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(D) The reaction for the dimerization of $NO_2$ is: $2NO_{2(g)} \rightarrow N_2O_{4(g)}$.
The enthalpy change of the reaction $(\Delta H_{reaction})$

Vedclass · Accepted Answer

$-14$

Vedclass · Answer

(D) The reaction for the dimerization of $NO_2$ is: $2NO_{2(g)} ightarrow N_2O_{4(g)}$.
The enthalpy change of the reaction $(\Delta H_{reaction})$ is calculated using the standard heats of formation $(\Delta H_f^o)$:
$\Delta H_{reaction} = \sum \Delta H_f^o(	ext{products}) - \sum \Delta H_f^o(	ext{reactants})$.
$\Delta H_{reaction} = \Delta H_f^o(N_2O_4) - 2 	imes \Delta H_f^o(NO_2)$.
Substituting the given values: $\Delta H_{reaction} = 2.0 - 2 	imes 8.0$.
$\Delta H_{reaction} = 2.0 - 16.0 = -14.0 \ kcal$.

The standard heats of formation in $kcal \ mol^{-1}$ of $NO_{2(g)}$ and $N_2O_{4(g)}$ are $8.0$ and $2.0$ respectively. The heat of dimerization of $NO_2$ in $kcal$ for the reaction $2NO_{2(g)} \rightarrow N_2O_{4(g)}$ is:

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