Step 1

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{\xb0}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{\u2206}}{\mathbf{H}}{\mathbf{\xb0}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{T}}{\mathbf{\u2206}}{\mathbf{S}}{\mathbf{\xb0}}}$

$\mathbf{\u2206}\mathbf{G}\mathbf{\xb0}\mathbf{}\mathbf{=}\mathbf{(}\mathbf{-}\mathbf{58}\mathbf{.}\mathbf{03}\mathbf{}\mathbf{kJ}\mathbf{)}\mathbf{}\mathbf{-}\mathbf{}\mathbf{(}\mathbf{298}\mathbf{}\overline{)\mathbf{K}}\mathbf{)}\mathbf{(}\mathbf{-}\mathbf{176}\mathbf{.}\mathbf{6}\mathbf{}\frac{\overline{)\mathbf{J}}}{\overline{)\mathbf{K}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{kJ}}{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\overline{)\mathbf{J}}}\mathbf{)}$

For the reaction at 298 K,

2NO_{2} (g) ⇌ N_{2}O_{4} (g)

the values of ΔH° and ΔS° are -58.03 kJ and -176.6 J/K, respectively. What is the value of ΔG° at 298 K? Assuming that ΔH° and ΔS° do not depend on temperature, at what temperature is ΔG° = 0? Is ΔG° negative above or below this temperature?

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