currently operating at 1335 °C, and the pressure is 1.075 atm. How many moles of air molecules are within the confines of the kiln? Express your answer to three significant figures and include the appropriate units.
Dry ice is solid carbon dioxide, A 1.33-g sample of dry ice is placed in an evacuated 4.33 - L vessel at 21.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.
If 60.5 moles of an ideal gas is at 9.89 atm at 47.00 °C, what is the volume of the gas? 
What is the pressure in a 18.6 L cylinder filled with 20.4 g of oxygen gas at a temperature of 333 K? Express your answer with the appropriate units.
What volume is occupied by 21 g of methane (CH4) at 27°C and 1.25 atm?a. 0Lb. not enough data to calculatec. 2.3199999999999998 Ld. 37.2 L e. 25.800000000000001 L 
A sample of carbon dioxide is contained in a 125.0 mL flask at 0.973 atm and 19.0°C. How many molecules of gas are in the sample?
Enter your answer in the provided box.Given that 8.33 moles of carbon monoxide gas are present in a container of volume 26.10 L, what is the pressure of the gas (in atm) if the temperature is 47°C?
A sample of carbon dioxide is contained in a 125.0 mL flask at 0.943 atm 17.4 degree C. How many molecules of gas are in the sample?
How many grams of helium are contained in a 2.0 L balloon at 30.0 ° C and at 735 mmHg?a. 66.1 gb. 26.5 gc. 0.477 gd. 0.312 g
A 2.45-L flexible flask at 15 C contains a mixture of N2, He, and Ne at partial pressures of 0.283 atm for N2, 0.151 atm for He, and 0.425 atm for Ne. (a) Calculate the total pressure of the mixture. atm (b) Calculate the volume in liters at STP occupied by He and Ne if the N2 is removed selectively. L
In the metallurgical process of refining nickel, the metal is first combined with carbon monoxide to form tetracarbonylnickel. which is a gas at 43°C:Ni(s) + 4CO(g) → Ni(CO)4(g)This reaction separates nickel from other solid impurities. Starting with 67.4 g of Ni, calculate the pressure of Ni(CO)4 in a container of volume 5.95 L. (Assume the above reaction goes to completion.)
A 50.0 L tank contains nitrogen gas at a pressure of 50.0 psi at 22°C. How many grams of nitrogen gas are in the tank? Do not include the units in your submitted answer.
A sample of helium gas collected at a pressure of 0.976 atm and a temperature of 24.0°C is found to occupy a volume of 21.2 liters. How many moles of He gas are in the sample?
An 8.85 L tire contains 0.525 mol of gas at a temperature of 319 K. What is the pressure (in atm) of the gas in the tire? Express your answer with the appropriate units.
Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2NaN3 (s) → 2Na (s) + 3N2 (g) Calculate the value of work, w, for the following system if 33.2 g of NaN3 reacts completely at 1.00 atm and 22 °C.
0.976 mol sample of helium gas at a temperature of 24.0°C is found to occupy a volume of 21.2 liters. The pressure of this gas sample is ___ mm Hg.
For 2SO2 (g) + O2 (g) ⇌ 2SO3 (g), Kp = 3.0 x 10 4 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.18 g of SO3 and 0.107 g of O2. How many grams of SO2 are in the vessel?Express your answer using two significant figures.
At a certain temperature and pressure, one liter of CO2 gas weighs 1.15 g. What is the mass of one liter of CH4 gas at the same temperature and pressure? 
What is the temperature of 0.43 mol of gas at a pressure of 1.0 atm and a volume of 11.7 L?Express your answer using two significant figures. 
An automobile tire has a maximum rating of 38.0 psi (gauge pressure). Part AThe tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi at a temperature of 120°C. While driving on a hot day the tire warms to 65.0°C and its volume expands to 12.2 L. What is the pressure in the tire after warming on a hot day? Express your answer in pound-force per square inch to 3 significant figures. 
If an 100 mL light bulb contains 0.20 grams of argon gas and 0.1 grams of nitrogen gas at 30.0 °C, what is the total pressure (atm) of the mixture of gases? (a) None of the above (b) 2.13 atm (c) 0.213 atm (d) 0.211 atm
If 2.69 moles of an ideal gas has a pressure of 1.12 atm, and a volume of 49.85 L, what is the temperature of the sample in degrees Celsius?
What pressure is exherted by 0.350 moles of carbon dioxide gas in a 2.25 L flask at 94.0 C? a. 57.1b. 0.213c. 4.69d. 475 e. 1.20
How many grams of CO2 are contained in 550 mL of the gas at STP? a. 1.08 g b. 0.28 g c. 1080 gd. 0.56 g e. 0.125 g
If an ideal gas has a pressure of 3.61 atm, a temperature of 52.50°C, and has a volume of 79.31 L, how many moles of gas are in the sample? 
A 5.00 L flask contains 3.50 g of sulfur trioxide, 2.45 g of carbon monoxide, and 3.99 g of argon all at 35 °C. What is the pressure (in atm) in the flask?
A 1.40 g sample of CO2 is contained in a 696 mL flask at 20.6°C. What is the pressure of the gas?
What volume is occupied by 0.968 mol of CO2 at 274.7 K and 743 mmHg?
If an ideal gas has a pressure of 2.93 atm, a temperature of 46.46oC  and has a volume of 62.65 L, how many moles of gas are in the sample?
A sample of oxygen was collected over water at 25°C and 0.852 atm. If the total sample volume was 2.950 L, how many moles of O2 were collected? 
