For which one of the following system $Δ E < Δ H$

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$2 {SO}_{2 (g)} + O_{2 (g)} \to 2 SO$

$2 {NH}_{3 (g)} \to N_{2 (g)} + 3 H_{2 (g)}$

$H_{2 (g)} + I_{2 (g)} \to 2 HI$

$N_{2 (g)} + O_{2 (g)} \to 2 NO$

answer is C.

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Detailed Solution

The first law of thermodynamics represents the conservation of energy which states that energy can neither be created nor be destroyed it can only change forms.

We know, $Δ H = Δ E + Δ n R T$

Where, $Δ H$ is the enthalpy change, $Δ E$ is the internal energy change and $Δ n$ is the number of gaseous moles of product - number of gaseous moles of reactant.

When $Δ n > 0, Δ H > Δ E$

And when $Δ n < 0, Δ H < Δ E$

Considering the equation, $2 {NH}_{3 (g)} \to N_{2 (g)} + 3 H_{2 (g)}$