Reversible reactions and equilibrium：練習題

In the Haber process for the production of ammonia, which material is the source of nitrogen gas?

The production of ammonia is shown by the equation:
\(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\)

The forward reaction is exothermic. Which change would increase the rate of the reaction but decrease the equilibrium yield of ammonia?

In the Haber process for the manufacture of ammonia, \(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\) (\( \triangle H = -92 \text{ kJ/mol} \)), the operating temperature is maintained at around \(450\,^{\circ}\text{C}\) rather than at a much lower temperature such as \(200\,^{\circ}\text{C}\). Why is this moderate temperature chosen?

What happens to the appearance of hydrated cobalt(II) chloride crystals when they are heated?

A reversible reaction is at equilibrium:
\(2A(g) + B(g) \rightleftharpoons 2C(g)\)
The forward reaction is exothermic. Which change would shift the position of equilibrium to the left?

When hydrated cobalt(II) chloride is heated, its color changes from pink to blue. State the name of the substance that must be added to the blue compound to reverse this color change.

For a reversible reaction \(\text{A(aq)} + \text{B(aq)} \rightleftharpoons \text{C(aq)}\), how does increasing the concentration of reactant \(\text{A}\) affect the position of equilibrium?

Describe the observation when water is added to anhydrous copper(II) sulfate and identify the type of chemical change occurring in terms of hydration.

(a) Hydrated copper(II) sulfate crystals can be used to test for the presence of water.
(i) State the color change observed when water is added to anhydrous copper(II) sulfate.
(ii) Describe how heat affects hydrated copper(II) sulfate crystals, including the name of the process that occurs.

(b) The following reversible reaction is at equilibrium in a closed container:
\(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\)
(i) State two characteristics of a system that is in dynamic equilibrium.
(ii) Predict the effect on the position of equilibrium if the concentration of nitrogen, \(N_2\), is increased.

The following equation represents the reversible reaction for the hydration of anhydrous copper(II) sulfate:

\(\text{CuSO}_4\text{(s)} + 5\text{H}_2\text{O(l)} \rightleftharpoons \text{CuSO}_4\cdot5\text{H}_2\text{O(s)}\)

(a) State the color of anhydrous copper(II) sulfate and the color of hydrated copper(II) sulfate.
(b) Describe how you could change hydrated copper(II) sulfate back into anhydrous copper(II) sulfate.
(c) Explain why this reaction is described as reversible.