Q: Which conversion factor would you use to convert moles of gas to volume at STP?

$$1\ \text{mole gas} = 22.4\ \text{L}$$

Question 1

A sample of nitrogen gas occupies 2.50 L at 1.00 atm and 300 K. If the pressure is increased to 2.00 atm and the temperature is decreased to 273 K, what will be the new volume of the gas? (Assume the number of moles remains constant.)

Accepted Answer

1.14 L

Question 2

A weather balloon contains 44 L of helium at 2.0 moles. If 3.0 moles of helium are added, what is the final volume of the balloon? (Assume temperature and pressure are constant.)

Accepted Answer

110 L

Question 3

Which of the following statements best describes Avogadro’s Law?

Accepted Answer

The volume of a gas is directly proportional to the number of moles, when temperature and pressure are constant.

Question 4

At STP, what is the volume occupied by 4.0 moles of methane ($$\mathrm{CH_4$}$$)?

Accepted Answer

89.6 L

Question 5

A scuba tank contains a mixture of helium and oxygen at a total pressure of 8.00 atm. If the partial pressure of oxygen is 1280 mmHg, what is the partial pressure of helium in atm? (1 atm = 760 mmHg)

Accepted Answer

6.32 atm

Question 6

Which equation represents the Combined Gas Law?

Accepted Answer

$$\frac{P_1$ V_1$}{T_1$} = \frac{P_2$ V_2$}{T_2$}$$

Question 7

A 0.180 L sample of helium gas at 0.800 atm and 29°C is compressed to 90.0 mL and 3.20 atm. What is the final temperature in °C? (Use the Combined Gas Law.)

Accepted Answer

60°C

Question 8

Which of the following is NOT a condition of STP?

Accepted Answer

Pressure of 2 atm

Question 9

A mixture of gases contains 2.0 atm of nitrogen, 1.0 atm of oxygen, and 0.5 atm of argon. What is the total pressure according to Dalton’s Law?

Accepted Answer

3.5 atm

Question 10

If you have 3.0 moles of a gas at STP, what volume will it occupy?

Accepted Answer

67.2 L

Question 11

A gas sample is transferred from a 1.00 L container at 2.00 atm and 300 K to a 2.00 L container at 1.00 atm. What is the final temperature, assuming the number of moles is constant?

Accepted Answer

600 K

Question 12

Which of the following best explains why the total pressure of a gas mixture is the sum of the partial pressures of each gas?

Accepted Answer

Each gas behaves independently and contributes to the total pressure through its own collisions.

Question 13

A hospital oxygen tank contains 5.0 moles of oxygen at STP. What is the volume of oxygen in the tank?

Accepted Answer

112 L

Question 14

If the number of moles of a gas is doubled at constant temperature and pressure, what happens to the volume?

Accepted Answer

The volume doubles.

Question 15

A gas mixture contains 400 mmHg of nitrogen, 300 mmHg of oxygen, and 100 mmHg of carbon dioxide. What is the total pressure in atm?

Accepted Answer

1.05 atm

Question 16

Which conversion factor would you use to convert moles of gas to volume at STP?

Accepted Answer

$$1\ 	ext{mole gas} = 22.4\ 	ext{L}$$

Question 17

A sample of gas has a volume of 500 mL at 1.00 atm and 273 K. If the temperature is increased to 546 K and the pressure is decreased to 0.50 atm, what is the new volume?

Accepted Answer

2000 mL

Question 18

Which law would you use to determine the effect of adding more moles of gas to a container at constant temperature and pressure?

Accepted Answer

Avogadro’s Law

Question 19

A mixture of gases in a medical ventilator contains 0.8 atm of oxygen and 0.2 atm of carbon dioxide. What is the total pressure?

Accepted Answer

1.0 atm

Question 20

A sample of argon gas is compressed from 3.0 L at 1.0 atm and 300 K to 1.0 L at 3.0 atm. What is the final temperature?

Accepted Answer

300 K

Gas Laws: Combined, Avogadro’s, STP, and Dalton’s Law

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