Question 1

A sealed glass container contains partial pressures of 0.80 atm CO₂ gas and 0.35 atm N₂ gas. What is the mole fraction of N₂ in the glass container?

Accepted Answer

The mole fraction of a gas is the ratio of its partial pressure to the total pressure. Total pressure = 0.80 atm + 0.35 atm = 1.15 atm. Mole fraction of N2 = 0.35 atm / 1.15 atm = 0.30.

Question 2

A sealed glass container contains partial pressures of 0.24 atm O₂, 0.45 atm CO₂, 0.64 atm N₂, and 0.46 atm H₂ gas in a 3.5 L container at 30.5°C. What is the total pressure exerted on the walls of the container?

Accepted Answer

The total pressure is the sum of the partial pressures: 0.24 atm + 0.45 atm + 0.64 atm + 0.46 atm = 1.79 atm.

Question 3

A mixture of 5.00 moles of neon and 3.00 moles of nitrogen occupy a volume of 36.0 L in a vessel where the total pressure is 6.00 atm. The partial pressure of the neon in the container is

Accepted Answer

The partial pressure of a gas in a mixture is given by the mole fraction of the gas multiplied by the total pressure. The mole fraction of neon is 5.00 moles / (5.00 moles + 3.00 moles) = 0.625. Therefore, the partial pressure of neon is 0.625 * 6.00 atm = 3.75 atm.

Question 4

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane, C₂H₆, in a 3.50 L container maintained at 35.20 °C?

Accepted Answer

The answer of What is the total pressure exerted by...

Question 5

What is the total pressure exerted by a gaseous mixture that consists of 1.00 g of hydrogen and 8.00 g of neon in a 2.80 L container maintained at 44.10 °C?

Accepted Answer

The answer of What is the total pressure exerted by...

Question 6

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 8.00 g of ethane (C₂H₆)in a 3.50-liter container maintained at 35.20 °C?

Accepted Answer

The answer of What is the total pressure exerted by...

Question 7

What is the mole fraction of methane in a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane (C₂H₆)in a 3.50 L container maintained at 35.20 °C?

Accepted Answer

The answer of What is the mole fraction of methane...

Question 8

A sample of oxygen gas was collected by displacement of water in a gas collection apparatus. The total pressure in the collection vessel was 744.2 torr, the temperature was 26.0 °C, and the vessel contained 522 mL of the collected gas. How many moles of oxygen were collected? (At 26.0 °C, the vapor pressure of water is 25.2 torr.)

Accepted Answer

The pressure of oxygen is the total pressure minus the vapor pressure of water: 744.2 torr - 25.2 torr = 719.0 torr. Convert this to atm: 719.0 torr / 760 torr/atm = 0.945 atm. Use the ideal gas law: PV = nRT, where P = 0.945 atm, V = 0.522 L, R = 0.0821 L·atm/mol·K, and T = 299 K (26.0 °C + 273). Solving for n gives n = (0.945 * 0.522) / (0.0821 * 299) = 0.0201 moles.

Question 9

A sample of hydrogen gas was collected by displacement of water in a large gas buret. The total pressure in the buret was measured as 764.2 torr, the temperature was 23.0 °C, and the buret contained 511 mL of the collected gas. How many moles of hydrogen were collected?(At 23.0 °C, the vapor pressure of water is 21.1 torr.)

Accepted Answer

To find the moles of hydrogen, first subtract the vapor pressure of water from the total pressure to get the pressure of hydrogen: 764.2 torr - 21.1 torr = 743.1 torr. Convert this pressure to atm: 743.1 torr / 760 torr/atm = 0.977 atm. Convert the volume to liters: 511 mL = 0.511 L. Use the ideal gas law: PV = nRT, where R = 0.0821 L·atm/mol·K and T = 23.0 °C = 296.15 K. Solving for n gives n = PV / RT = (0.977 atm)(0.511 L) / (0.0821 L·atm/mol·K)(296.15 K) = 0.0206 moles.

Question 10

A sample of nitrogen gas was collected by displacement of water in a gas collection flask. The total pressure in the collection flask was measured as 754.2 torr, the temperature was 20.0 °C, and the measured volume of gas collected was 516 mL. How many grams should the nitrogen weigh? (At 20.0 °C, the vapor pressure of water is 17.5 torr.)

