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  • Calculate b) the equilibrium constant for the formation of NO_2 from NO and O_2 at 298 K NO (g) + ½ O_2 (g) NO_2 (g) where

7.24     Calculate  b) the equilibrium constant for the formation of NO2 from NO and O2 at 298K

                NO{(g)}+\frac{1}{2}O_{2}(g) \rightleftharpoons NO_{2}(g)

                where

                \Delta _{f}G^{+}\left [ NO_{2} \right ]=52.0kJ/mol 

                \Delta _{f}G^{+}\left [ NO \right ]=87.0kJ/mol

                \Delta _{f}G^{+}\left [ O_{2} \right ]=0kJ/mol

Answers (1)

best_answer

We know that, 
The relation between \Delta G^0 and equilibrium constant (K_c) is expressed as;
\Delta G^0 = 2.303\times RT\log K_c

\Rightarrow \frac{-35\times 10^{-3}}{-2.303\times 8.314\times 298} = 6.134
Therefore, K_c = anti\log 6.134
                           =1.36\times 10^6

Posted by

manish

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