The reaction A $\to$ C has activation for the forward and the backward reaction as 25 kJ and 32 kJ respectively. The $Δ$ H for the reaction is

57 kJ

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-57 kJ

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7 kJ

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-7 kJ

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Solution

The correct option is D -7 kJ
$Δ$ H= $E_{a}$ (forward) - $E_{a}$ (backward)
= 25 - 32 = - 7 KJ

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The reaction A → C has activation for the forward and the backward reaction as 25 kJ and 32 kJ respectively. The Δ H for the reaction is

The correct option is D -7 kJ ΔH=Ea (forward) - Ea (backward) = 25 - 32 = - 7 KJ

The reaction A $\to$ C has activation for the forward and the backward reaction as 25 kJ and 32 kJ respectively. The $Δ$ H for the reaction is

The correct option is D -7 kJ
$Δ$ H= $E_{a}$ (forward) - $E_{a}$ (backward)
= 25 - 32 = - 7 KJ