In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under **Standard State conditions**.

Concept #1: Understanding Standard State Conditions

Concept #2: Standard Molar Volume

At **STP**, **1 mole** of any ideal gas will occupy exactly **22.4 Liters** of volume inside a container.

Knowing the meaning of STP allows you to now further manipulate the Ideal Gas Law.

Concept #3: Combined Gas Law

Practice: What volume will 5.72 x 10^{25} atoms of argon gas occupy at STP?

Concept #4: Using the Ideal Gas Law to find density or molar mass

The Ideal Gas Law can be further manipulated into new equations. These new equations can help us find the density or molar mass of a gas.

When calculating the density of a gas it is essentially to also recall the formula of that gas in order to find the molar mass, M.

Practice: What is the density of chlorine gas at STP?

Remember that units for molar mass are grams of compound divided by the moles of that compound.

Practice: An unknown gas sample weighs 3.12 g. If it has a volume of 0.206 µL when the temperature is 45^{o}C and the pressure is 957 torr. What is its molar mass?

Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?
A. 1.00 L
B. 2.00 L
C. 5.6 L
D. 11.2 L
E. 22.4 L

What is the volume occupied at STP by a mixture of 4.00 g of He(g), 2.00 g of H2(g) and 32.0 g of O2(g)?
A. 6.15 L
B. 11.2 L
C. 22.4 L
D. 44.8 L
E. 67.2 L

What volume will 3.12 grams of helium occupy at STP?

Which of the following gases has the highest density at STP?
A. sulfur trioxide, SO 3
B. carbon dioxide
C. NO 2
D. argon
E. nitrogen

How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)
a) 11.6
b) 2.32
c) 4.64
d) 52.0
e) 104

What volume will 0.780 moles of Xe occupy at STP?

For the combustion of sucrose, C12H22O11, shown below:
a) How many moles of oxygen are required to react with 1.00g of sucrose?
C12H22O11 + 12O2 → 12CO2 + 11H2O
b) If the CO2 produced from the combustion of 1.00g of sucrose is trapped in a balloon, what volume will it occupy at STP?

A sample of N2 gas occupies a volume of 746 mL at STP. What volume would N 2 gas occupy at 155°C at a pressure of 368 torr?
1. 983 mL
2. 566 mL
3. 3295 mL
4. 312 mL
5. 588 mL
6. 323 mL
7. 2415 mL
8. 1792 mL

Which gas sample has the greatest volume at STP?
a. 5g Ar
b. 5g Rn
c. 5g Ne
d. 5g Kr
e. 5g Xe

Determine the theoretical yield of K 2CO3 when 0.392 moles of KO 2 react with 29.0 L CO2 (at STP – 0°C, 1 atm). The molar mass of KO 2 = 71.10 g/mol and K 2CO3 = 138.21 g/mol.
4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g)
a. 27.1 g
b. 179 g
c. 91.7 g
d. 206 g
e. 61.0 g

At STP what volume of N 2 will react completely with 22.2 L H 2 to produce NH3?
N2(g) + 3H2 (g) → 2NH 3 (g)
a. 7.4 L
b. 14.8 L
c. 22.2 L
d. 44.4 L
e. 66.6 L

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.

Determine the volume of O2 (at STP) formed when 50.0 g of KClO 3 decomposes according to the following reaction.
2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)
A) 8.22 L
B) 9.14 L
C) 14.6 L
D) 12.3 L
E) 13.7 L

The action of some commercial drain cleaners is based on the following reaction:
2 NaOH (s) + 2 Al (s) + 6 H2O (l) → 2 NaAl(OH)4 (s) + 3 H 2 (g)
What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?
A) 8.59 L
B) 3.50 L
C) 5.25 L
D) 7.87 L

Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction:
2 NaN3(s) → 2Na(s) + 3 N2(g)
If an automobile air bag has a volume of 11.8 L, what mass of NaN 3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.

Lithium reacts with nitrogen gas according to the reaction:
6 Li(s) + N2(g) → 2 Li3N(s)
What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation:
CH4(g) + H2O(g) → CO(g) + 3 H2(g)
In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

An ideal gas occupies 49.0 L at 994 torr and 41.0°C.
What volume would it occupy at STP?
1. 0.0136 L
2. 73.7 L
3. 55.7 L
4. 58.7 L
5. 105 L
6. 39.1 L
7. 69.9 L
8. 0.0179 L
9. 22.4 L

If a reaction occurs in the gas phase at STP, we can determine the
mass of a product from the volumes of reactants. Explain.