Accepted Answer

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Question 11

A sample of methane gas (CH₄)was collected by displacement of water in a gas collection flask. The total pressure in the collection flask was measured as 758.2 torr, the temperature was 25.0 °C, and the measured volume of gas in the flask was 526.0 mL. How many grams should the methane weigh? (At 25.0 °C, the vapor pressure of water is 23.8 torr.)

Accepted Answer

The answer of A sample of methane gas (CH₄)was collected...

Question 12

A gas mixture contains 5.00 liters of a mixture of nitrogen gas and oxygen gas. The total pressure in the tank is 38.6 atm when the temperature is 25.0 °C, and the mole fraction of oxygen is 0.400. How much does the oxygen in the tank weigh?

Accepted Answer

The answer of A gas mixture contains 5.00 liters of...

Question 13

A gas mixture is 50.00% helium and 50.00% methane, by volume. What is the mole fraction of methane in the mixture?

Accepted Answer

The answer of A gas mixture is 50.00% helium and...

Question 14

A gaseous substance effuses twice as rapidly as sulfur dioxide gas. The gas could be

Accepted Answer

The answer of A gaseous substance effuses twice as rapidly...

Question 15

The average speed at which a nitrogen molecule effuses at 30.0 °C is 480 meters per second. The average speed at which a butene molecule (C₄H₈)effuses at this same temperature should therefore be

Accepted Answer

The average speed of effusion is inversely proportional to the square root of the molar mass. The molar mass of nitrogen (N2) is 28 g/mol, and for butene (C4H8) it is 56 g/mol. Using the formula v1/v2 = sqrt(M2/M1), we find the speed for butene is approximately 339 m/s.

Question 16

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which krypton gas effuses at this same temperature should therefore be

Accepted Answer

The average speed of a gas molecule is inversely proportional to the square root of its molar mass. Krypton has a higher molar mass than methane, so its effusion speed will be lower. Using the formula for effusion rates, the speed of krypton is approximately 276 m/s.

Question 17

1.000 atm of dry nitrogen, placed in a container having a pinhole opening in its side, leaks from the container 2.28 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of the following species could be the unknown gas?

Accepted Answer

The rate of effusion is inversely proportional to the square root of the molar mass (Graham's law). Since nitrogen effuses 2.28 times faster, the unknown gas must have a molar mass approximately (2.28)^2 times that of nitrogen (28 g/mol), which is about 145 g/mol. SF6 has a molar mass of 146 g/mol, making it the likely candidate.

Question 18

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which an argon molecule effuses at this same temperature should therefore be

Accepted Answer

The answer of The average speed at which a methane...

Question 19

According to the kinetic theory of gases, the average kinetic energy of the gas particles in a gas sample is directly proportional to the

Accepted Answer

The kinetic theory of gases states that the average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas.

Question 20

If container "A"is occupied by 1.00 mole of oxygen gas while container "B"is occupied by 20.0 grams of nitrogen gas and both containers are maintained at 0.00 °C and 650 torr then,

Accepted Answer

The answer of If container "A"is occupied by 1.00 mole...

Quiz 11: Properties of Gases

A sealed glass container contains partial pressures of 0.80 atm CO₂ gas and 0.35 atm N₂ gas. What is the mole fraction of N₂ in the glass container?

A sealed glass container contains partial pressures of 0.24 atm O₂, 0.45 atm CO₂, 0.64 atm N₂, and 0.46 atm H₂ gas in a 3.5 L container at 30.5°C. What is the total pressure exerted on the walls of the container?

A mixture of 5.00 moles of neon and 3.00 moles of nitrogen occupy a volume of 36.0 L in a vessel where the total pressure is 6.00 atm. The partial pressure of the neon in the container is

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane, C₂H₆, in a 3.50 L container maintained at 35.20 °C?

What is the total pressure exerted by a gaseous mixture that consists of 1.00 g of hydrogen and 8.00 g of neon in a 2.80 L container maintained at 44.10 °C?

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 8.00 g of ethane (C₂H₆) in a 3.50-liter container maintained at 35.20 °C?

What is the mole fraction of methane in a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane (C₂H₆) in a 3.50 L container maintained at 35.20 °C?

A gas mixture contains 5.00 liters of a mixture of nitrogen gas and oxygen gas. The total pressure in the tank is 38.6 atm when the temperature is 25.0 °C, and the mole fraction of oxygen is 0.400. How much does the oxygen in the tank weigh?

