# 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                $\Delta _{f}G^{+}\left [ NO_{2} \right ]=52.0kJ/mol$                 $\Delta _{f}G^{+}\left [ NO \right ]=87.0kJ/mol$                $\Delta _{f}G^{+}\left [ O_{2} \right ]=0kJ/mol$

M manish

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

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