Question 1

Which of the following best describes an ideal gas according to the kinetic molecular theory?

Accepted Answer

A gas in which molecules are far apart and do not interact with each other.

Question 2

Which equation correctly represents the ideal gas law?

Accepted Answer

$$PV = nRT$$

Question 3

A sample of gas occupies 2.0 L at 1.0 atm and 300 K. If the pressure is increased to 2.0 atm and the temperature is decreased to 150 K, what will be the new volume of the gas? (Assume the amount of gas is constant.)

Accepted Answer

$$V_2 = 0.5$$\ \mathrm{L}$$

Question 4

Which of the following statements about the law of conservation of mass is correct?

Accepted Answer

The total mass of reactants equals the total mass of products in a chemical reaction.

Question 5

A barometer uses mercury to measure atmospheric pressure. If the density of mercury is $$13.6\ \mathrm{g/cm^3$}$$, what is the pressure exerted by a $$76\ \mathrm{cm}$$ column of mercury? (Use $$g = 9.8\ \mathrm{m/s^2$}$$ and $$1\ \mathrm{atm} = 101325\ \mathrm{Pa})$$

Accepted Answer

$$P = 1.01\ \mathrm{atm}$$

Question 6

Which of the following is the correct SI unit for pressure?

Accepted Answer

N/m$$^2$$

Question 7

If you mix 2.0 moles of helium and 3.0 moles of neon in a container at constant temperature and volume, what is the total pressure exerted by the mixture?

Accepted Answer

The total pressure is equal to the sum of the partial pressures of helium and neon.

Question 8

Which formula would you use to calculate the force exerted by a gas on the walls of its container?

Accepted Answer

$$F = P 	imes A$$

Question 9

During inhalation, the volume of your lungs increases. According to Boyle's Law, what happens to the pressure inside your lungs if the amount of air and temperature remain constant?

Accepted Answer

The pressure inside your lungs decreases.

Question 10

Which of the following is the correct value for the gas constant $$R in $$units of $$\mathrm{L \cdot atm/(mol \cdot K)}$$?

Accepted Answer

$$R = 0.08206$$

Question 11

A firefighter needs to pump water from a lake up a mountain. If the density of water is $$1.00\ \mathrm{g/cm^3$}$$, how tall would the column of water need to be to exert the same pressure as a $$76\ \mathrm{cm}$$ column of mercury?

Accepted Answer

$$h_{water} = 1034\ \mathrm{cm}$$

Question 12

Which of the following is NOT an assumption of the ideal gas law?

Accepted Answer

Gas molecules lose energy when they collide.

Question 13

If the pressure exerted by a liquid in a barometer is given by $$P = g \cdot d \cdot h$$, which variable would you change to increase the pressure reading?

Accepted Answer

Increase the height $$h of $$the liquid column.

Question 14

Which of the following best explains why gases are often considered ideal in laboratory settings?

Accepted Answer

Because gas molecules are far apart and interact weakly.

Question 15

A sealed container holds 1.0 mol of gas at 2.0 atm and 300 K. If the temperature is doubled and the volume remains constant, what is the new pressure?

Accepted Answer

$$P_2 = 4.0$$\ \mathrm{atm}$$

Question 16

Which of the following is a consequence of molecular motion in gases?

Accepted Answer

Pressure exerted by the gas on the walls of its container.

Question 17

Which of the following is the correct relationship for Newton's Law as applied to the mass of mercury in a barometer?

Accepted Answer

$$F = g \cdot m$$

Question 18

If the volume of a gas is doubled while the temperature and amount of gas remain constant, what happens to the pressure?

Accepted Answer

The pressure is halved.

Question 19

Which of the following is a real-world example of the law of conservation of mass?

Accepted Answer

The total mass of reactants and products in a chemical reaction remains unchanged.

General Chemistry I: Gases and Energetics – Study Notes

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