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl.Determine the percent composition of the substance.

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl.Calculate its empirical formula.

You may want to reference (Pages 407 - 410)Section 10.5 while completing this problem.What is the molar mass of an unknown hydrocarbon whose density is measured to be 1.97 g/L at STP?

A gaseous hydrogen and carbon containing compound is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, was found to be 0.646 g.What is the molecular formula of the compound?

If 6.00
mol of an ideal gas at STP were confined to a cube, what would be the
length in cm of an edge of this cube?

You may want to reference (Pages 212 - 215) Section 5.5 while completing this problem.Use the molar volume of a gas at STP to calculate the density (in g/L) of carbon dioxide gas at STP.

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.
You may want to reference (Pages 404 - 407) Section 10.4 while completing this problem.What volume would the gas occupy at STP?

You may want to reference (Pages 410 - 412)Section 10.6 while completing this problem.A 4.0-L vessel containing N2 at STP and a 2.0-L vessel containing H2 at STP are connected by a valve. If the valve is opened allowing the two gases to mix, what is the mole fraction of hydrogen in the mixture?

Suppose you have two 1-L flasks, one containing N2 at STP and the other containing CH4 at STP.
You may want to reference (Pages 415 - 419)Section 10.8 while completing this problem.How do these systems compare with respect to the number of molecules?

Suppose you have two 1-L flasks, one containing N2 at STP and the other containing CH4 at STP.
You may want to reference (Pages 415 - 419)Section 10.8 while completing this problem.How do these systems compare with respect to density?

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 30.1 g of neon at STP.

Define molar volume for a gas at STP.

Give molar volume value for a gas at STP.

What is the molar volume of an ideal gas at STP?

One mole of nitrogen and one mole of neon are combined in a closed container at STP.How big is the container?

A gas sample at STP contains 1.26 g oxygen and 1.76 g nitrogen.
You may want to reference (Page 215) Section 5.6 while completing this problem.What is the volume of the gas sample?

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.
You may want to reference (Pages 404 - 407) Section 10.4 while completing this problem.What volume will the Cl2 occupy at STP?

Consider the following gases, all at STP: Ne, SF6, N2, CH4.Which one is closest to an ideal gas in its behavior?

Comparison of molar volumes at STP.Which gas deviates most from ideal behavior?

Consider the following gases, all at STP: Ne, SF6, N2, CH4.Which one has the highest total molecular volume relative to the space occupied by the gas?

You may want to reference (Page 211) Section 5.5 while completing this problem.Rank the gases Ar, N2, CH4, and C2H6 in order of increasing density at STP.

The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?1. 87.8 g2. There is not enough information to solve.3. 44.8 g4. 0.0875 g5. 43.9 g6. 0.510 g

Methane, CH4(g), reacts with steam to give synthesis gas, a mixture of carbon monoxide and hydrogen.
CH4 (g) + H2O(g) → CO(g) + H2(g) [unbalanced]
What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas?

Consider three 1-L flasks at STP. Flask A contains NH 3 gas, flask B contains NO2 gas, and flask C contains N2 gas. In which flask are the molecules least polar and therefore most ideal in behavior?

The density of a gas is 1.43 g/L at STP. Calculate its density under a pressure of 743 torr and 26°C

A gas has a density of 3.214 g/L at 728 torr and 24°C. What would be its density at STP?

One mole of nitrogen and one mole of neon are combined in a closed container at STP.
How big is the container?

