Question 1

A reaction vessel contains the following equilibrium: $$\mathrm{N_2$(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)}. If $$the volume of the vessel is suddenly decreased at constant temperature, what will happen to the position of equilibrium?

Accepted Answer

The equilibrium will shift to the right, favoring the formation of $$\mathrm{NH_3$(g)}.$$

Question 2

For the reaction $$\mathrm{2SO_2(g) + O_2$(g) \rightleftharpoons 2SO_3(g)}$$, what is the effect of increasing the pressure by decreasing the volume?

Accepted Answer

The equilibrium shifts to the right, producing more $$\mathrm{SO_3$(g)}.$$

Question 3

Consider the reaction $$\mathrm{C_2H_4(g) + Cl_2$(g) \rightleftharpoons C_2H_4Cl_2(g)}$$ ($$\Delta H \u003c 0). $$What will happen to the equilibrium concentrations of $$\mathrm{C_2H_4}$$ and $$\mathrm{C_2H_4Cl_2} if $$the pressure is increased by compressing the system?

Accepted Answer

$$[\mathrm{C_2H_4}]$$ decreases and $$[\mathrm{C_2H_4Cl_2}]$$ increases.

Question 4

A system at equilibrium is compressed, causing the pressure to increase. Which of the following statements is true regarding the direction of the shift for a reaction where $$\Delta n_g \u003c 0$$?

Accepted Answer

The equilibrium shifts to the right, toward fewer moles of gas.

Question 5

For the reaction $$\mathrm{N_2$(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)}$$, what happens if the pressure is decreased by increasing the volume?

Accepted Answer

The equilibrium shifts to the left, favoring the formation of $$\mathrm{N_2$(g)}$$ and $$\mathrm{H_2$(g)}.$$

Question 6

Which of the following changes will NOT affect the position of equilibrium for a gaseous reaction?

Accepted Answer

Adding an inert gas at constant volume.

Question 7

A reaction at equilibrium has $$\Delta n_g = 0. $$What will be the effect of increasing the pressure by decreasing the volume?

Accepted Answer

There will be no effect on the position of equilibrium.

Question 8

Consider the following equilibrium: $$\mathrm{2NO_2(g) \rightleftharpoons N_2O_4(g)}. If $$the system is compressed, what will happen to the equilibrium?

Accepted Answer

The equilibrium will shift to the right, forming more $$\mathrm{N_2O_4(g)}.$$

Question 9

Which of the following best explains why increasing the pressure shifts the equilibrium toward the side with fewer moles of gas?

Accepted Answer

The system reduces the total number of gas molecules to counteract the increase in pressure.

Question 10

A reaction mixture at equilibrium is subjected to a sudden decrease in pressure (by increasing the volume). For the reaction $$\mathrm{2SO_3(g) \rightleftharpoons 2SO_2(g) + O_2$(g)}$$, what will be the effect?

Accepted Answer

The equilibrium will shift to the right, producing more $$\mathrm{SO_2$(g)}$$ and $$\mathrm{O_2$(g)}.$$

Chapter 16 lecture 2

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