WGU D425 Intro To Chemistry (latest version)KGO1

Exam questions and highlighted correct answer

1. Which conditions would lead to the largest deviation from ideal gas behavior?

A. 0.01 atm and -50°C

B. 1 atm and 100°C

C. 5 atm and 0°C

D. 2000 atm and 0°C

2. As the temperature of the gas decreases and the pressure increases, which phase change occurs?

A. Condensation

B. Evaporation

C. Compression

D. Expansion

3. Under which conditions would a sample of oxygen gas behave most like an ideal gas?

A. 1 atm and 4500 K

B. 56 atm and 4134 K

C. 120 atm and 700 K

D. 200 atm and 323 K

4. Why do real gases exhibit lower pressures than predicted by ideal gas behavior at low pressure and temperature?

A. Intermolecular attraction is significant.

B. Molecules have finite volume.

C. Molecules are not round.

D. Collisions are more frequent.

5. Given: R = 0.08205 L·atm/(mol·K). What is the required volume of a tank that needs to contain 25.0 moles of N₂ gas at 1.20 atm and 0°C?

A. 159 L

B. 377 L

C. 467 L

D. 505 L

Note: The temperature was unclear in the scan; it was read as 0°C (273.15 K).

6. Given: R = 0.08205 L·atm/(mol·K). A cylinder of 0.75 moles of nitrogen gas currently sits at a temperature of 11°C and 0.247 atm. What is the volume of the cylinder in liters?

A. 0.014 L

B. 2.7 L

C. 17 L

D. 71 L

7. Given: R = 0.08205 L·atm/(mol·K). If a 191 L tank at 301 K contains 9.20 moles of xenon (Xe) gas, what is its pressure in atmospheres?

A. 0.841 atm

B. 1.19 atm

C. 14.5 atm

D. 227 atm

8. The following chemical reaction reaches equilibrium: 2OF₂(g) + 2SO₂(g) ⇌ 2SO₃(g) + F₂(g) + heat. How is the chemical equilibrium affected when the temperature increases?

A. The concentration of the reactants will decrease, while the concentration of the products will increase.

B. The concentrations of both the reactants and the products will not change.

C. The concentrations of both the reactants and the products will increase.

D. The concentration of the reactants will increase, while the concentration of the products will decrease.

Note: The reaction equation was partly garbled in the scan and is shown as it could be read.

9. The decomposition of two units of water vapor (H₂O) to one unit of gaseous oxygen (O₂) and two units of gaseous hydrogen (H₂) is an endothermic reaction: 2H₂O(g) ⇌ O₂(g) + 2H₂(g). If the temperature is decreased, what will happen to the concentrations of the products and the reactants when the system reestablishes its equilibrium?

A. The concentration of the reactants will increase, while the concentration of the products will decrease.

B. The concentration of the reactants will decrease, while the concentration of the products will increase.

C. The concentrations of both the reactants and the products will decrease.

D. The concentrations of the reactants and the products will not change.

10. The reaction between one unit of gaseous iodine (I₂) and one unit of hydrogen gas (H₂) to yield two units of gaseous hydroiodic acid (HI) reaches an equilibrium state: I₂(g) + H₂(g) ⇌ 2HI(g). What is the effect on the products and reactants if the amount of hydrogen (H₂) is increased?

A. The concentration of the reactants will increase, while the concentration of the products will decrease.

B. The concentrations of the reactants and the products will not change.

C. The concentration of the reactants will decrease, while the concentration of the products will increase.

D. The concentrations of both the reactants and the products will decrease.

11. Which equilibrium constant expression represents the following balanced chemical equation? 2NO(g) + O₂(g) ⇌ 2NO₂(g)

K = [NO₂]² / ([NO]²[O₂])

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