What volume will 40.0 L of He at 50.00°C and 1201 torr occupy at STP?A. 26.7 LB. 18.6 LC. 12.8 LD. 53.4 LE. 31.1 L

Calculate the density of nitrogen gas at STP.A. 0.625 g/LB. 1.25 g/LC. 6.83 g/LD. 13.7 g/LE. Cannot be calculated with this information (undefined)

A balloon filled with helium occupies 20.0 L at 1.50 atm and 25°C. How many moles of helium will there be in the balloon at STP?A. 22.4 molesB. 1.12 molesC. 0.0446 molesD. 0.893 molesE. 1.23 molesF. 4.55 moles

If 250 mL of a gas at STP weighs 2 g, what is the molar mass of the gas?A. 179 g • mol-1B. 8.00 g • mol-1C. 56.0 g • mol-1D. 28.0 g • mol-1E. 44.8 g • mol-1

Find out the volume contained by 6.8 g of ammonia at STP. (N=14, H=1)

Which gas sample has the greatest volume at STP?a. 20g of Neb. 2g of H2c. 8g of Hed. 20 g of N2

Consider the following gas phase reaction:2NO(g) + O2(g) → 2NO2(g)400. mL of NO at STP is reacted with 500. mL of O2 at STP. Calculate the volume of the reaction mixture at STP after the reaction goes to completion.a. 700 mLb. 800 mLc. 900 mLd. 1300 mLe. 100 mL

If sufficient acid is used to react completely with 21.0 grams of Mg
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
what volume of hydrogen at STP would be produced?
1. 9.68 liters
2. 19.37 liters
3. 10.60 liters
4. 22.40 liters
5. 4.84 liters

A hypothetical rock was harvested from another planet. Trapped inside was a diatomic gas. A volume of 1.25 mL of the gas was extracted from the rock at STP. The mass of the gas sample was determined to be 2.12 mg. Identify the gas.1. oxygen2. None of these3. hydrogen4. nitrogen5. fluorine

Standard conditions (STP) is defined as1. 273.15 K, 760 torr.2. 0 K, 250 atm.3. 100 K, 1 torr.4. 273.15 K, 250 torr.5. 0 K, 1 atm.

A sample of helium (He) occupies 4 liters at STP. What pressure is necessary to change the volume to 2 liters at 20°C?
1. 2.1464 atm
2. 2.0 atm
3. 2.36 atm
4. 4.361 atm
5. 4.0 atm

Assuming ideal behavior, what is the density of argon gas at STP, in g/L?a) 0.0176 g/Lb) 0.0250 g/Lc) 1.63 g/Ld) 1.78 g/Le) 181. g/L

A 574cm3 volume of Na2CO3 solution was warmed with an excess of sulfuric acid until all action ceased. A 9.0 L volume of dry CO2 gas measured at STP was given off and collected. What was the molarity of the sodium carbonate solution?a) 0.30b) 0.40c) 0.50d) 0.60e) 0.70

Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

What is the density of Xe gas at STP? Give your result in g/L.a. 0.00156b. 64.0c. 5.86d. 5.37e. 0.178

A mixture of hydrogen and helium is 25.0% hydrogen by mass. What is the partial pressure of hydrogen (in atm) in the mixture at STP?a) 0.460b) 0.399c) 0.520d) 0.250e) 0.380

Which of the following gases has the greatest density at STP?A) NO2 (molar mass = 46.01 g/mol)B) Xe (molar mass = 131.3 g/mol)C) SO2 (molar mass = 64.07 g/mol)D) SF6 (molar mass = 146.07 g/mol)E) All of these samples have the same density at STP.

Which of the following samples will have the greatest volume at STP?a. 22 g Neb. 22 g Hec. 22 g O2d. 22 g Cl2 e. All have the same V at STP

Arrange the following gases in order of decreasing density at STP. Rank from largest to smallest.F2O2Cl2Ne

Using the graph below, determine the gas that has the lowest density at STP.A) AB) BC) CD) DE) All of the gases have the same density at STP.

Use the molar volume of a gas at STP to calculate the density (in g/L) of nitrogen gas at STP.

If the density of a gas 1.43 g/L at STP, what is the molecular weight of the gas?

Which of the following samples has the greatest density at STP?a. SO2b. Arc. SF6d. NOe. He

Which of the following gases has the largest density at STP?a. Heb. C2H2 c. F2d. N2e. H2

Consider the following diagram:Container A (with porous walls) is filled with air at STP. It is then inserted into a large enclosed container (B), which is then flushed with H2(g). What will happen to the pressure inside container A? Explain your answer.