A gas mixture is 50.00% helium and 50.00% methane, by volume. What is the mole fraction of methane in the mixture?

A gaseous substance effuses twice as rapidly as sulfur dioxide gas. The gas could be

The average speed at which a nitrogen molecule effuses at 30.0 °C is 480 meters per second. The average speed at which a butene molecule (C₄H₈) effuses at this same temperature should therefore be

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which krypton gas effuses at this same temperature should therefore be

1.000 atm of dry nitrogen, placed in a container having a pinhole opening in its side, leaks from the container 2.28 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of the following species could be the unknown gas?

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which an argon molecule effuses at this same temperature should therefore be

According to the kinetic theory of gases, the average kinetic energy of the gas particles in a gas sample is directly proportional to the

If container "A"is occupied by 1.00 mole of oxygen gas while container "B"is occupied by 20.0 grams of nitrogen gas and both containers are maintained at 0.00 °C and 650 torr then,

Quiz 11: Properties of Gases

A sealed glass container contains partial pressures of 0.80 atm CO2 gas and 0.35 atm N2 gas. What is the mole fraction of N2 in the glass container?

A sealed glass container contains partial pressures of 0.24 atm O2, 0.45 atm CO2, 0.64 atm N2, and 0.46 atm H2 gas in a 3.5 L container at 30.5°C. What is the total pressure exerted on the walls of the container?

A mixture of 5.00 moles of neon and 3.00 moles of nitrogen occupy a volume of 36.0 L in a vessel where the total pressure is 6.00 atm. The partial pressure of the neon in the container is

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane, C2H6, in a 3.50 L container maintained at 35.20 °C?

What is the total pressure exerted by a gaseous mixture that consists of 1.00 g of hydrogen and 8.00 g of neon in a 2.80 L container maintained at 44.10 °C?

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 8.00 g of ethane (C2H6) in a 3.50-liter container maintained at 35.20 °C?

What is the mole fraction of methane in a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane (C2H6) in a 3.50 L container maintained at 35.20 °C?

A gas mixture contains 5.00 liters of a mixture of nitrogen gas and oxygen gas. The total pressure in the tank is 38.6 atm when the temperature is 25.0 °C, and the mole fraction of oxygen is 0.400. How much does the oxygen in the tank weigh?

A gas mixture is 50.00% helium and 50.00% methane, by volume. What is the mole fraction of methane in the mixture?

A gaseous substance effuses twice as rapidly as sulfur dioxide gas. The gas could be

The average speed at which a nitrogen molecule effuses at 30.0 °C is 480 meters per second. The average speed at which a butene molecule (C4H8) effuses at this same temperature should therefore be

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which krypton gas effuses at this same temperature should therefore be

1.000 atm of dry nitrogen, placed in a container having a pinhole opening in its side, leaks from the container 2.28 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of the following species could be the unknown gas?

The average speed at which a methane molecule effuses at 28.5 °C is 631 meters per second. The average speed at which an argon molecule effuses at this same temperature should therefore be

According to the kinetic theory of gases, the average kinetic energy of the gas particles in a gas sample is directly proportional to the

If container "A"is occupied by 1.00 mole of oxygen gas while container "B"is occupied by 20.0 grams of nitrogen gas and both containers are maintained at 0.00 °C and 650 torr then,

A sealed glass container contains partial pressures of 0.80 atm CO₂ gas and 0.35 atm N₂ gas. What is the mole fraction of N₂ in the glass container?

A sealed glass container contains partial pressures of 0.24 atm O₂, 0.45 atm CO₂, 0.64 atm N₂, and 0.46 atm H₂ gas in a 3.5 L container at 30.5°C. What is the total pressure exerted on the walls of the container?

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane, C₂H₆, in a 3.50 L container maintained at 35.20 °C?

What is the total pressure exerted by a gaseous mixture that consists of 8.00 g of methane and 8.00 g of ethane (C₂H₆) in a 3.50-liter container maintained at 35.20 °C?

What is the mole fraction of methane in a gaseous mixture that consists of 8.00 g of methane and 12.00 g of ethane (C₂H₆) in a 3.50 L container maintained at 35.20 °C?

The average speed at which a nitrogen molecule effuses at 30.0 °C is 480 meters per second. The average speed at which a butene molecule (C₄H₈) effuses at this same temperature should therefore be