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  • Calculate a) ∆G^+ 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 a) \Delta G^{0} 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

Given data,

     \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

given chemical reaction-
NO{(g)}+\frac{1}{2}O_{2}(g) \rightleftharpoons NO_{2}(g)

for the reaction, 
\Delta G^0 = \Delta G^0(products) - \Delta G^0 (reactants)
           = (52-87-0)
           = -35 kJ/mol

 

Posted by

manish

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