Q: Which of the following is the correct definition of STP in chemistry?

Standard Temperature and Pressure: $$0^\circ \text{C}$$ and $$1\ \text{atm}$$

Question 1

A sample of oxygen gas is collected over water at 25°C. The total pressure in the collection vessel is 755 mmHg, and the vapor pressure of water at 25°C is 24 mmHg. What is the partial pressure of the oxygen gas?

Accepted Answer

$$731\ 	ext{mmHg}$$

Question 2

Which of the following statements best explains why real gases deviate from ideal gas behavior at high pressures?

Accepted Answer

Intermolecular forces between gas particles become significant.

Question 3

A 2.00 L container holds 0.100 mol of nitrogen gas at 27°C. What is the pressure of the gas in atmospheres? (Use $$R = 0.0821\ 	ext{L} \cdot 	ext{atm} / 	ext{mol} \cdot 	ext{K})$$

Accepted Answer

$$1.23\ 	ext{atm}$$

Question 4

Which of the following is NOT a property common to all gases?

Accepted Answer

They have definite shape and volume.

Question 5

A mixture contains 2.0 mol of helium and 3.0 mol of neon in a 10.0 L container at 300 K. If the total pressure is 1.5 atm, what is the partial pressure of neon?

Accepted Answer

$$0.90\ 	ext{atm}$$

Question 6

Which equation correctly represents the Ideal Gas Law?

Accepted Answer

$$PV = nRT$$

Question 7

At STP, what is the volume occupied by 2.00 mol of an ideal gas?

Accepted Answer

$$44.8\ 	ext{L}$$

Question 8

A manometer is used to measure the pressure of a gas sample. If the mercury level is 15 mm higher on the open end than on the gas end, and atmospheric pressure is 760 mmHg, what is the pressure of the gas?

Accepted Answer

$$775\ 	ext{mmHg}$$

Question 9

According to the Kinetic Molecular Theory, which of the following statements is true?

Accepted Answer

Gas particles are in constant, random motion.

Question 10

A 5.00 L container holds a mixture of gases: 1.00 mol of O$$_2$$, 2.00 mol of N$$_2$$, and 1.00 mol of CO$$_2 at 300 K. $$What is the mole fraction of N$$_2 in $$the mixture?

Accepted Answer

$$0.40$$

Question 11

Which of the following best describes the effect of increasing temperature on the average velocity of gas molecules?

Accepted Answer

The average velocity increases.

Question 12

A 10.0 L tank contains 4.00 mol of hydrogen gas at 300 K. What is the pressure in the tank? (Use $$R = 0.0821\ 	ext{L} \cdot 	ext{atm} / 	ext{mol} \cdot 	ext{K})$$

Accepted Answer

$$9.85\ 	ext{atm}$$

Question 13

Which of the following is a correct statement of Dalton’s Law of Partial Pressures?

Accepted Answer

The total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas.

Question 14

Which of the following best explains why helium is used in deep-sea diving tanks instead of nitrogen?

Accepted Answer

Helium is less soluble in blood than nitrogen, reducing the risk of decompression sickness.

Question 15

A gas sample has a volume of 500 mL at 1.00 atm and 273 K. What will be its volume at 2.00 atm and 273 K?

Accepted Answer

$$250\ 	ext{mL}$$

Question 16

Which of the following is the correct definition of STP in chemistry?

Accepted Answer

Standard Temperature and Pressure: $$0^\circ 	ext{C}$$ and $$1\ 	ext{atm}$$

Question 17

A real gas will behave most ideally under which of the following conditions?

Accepted Answer

High temperature and low pressure

Question 18

A 1.00 L flask contains 0.50 mol of argon and 0.50 mol of neon at 300 K. If the total pressure is 24.6 atm, what is the mole percent of argon?

Accepted Answer

$$50\%$$

Question 19

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

Pressure is inversely proportional to volume.

Question 20

A scuba tank contains air at a pressure of 200 atm at 27°C. If the tank is left in the sun and the temperature rises to 47°C, what is the new pressure in the tank? (Assume volume is constant.)

Accepted Answer

$$213\ 	ext{atm}$$

Properties and Behavior of Gases

Study Guide - Practice Questions

Study Guide - Flashcards