A 8.20-L container holds a mixture of two gases at 31° C. The partial pressures of gas A and gas B, respectively, are 0.327 atm and 0.546 atm. If 0.100 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?
Enter your answer in thr provided box.What is the volume of 5.37 moles of an ideal gas at 35.5°C and 1.00 atm?
If 6.01 moles of an ideal gas has a pressure of 1.43 atm, and a volume of 22.81 L, what is the temperature the sample? 
If 7.72 motes of an ideal gas has a pressure of 2.78 atm, and a volume of 33.67 L, what is the temperature of the sample in degrees Celsius? 
Enter your answer in the provided box.Given that 5.31 moles of carbon monoxide gas are present in a container of volume 12.10 L, what is the pressure of the gas (in atm) if the temperature is 55 °C?
At what temperature do 0.026695 mol of Ne in a 893.7 mL container exert a pressure of 0.90 atm? 
lf 88.5 mol of an ideal gas occupies 86.5 L at 17.00 °C, what is the pressure of the gas? 
Carbon monoxide gas is collected at 31.0°C in an evacuated flask with a measured volume of 10.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.050 atm. Calculate the mass and number of moles of carbon monoxide gas that were collected. Round your answer to 2 significant digits. 
A weather balloon is inflated to a volume of 30.0 L at a pressure of 742 mmHg and a temperature of 29.9°C. The balloon rises in the atmosphere to an altitude where the pressure is 380. mmHg and the temperature is -13.6°C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.
A 9.40-L container holds a mixture of two gases at 15°C. The partial pressures of gas A and gas B. respectively, are 0.327 atm and 0.665 atm. If 0.210 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?
A sample of argon gas collected at a pressure of 0.702 atm and a temperature of 291 K is found to occupy a volume of 653 millimeters. How many moles of Ar gas are in the sample?
If 75.5 mol of an ideal gas occupies 88.5 L at 71.00 °C, what is the pressure of the gas?
A sample of xenon gas collected at a pressure of 1.50 atm and a temperature of 275 K is found to occupy a volume of 860. Milliliters. How moles of Xe gas are in the sample? 
At what temperature will 2.55 mole of an ideal gas in a 1.30 L container exert a pressure of 1.10 atm?
Part AIf the pressure exerted by ozone, O3. In the stratosphere is 3.0 x 10-3 atm and the temperature is 251 K, how many ozone molecules are in a liter? Express your answer using two significant figures. 
Part Athe volume, in liters, occupied by 1.70 moles of N2 gas V = _______ LPart B the number of moles of CO2 in 3.80 L of CO2 gas v = _______ mol
If 29.5 mol of an ideal gas occupies 13.5 L at 79.00°C, what is the pressure of the gas? 
A 22.4 L high pressure reaction vessel is charged with 0.3910 mol of iron powder and 1.20 atm of oxygen gas at standard temperature. On heating, the iron and oxygen react according to the balanced reaction below. 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) After the reaction vessel is cooled, and assuming the reaction goes to completion, what pressure of oxygen remains?
To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 1.1-L bulb, then filled it with the gas at 1.90 atm and 24.0°C and weighed it again. The difference in mass was 2.3 g. Identify the gas. Express your answer as a chemical formula.
A sample of argon gas at STP occupies 34.0 L. What mass of argon is present in the 
Calcium carbonate, CaCO3(s), decomposes upon heating to give CaO(s) and CO2(g). A sample of CaCO3 is decomposed, and the carbon dioxide is collected in a sealed 250 mL flask. After the decomposition is complete, the gas has a pressure of 1.6 atm at a temperature of 31 °C. How many moles of CO2 gas were generated? (Ideal gas equation: PV = nRT.)
If an ideal gas has a pressure of 4.29 atm, a temperature of 457 K, and has a volume of 60.27 L, how many moles of gas are in the sample?
How many grams of CO2 are contained in 550 mL of the gas at STP? a. 1.08g b. 0.28 g c. 1080 g d. 0.56 g e. 0.125 g
lf 8.28 moles of an ideal gas has a pressure of 1.57 atm, and a volume of 87.35 L, what is the temperature of the sample in degrees Celsius?
Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25oC and 1.0 atm. R = 0.08206 Latm/molK0.0186 L4.5 L11.2 L48.2 L53.7 L
Enetr your answer in the provided box.A sample of nitrogen gas in a 2.7-L container at a temperature of 17°C exerts a pressure of 5.1 atm. Calculate the number of moles of gas in the sample.
If 4.33 moles of an ideal gas has a pressure of 3.14 atm, and a volume of 76.85 L, what is the temperature of the sample in degrees Celsius?  
An environmental chemist sampling industrial exhaust gases from a coal-burning plant collects a CO2-SO2-H2O mixture in a 21.0-L steel tank until the pressure reaches 821.2 torr at 46.0°C. How many moles of gas are collected? ____________ mol gas If the SO2 concentration in the mixture is 1.57 x 103 parts per million by volume (ppmv), what is its partial pressure? ___________ torr 
A sample of an ideal gas has a volume of 3.60 L at 14.40 C and 1.80 atm. What is the volume of the gas at 24.20°C and 0.988 atm?
If 3.63 moles of an ideal gas has a pressure of 1.25 atm, and a volume of 77.29 L. What is the temperature of the sample in degrees Celsius? 
If an ideal gas has a pressure of 6.07 atm, a temperature of 10.42 °C, and has a volume of 69.83 L how many moles of gas are in the sample?