Q: Convert a pressure of 132 psi to mmHg. (1 atm = 14.7 psi, 1 atm = 760 mmHg)

$132 \text{ psi} \times \frac{1 \text{ atm}}{14.7 \text{ psi}} \times \frac{760 \text{ mmHg}}{1 \text{ atm}} = 6,824 \text{ mmHg}$

Q: Which formula represents Boyle's Law?

$V_1 \times P_1 = V_2 \times P_2$

Q: A sample of gas occupies 2.0 L at 1.0 atm. If the pressure is increased to 4.0 atm at constant temperature, what is the new volume?

$V_2 = \frac{V_1 \times P_1}{P_2} = \frac{2.0 \text{ L} \times 1.0 \text{ atm}}{4.0 \text{ atm}} = 0.5 \text{ L}$

Q: A balloon is moved from an ice water bath (0°C) to a boiling water bath (100°C) at constant pressure. If its initial volume is 1.0 L, what is its final volume? (Use Kelvin for temperature)

$V_2 = V_1 \times \frac{T_2}{T_1} = 1.0 \text{ L} \times \frac{373 \text{ K}}{273 \text{ K}} = 1.37 \text{ L}$

Q: If 0.5 moles of a gas occupy 10.0 L at constant temperature and pressure, how many liters will 2.0 moles occupy?

$V_2 = V_1 \times \frac{n_2}{n_1} = 10.0 \text{ L} \times \frac{2.0}{0.5} = 40.0 \text{ L}$

Question 1

Which of the following statements best explains why atmospheric pressure decreases with increasing altitude?

Accepted Answer

The number of gas particles in a given volume decreases as altitude increases.

Question 2

A barometer is used to measure atmospheric pressure. If the atmospheric pressure is 760 mmHg, what is the height of the mercury column in the barometer?

Accepted Answer

760 mm

Question 3

Which equation correctly relates pressure, force, and area for a gas?

Accepted Answer

$P = \frac{F}{A}$

Question 4

A manometer is used to measure the pressure of a gas sample. If the mercury level on the left side of the tube is higher than the right, what does this indicate?

Accepted Answer

The gas pressure is less than the atmospheric pressure.

Question 5

Convert a pressure of 132 psi to mmHg. (1 atm = 14.7 psi, 1 atm = 760 mmHg)

Accepted Answer

$132 	ext{ psi} 	imes \frac{1 	ext{ atm}}{14.7 	ext{ psi}} 	imes \frac{760 	ext{ mmHg}}{1 	ext{ atm}} = 6,824 	ext{ mmHg}$

Question 6

According to Boyle's Law, what happens to the volume of a gas if the pressure is doubled at constant temperature?

Accepted Answer

The volume is halved.

Question 7

Which formula represents Boyle's Law?

Accepted Answer

$V_1 	imes P_1 = V_2 	imes P_2$

Question 8

A sample of gas occupies 2.0 L at 1.0 atm. If the pressure is increased to 4.0 atm at constant temperature, what is the new volume?

Accepted Answer

$V_2 = \frac{V_1 	imes P_1}{P_2} = \frac{2.0 	ext{ L} 	imes 1.0 	ext{ atm}}{4.0 	ext{ atm}} = 0.5 	ext{ L}$

Question 9

According to Charles's Law, what happens to the volume of a gas when the temperature is increased at constant pressure?

Accepted Answer

The volume increases.

Question 10

Which equation correctly represents Charles's Law?

Accepted Answer

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

Question 11

A balloon is moved from an ice water bath (0°C) to a boiling water bath (100°C) at constant pressure. If its initial volume is 1.0 L, what is its final volume? (Use Kelvin for temperature)

Accepted Answer

$V_2 = V_1 	imes \frac{T_2}{T_1} = 1.0 	ext{ L} 	imes \frac{373 	ext{ K}}{273 	ext{ K}} = 1.37 	ext{ L}$

Question 12

Avogadro's Law states that the volume of a gas is directly proportional to the number of moles at constant temperature and pressure. Which equation represents this law?

Accepted Answer

$\frac{V_1}{n_1} = \frac{V_2}{n_2}$

Question 13

If 0.5 moles of a gas occupy 10.0 L at constant temperature and pressure, how many liters will 2.0 moles occupy?

Accepted Answer

$V_2 = V_1 	imes \frac{n_2}{n_1} = 10.0 	ext{ L} 	imes \frac{2.0}{0.5} = 40.0 	ext{ L}$

Question 14

Which of the following is NOT a basic property described by the simple gas laws?

Accepted Answer

Density (D)

Question 15

Which pressure unit is equivalent to 1 atm?

Accepted Answer

101,325 Pa

Question 16

A gas sample in a rigid container is heated from 300 K to 600 K. What happens to the pressure, assuming the amount and volume remain constant?

Accepted Answer

The pressure doubles.

Question 17

Which of the following best describes the molecular interpretation of Boyle's Law?

Accepted Answer

As the volume decreases, gas molecules collide with the container walls more frequently, increasing pressure.

Question 18

Which of the following is a correct statement about the relationship between pressure and particle density in a gas?

Accepted Answer

Higher particle density results in higher pressure.

Gases: Properties, Laws, and Molecular Interpretation

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