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For the reaction, $2 {NH}_{3} (g) ⟶ N_{2} (g) + 3 H_{2} (g)$
Identify the statement which is not correct :

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$S_{m N_{2}}^{\circ} + 3 S_{m H_{2}}^{\circ} > 2 S_{m {NH}_{3}}^{\circ}$

Heat absorbed at constant pressure and temperature will be more as compared to heat absorbed at constant volume.

$Σ$ Bond energy $reactant > \sum$ Bond energy product

The value of $Δ G^{\circ}$ is expected to be negative at extremely low temperatures.

answer is D.

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Detailed Solution

For $2 {NH}_{3} (g) ⟶ N_{2} (g) + 3 H_{2} (g)$

Decomposition is endothermic, with increase of entropy. For $Δ G < 0 . T$ must be high.

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