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Standard VIII

Chemistry

Collision Theory

If for a reac...

Question

If for a reaction, $A \to B$ , $Δ H = - 10 {kJ mol}^{- 1}$ and $E_{a} = 50 {kJ mol}^{- 1}$ , the energy of activation for the reaction, $B \to A$ will be:

40 {kJ mol}^{- 1}

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50 {kJ mol}^{- 1}

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- 50 {kJ mol}^{- 1}

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60 {kJ mol}^{- 1}

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Solution

The correct option is D $60 {kJ mol}^{- 1}$
$Δ H (A \to B) = - 10 {kJ mol}^{- 1}$
Hence, it is an exothermic reaction.

$∴ E_{a} (A \to Activated state) = 50 {kJ mol}^{- 1}$
$∴ E_{a} (B \to Activated state)$
$= E_{a} (Activated state) + Δ H$
$= 50 + 10 = 60 {kJ mol}^{- 1}$

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If for a reaction, A→B, ΔH=−10 kJ mol−1 and Ea=50 kJ mol−1, the energy of activation for the reaction, B→A will be:

The correct option is D 60 kJ mol−1ΔH(A→B)=−10 kJ mol−1 Hence, it is an exothermic reaction. ∴Ea (A→Activated state)=50 kJ mol−1 ∴Ea (B→Activated state) =Ea (Activated state)+ΔH =50+10=60 kJ mol−1

If for a reaction, $A \to B$ , $Δ H = - 10 {kJ mol}^{- 1}$ and $E_{a} = 50 {kJ mol}^{- 1}$ , the energy of activation for the reaction, $B \to A$ will be:

The correct option is D $60 {kJ mol}^{- 1}$
$Δ H (A \to B) = - 10 {kJ mol}^{- 1}$
Hence, it is an exothermic reaction.

$∴ E_{a} (A \to Activated state) = 50 {kJ mol}^{- 1}$
$∴ E_{a} (B \to Activated state)$
$= E_{a} (Activated state) + Δ H$
$= 50 + 10 = 60 {kJ mol}^{- 1}$