$2 A + 3 B \to 2 C; Δ H = - 40 k c a l$
Activation energy, $E_{a}$ for the given reaction is $70 k c a l$ . The activation energy for
$2 C \to 2 A + 3 B$ is:

110 k c a l

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30 k c a l

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- 110 k c a l

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- 30 k c a l

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Solution

The correct option is A $110 k c a l$
The given reaction is an exothermic reaction since $Δ H = - v e$
$E_{a_{F}}$ =Activation energy of the forward reaction
$E_{a_{B}}$ = Activation energy of the backward reaction

Enthalpy change can be expressed also in terms of activation energy,

$Δ H = E_{a_{F}} - E_{a_{B}}$
$- 40 = 70 - E_{a_{B}}$
$E_{a_{B}} = 110 k c a l$

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2A+3B→2C;ΔH=−40kcal Activation energy, Ea for the given reaction is 70 kcal. The activation energy for 2C→2A+3B is:

The correct option is A 110 kcalThe given reaction is an exothermic reaction since ΔH=−ve EaF =Activation energy of the forward reaction EaB= Activation energy of the backward reaction Enthalpy change can be expressed also in terms of activation energy, ΔH=EaF−EaB −40=70−EaB EaB=110kcal

$2 A + 3 B \to 2 C; Δ H = - 40 k c a l$
Activation energy, $E_{a}$ for the given reaction is $70 k c a l$ . The activation energy for
$2 C \to 2 A + 3 B$ is: