Q: A gas mixture contains 72.8% chlorine and 27.2% neon by mass. If the total pressure is 809 mmHg, what is the partial pressure of neon?

$$P_{Ne} = 0.272 \times 809 = 220.85$$ mmHg

Question 1

Which of the following is the correct SI unit for pressure, and after whom is it named?

Accepted Answer

Pascal (Pa), named after Blaise Pascal

Question 2

A gas sample is transferred from a 5.0 L container to a 10.0 L container at constant temperature and amount. What happens to the pressure?

Accepted Answer

It will decrease

Question 3

Which of the following best describes the relationship between pressure and volume for a fixed amount of gas at constant temperature (Boyle's Law)?

Accepted Answer

Inversely proportional

Question 4

According to the Kinetic Molecular Theory, which condition makes a real gas behave most ideally?

Accepted Answer

Low pressure, high temperature

Question 5

A 500 mL container at a pressure of 600 mmHg contains 29.3 g of nitrogen gas at 50 ºC. Which units must be used for the Ideal Gas Law calculation?

Accepted Answer

Pressure in atm, volume in L, temperature in K, n in moles

Question 6

Which of the following statements is TRUE about the kinetic molecular theory?

Accepted Answer

The collisions of particles with one another are completely elastic.

Question 7

A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL, and a temperature of 31 ºC. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25 ºC? (Use the combined gas law.)

Accepted Answer

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

Question 8

Which law explains why the volume of a balloon increases when more gas is added at constant temperature and pressure?

Accepted Answer

Avogadro’s Law

Question 9

A gas mixture contains 72.8% chlorine and 27.2% neon by mass. If the total pressure is 809 mmHg, what is the partial pressure of neon?

Accepted Answer

$$P_{Ne} = 0.272 	imes 809 = 220.85$$ mmHg

Question 10

Which of the following is the correct formula for Dalton’s Law of Partial Pressures using fractional composition?

Accepted Answer

$$P_{Gas} = m_{Gas} \cdot P_{Total}$$

Question 11

A sample of dichloromethane gas (CH$$_2Cl$_2) $$occupies 32.6 L at 310 K and 5.30 atm. What is its volume at STP?

Accepted Answer

$$V_2$$ = $$V_1$$ \frac{$$P_1$$}{$$P_2$$} \frac{$$T_2$$}{$$T_1$$}$$, where P_2$ = 1$$ atm, $$T_2 = 273$ K

Question 12

Which of the following is NOT a postulate of the Kinetic Molecular Theory?

Accepted Answer

The volume of gas particles is significant compared to the container.

Question 13

A 10.0 L cylinder with a movable piston contains 10.0 g of xenon gas. When an additional 10.0 g of xenon gas are added, the volume increases. Which Chemistry Gas Law can be used to justify this result?

Accepted Answer

Avogadro’s Law

Question 14

Which of the following is the correct relationship for the Ideal Gas Law?

Accepted Answer

$$PV = nRT$$

Question 15

A sample of gas initially has a volume of 900 mL at 520 K and 1.85 atm. What is the pressure if the volume decreases to 330 mL while the temperature increases to 770 K?

Accepted Answer

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

Question 16

Which of the following is the correct value for the standard molar volume of an ideal gas at STP?

Accepted Answer

22.4 L

Question 17

The metabolic breakdown of glucose is given by: $$\mathrm{C_6H_{12}O_6$ (s) + 6 O_2$ (g) \rightarrow 6 CO_2$ (g) + 6 H_2O (l)}. If 231.88 g $$glucose is used up at 34 ºC and 1728.9 torr, what is the volume (in mL) of CO$$_2$$ produced?

Accepted Answer

Calculate moles of glucose, use stoichiometry to find moles CO$$_2$$, then use $$PV = nRT to $$solve for $$V.$$

Question 18

Which of the following statements about STP (Standard Temperature and Pressure) is correct?

Accepted Answer

STP is 0 ºC (273 K) and 1 atm.

Study Notes: Gases (Ch.11) – Introductory Chemistry

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