1. Tardigrade
  2. Question
  3. Chemistry
  4. The equlibrium constant for the reaction 2NO2(g) leftharpoons 2NO(g)+O2(g) is 2× 10-6 at 185° C . Then the equilibrium constant for the reaction, 4NO(g)+2O2(g) leftharpoons 2NO2(g) at the same temperature would be

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Q. 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

KEAMKEAM 2007Equilibrium

Solution:

$ 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}} $