Question 1

A scuba diver descends to a depth where the pressure is 3.0 atm. If the diver's air tank initially contains 12.0 L of air at 1.0 atm, what will be the volume of air available to the diver at the new depth, assuming temperature remains constant? (Use Boyle's Law: $$P_1V_1 = P_2V_2)$$

Accepted Answer

$$4.0\ \mathrm{L}$$

Question 2

Which of the following statements best describes Charles’ Law?

Accepted Answer

At constant pressure, the volume of a gas is directly proportional to its absolute temperature.

Question 3

A balloon filled with helium has a volume of $$2.5\ \mathrm{L} at$$ $$25^\circ\mathrm{C}. If $$the temperature increases to $$50^\circ\mathrm{C} at $$constant pressure, what is the new volume? (Use Charles’ Law: $$\frac{V_1$}{T_1$} = \frac{V_2$}{T_2$}$$, temperatures in Kelvin)

Accepted Answer

$$2.8\ \mathrm{L}$$

Question 4

Which equation correctly represents Gay-Lussac’s Law?

Accepted Answer

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

Question 5

A gas at $$2.0\ \mathrm{atm}$$ and $$300\ \mathrm{K} is $$heated to $$600\ \mathrm{K} at $$constant volume. What is the final pressure? (Use Gay-Lussac’s Law: $$\frac{P_1$}{T_1$} = \frac{P_2$}{T_2$})$$

Accepted Answer

$$4.0\ \mathrm{atm}$$

Question 6

Which of the following is the correct form of the Combined Gas Law?

Accepted Answer

$$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$}$$

Question 7

A sample of gas occupies $$5.0\ \mathrm{L} at$$ $$1.0\ \mathrm{atm}$$ and $$273\ \mathrm{K}. $$What will be its volume at $$2.0\ \mathrm{atm}$$ and $$546\ \mathrm{K}$$? (Use the Combined Gas Law: $$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$})$$

Accepted Answer

$$5.0\ \mathrm{L}$$

Question 8

According to Avogadro’s Law, which of the following is true?

Accepted Answer

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

Question 9

A $$2.0\ \mathrm{L}$$ container holds $$0.10\ \mathrm{mol} of $$oxygen gas at STP. If the amount of oxygen is doubled, what will be the new volume, assuming temperature and pressure remain constant? (Use Avogadro’s Law: $$\frac{V_1$}{n_1$} = \frac{V_2$}{n_2$})$$

Accepted Answer

$$4.0\ \mathrm{L}$$

Question 10

A medical oxygen tank contains $$10.0\ \mathrm{L} of $$gas at $$200\ \mathrm{atm}$$ and $$300\ \mathrm{K}. If $$the gas is released into a room at $$1.0\ \mathrm{atm}$$ and $$300\ \mathrm{K}$$, what volume will it occupy? (Use Boyle’s Law: $$P_1V_1 = P_2V_2)$$

Accepted Answer

$$2000\ \mathrm{L}$$

Question 11

Which of the following scenarios best illustrates the application of Charles’ Law in everyday life?

Accepted Answer

A car tire expands in volume on a hot day.

Question 12

A gas sample at $$1.0\ \mathrm{atm}$$ and $$273\ \mathrm{K}$$ has a volume of $$22.4\ \mathrm{L}. If $$the temperature is increased to $$546\ \mathrm{K}$$ and the pressure is doubled, what is the new volume? (Use the Combined Gas Law: $$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$})$$

Accepted Answer

$$22.4\ \mathrm{L}$$

Question 13

Which of the following is NOT an assumption of the empirical gas laws?

Accepted Answer

Gas molecules are always in liquid state.

Question 14

A $$3.0\ \mathrm{L}$$ sample of nitrogen gas at $$2.0\ \mathrm{atm}$$ and $$300\ \mathrm{K} is $$transferred to a $$6.0\ \mathrm{L}$$ container at $$400\ \mathrm{K}. $$What is the new pressure? (Use the Combined Gas Law: $$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$})$$

Accepted Answer

$$0.75\ \mathrm{atm}$$

Question 15

If the pressure of a gas is doubled while its temperature is kept constant, what happens to its volume according to Boyle’s Law?

Accepted Answer

The volume is halved.

Question 16

A $$1.0\ \mathrm{mol}$$ sample of gas at STP occupies $$22.4\ \mathrm{L}. If$$ $$0.5\ \mathrm{mol} of $$the same gas is measured at STP, what volume will it occupy? (Use Avogadro’s Law)

Accepted Answer

$$11.2\ \mathrm{L}$$

Question 17

Which gas law would you use to determine the final pressure of a gas when both its volume and temperature change?

Accepted Answer

Combined Gas Law

Question 18

A weather balloon is filled with $$100.0\ \mathrm{L} of $$helium at $$1.0\ \mathrm{atm}$$ and $$300\ \mathrm{K}. As it $$rises, the pressure drops to $$0.5\ \mathrm{atm}$$ and the temperature drops to $$250\ \mathrm{K}. $$What is the new volume? (Use the Combined Gas Law: $$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$})$$

Accepted Answer

$$240\ \mathrm{L}$$

Empirical Gas Laws: Fundamental Principles and Calculations

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