Dilute aqueous hydrogen peroxide is used as a bleaching agent and for disinfecting surfaces and small cuts. Its concentration is sometimes given as a certain number of “volumes hydrogen peroxide,” which refers to the number of volumes of O2 gas, measured at STP, that a given volume of hydrogen peroxide solution will release when it decomposes to O2 and liquid H2O. How many grams of hydrogen peroxide are in 0.100 L of “20 volumes hydrogen peroxide” solution?

Consider the following reaction:4Al(s) + 3O2(g) → 2Al2O3(s)It takes 2.00 L of pure oxygen gas at STP to react completely with a certain sample of aluminum. What is the mass of aluminum reacted?

You may want to reference (Pages 223 - 223) Section 5.7 while completing this problem.Lithium reacts with nitrogen gas according to the following reaction: 6Li(s) + N2(g) → 2Li3N(s)6 m Li(s) + N_2 (g) ightarrow 2 m Li_3N(s)What mass of lithium is required to react completely with 57.6 mL of N2 gas at STP?

When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced.
What volume of H2(g) is produced when 6.2g of Al(s) reacts at STP?

Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction.2 NaN3(s) → 2Na(s) + 3 N2 (g)If an automobile air bag has a volume of 11.8 L , what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation:CH4(g) + H2O(g) → CO(g) + 3 H2 (g)In a particular reaction, 26.0 L of methane gas (measured at a pressure of 734 torr and a temperature of 25 oC) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 oC). The reaction produces 26.6 L of hydrogen gas measured at STP.What is the percent yield of the reaction?

You may want to reference (Pages 223 - 223) Section 5.7 while completing this problem.Hydrogen and oxygen combine to form H2O via the following reaction:2H2(g) + O2(g) → 2H2O(g)How many liters of oxygen (at STP) are required to form 12.6 g of H2O?

Combustible vapor-air mixtures are flammable over a limited range of concentrations. The minimum volume % of vapor that gives a combustible mixture is called the lower flammable limit (LFL). Generally, the LFL is about half the stoichiometric mixture, which is the concentration required for complete combustion of the vapor in air. (b) What volume (in mL) of n-hexane (d = 0.660 g/cm3) is required to produce a flammable mixture of hexane in 1.000 m3 of air at STP?

Radon (Rn) is the heaviest, and only radioactive, member of Group 8A(18) (noble gases). It is a product of the disintegration of heavier radioactive nuclei found in minute concentrations in many common rocks used for building and construction. In recent years, there has been growing concern about the cancers caused from inhaled residential radon. If 1.0x1015 atoms of radium (Ra) produce an average of 1.373x104 atoms of Rn per second, how many liters of Rn, measured at STP, are produced per day by 1.0 g of Ra?

How many grams of phosphorus react with 35.5 L of O 2 at STP to form tetraphosphorus decoxide?P4(s) + 5O2(g) ⟶P4O10(s)

How many grams of potassium chlorate decompose to potassium chloride and 638 mL of O2 at 128°C and 752 torr?2KClO3(s) ⟶2KCl(s) + 3O2(g)

How many grams of phosphine (PH 3) can form when 37.5 g of phosphorus and 83.0 L of hydrogen gas react at STP?P4(s) + H2(g) ⟶PH3(g) [unbalanced]

When 35.6 L of ammonia and 40.5 L of oxygen gas at STP burn, nitrogen monoxide and water form. After the products return to STP, how many grams of nitrogen monoxide are present? NH 3(g) + O2(g) ⟶NO(g) + H2O(l) [unbalanced]

What volume of O2 at STP is required to oxidize 8.0 L of NO at STP to NO2? What volume of NO2 is produced at STP?

Consider the following questions: (a) What is the total volume of the CO2(g) and H2O(g) at 600 °C and 0.888 atm produced by the combustion of 1.00 L of C2H6(g) measured at STP?

Roasting galena [lead(II) sulfide] is a step in the industrial isolation of lead. How many liters of sulfur dioxide, measured at STP, are produced by the reaction of 3.75 kg of galena with 228 L of oxygen gas at 220°C and 2.0 atm? Lead(II) oxide also forms.

Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction:2NaN3(s) → 2Na(s) + 3N2(g)What mass of NaN3(s) must be reacted to inflate an air bag to 70.0 L at STP?

Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions:3C2H4 + 2 H2SO4 ⟶ C2H5HSO4 + (C2H5)2SO4 C2H5HSO4 + (C2H5)2SO4 + 3 H2O ⟶ 3 C2H5OH + 2 H2SO4What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?

An unknown diatomic gas has a density of 3.164 g/L at STP. What is the identity of the gas?

The density of a certain gaseous fluoride of phosphorus is 3.93 g/L at STP. Calculate the molar mass of this fluoride and determine its molecular formula.

An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g CO2 and 0.0991 g H2O. A sample of 0.4831 g of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129). At STP, 27.6 mL of dry N2 was obtained. In a third experiment, the density of the compound as a gas was found to be 4.02 g/L at 127°C and 256 torr. What are the empirical and molecular formulas of the compound?

At STP, 1.0 L Br2 reacts completely with 3.0 L F2, producing 2.0 L of a product. What is the formula of the product? (All substances are gases.)

A 2.50-L sample of a colorless gas at STP decomposed to give 2.50 L of N2 and 1.25 L of O2 at STP. What is the colorless gas?

Cyclopropane, a gas that when mixed with oxygen is used as a general anesthetic, is composed of 85.7% C and 14.3% H by mass. If the density of cyclopropane is 1.88 g/L at STP, what is the molecular formula of cyclopropane?

To derive the ideal-gas equation, we assume that the volume
of the gas atoms/molecules can be neglected.Given the
atomic radius of neon, 0.69 Å , and knowing that a sphere has a volume of 4/3 πr3, calculate the fraction of space that Ne{
m Ne} atoms occupy in a sample of neon at STP.

A student adds 4.00 g of dry ice (solid CO2) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous CO2)?

The effect of chlorofluorocarbons (such as CCl2F2) on the depletion of the ozone layer is well known. The use of substitutes, such as CH3CH2F(g), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP: (a) CCl2F2(g)

The effect of chlorofluorocarbons (such as CCl2F2) on the depletion of the ozone layer is well known. The use of substitutes, such as CH3CH2F(g), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:(b) CH3CH2F(g)

Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?

An aerosol spray can with a volume of 250 mL contains 2.30 g of propane gas (C3H8) as a propellant.You may want to reference (Pages 404 - 407) Section 10.4 while completing this problem.What volume would the propane occupy at STP?

A mixture of 0.200 g of H2, 1.00 g of N2, and 0.820 g of Ar is stored in a closed container at STP. Find the volume of the container, assuming that the gases exhibit ideal behavior.

A sample of Freon-12 (CF2Cl2) occupies 25.5 L at 298 K and 153.3 kPa. Find its volume at STP.

What is the density of Xe gas at STP?

How many moles of gaseous arsine (AsH 3) occupy 0.0400 L at STP? What is the density of gaseous arsine?

A 1-L sample of CO initially at STP is heated to 546 K, and its volume is increased to 2 L. (a) What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall?

A liter of methane gas, CH4, at STP contains more atoms of hydrogen than does a liter of pure hydrogen gas, H2, at STP. Using Avogadro’s law as a starting point, explain why.

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions?b. The temperature is decreased to -50°C.

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions?c. The volume is decreased to 0.5 L.

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions?d. The number of moles of neon is doubled.

A sample of oxygen gas has a volume of 2.50 L at STP. How many grams of O2 are present?

Calculate the volume of 63.5 g of carbon monoxide at STP. Report your answer to one decimal place!

If the density of an ideal gas at STP if found to be 0.716 g/L, what is its molar mass?

A sample of carbon dioxide gas (CO2) has a volume of 2.5 L at standard temperature and pressure (STP). How many molecules of carbon dioxide gas are in the sample?

An open flask sitting in a lab fridge looks empty, but we know that actually it is filled with a mixture of gases called air. If the flask volume is 1.50L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain?

Be sure to answer all parts.How many moles of gaseous arsine (AsH3) occupy 0.273 L at STP? What is the density of gaseous arsine?

Enter your answer in the provided box.A sample of Freon-12(CF2Cl2) occupies 10.0 L at 293 K and 128.00 kPa. Find its volume at STP.

Calculate the volume occupied by 56.5 g of argon gas at STP. 22.4 L 31.7 L 34.6 L 1, 270 L 1, 380 L