Multiple Choice
Given the reaction: N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g), the equilibrium constant K for this reaction is:
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
Which of the reactions is likely to produce more O2 at equilibrium at 25°C?
A
2 NO(g) ⇌ N2(g) + O2(g) Keq = 2.4 x 1030
B
2 NO2(g) ⇌ 2 NO + O2(g) Keq = 5.8 x 10–5
C
2 CO2(g) ⇌ O2(g) + 2 CO(g) Keq = 3.1 x 10–5
D
2 H2O(g) ⇌ 2 H2(g) + O2(g) Keq = 5.1 x 10–82
Verified step by step guidance1
Identify the equilibrium constant (Keq) for each reaction. The equilibrium constant provides insight into the extent of the reaction at equilibrium. A larger Keq indicates a greater extent of reaction towards the products.
Compare the Keq values for each reaction: 2 NO(g) ⇌ N2(g) + O2(g) has Keq = 2.4 x 10^30, 2 NO2(g) ⇌ 2 NO + O2(g) has Keq = 5.8 x 10^-5, 2 CO2(g) ⇌ O2(g) + 2 CO(g) has Keq = 3.1 x 10^-5, and 2 H2O(g) ⇌ 2 H2(g) + O2(g) has Keq = 5.1 x 10^-82.
Recognize that a larger Keq value indicates that the reaction favors the formation of products at equilibrium. Therefore, the reaction with the largest Keq will produce more O2 at equilibrium.
Analyze the Keq values: 2.4 x 10^30 is significantly larger than the other Keq values, indicating that the reaction 2 NO(g) ⇌ N2(g) + O2(g) is heavily product-favored.
Conclude that the reaction 2 NO(g) ⇌ N2(g) + O2(g) is likely to produce the most O2 at equilibrium at 25°C due to its significantly larger Keq value compared to the other reactions.
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