For the reaction at 298 ,K

CHEMISTRY · Single correct · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

For the reaction 2 NO2(g)⇌N2O4(g)2\,\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) at 298\,K, the equilibrium constant is K=170K = 170. A sealed vessel is found to have Q=50Q = 50 for the forward reaction as written. A student instead considers the reaction written in the reverse direction: N2O4(g)⇌2 NO2(g)\text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) Which of the following best describes the system’s response relative to this rewritten reaction? (a) It will shift toward products (2 NO2)(2\,\text{NO}_2) because Qnew>KnewQ_{\text{new}} > K_{\text{new}}. (b) It will shift toward products (2 NO2)(2\,\text{NO}_2) because Qnew<KnewQ_{\text{new}} < K_{\text{new}}. (c) It will shift toward reactants (N2O4)(\text{N}_2\text{O}_4) because Qnew>KnewQ_{\text{new}} > K_{\text{new}}. (d) It will shift toward reactants (N2O4)(\text{N}_2\text{O}_4) because Qnew<KnewQ_{\text{new}} < K_{\text{new}}.

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