Question

The equlibrium constant for the reaction $ 2N{{O}_{2}}(g) \rightleftharpoons 2NO(g)+{{O}_{2}}(g) $ is $ 2\times {{10}^{-6}} $ at $ 185{}^\circ C $ . Then the equilibrium constant for the reaction, $ 4NO(g)+2{{O}_{2}}(g) \rightleftharpoons $ $ 2N{{O}_{2}}(g) $ at the same temperature would be

• A. $ 2.5\times {{10}^{-5}} $
• B. $ 4\times {{10}^{-12}} $
• C. $ 2.5\times {{11}^{11}} $
• D. $ 2\times {{10}^{6}} $

Answer 1

The Correct Option is C

$ 2N{{O}_{2}}(g) \rightleftharpoons 2NO(g)+{{O}_{2}}(g) $ $ K=\frac{{{[NO]}^{2}}[{{O}_{2}}]}{{{[N{{O}_{2}}]}^{2}}}=2\times {{10}^{-6}} $ $ 4N{{O}_{2}}(g)+2{{O}_{2}}(g)4N{{O}_{2}}(g) $ $ K=\frac{{{[N{{O}_{2}}]}^{4}}}{{{[NO]}^{4}}{{[{{O}_{2}}]}^{2}}} $ $ =\frac{1}{{{(K)}^{2}}}=\frac{1}{{{(2\times {{10}^{-6}})}^{2}}} $ Equilibrium constant $ K=0.25\times {{10}^{12}} $ $ =2.5\times {{10}^{11}} $