Question

For a reaction $A\to B$, enthalpy of reaction is $–4.2kJmo{l}^{–1}$ and enthalpy of activation is $9.6kJmo{l}^{–1}$. The correct potential energy profile for the reaction is shown in option.

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• A.
• B.
• C.
• D.

Answer 1

The correct option is C

For the reaction,
$A\to B\Delta H=-4.2kJmo{l}^{-1}$
Thus, the reaction is exothermic.
Hence, energy of reactants are higher than the products.

Also, enthalpy of activation ($E_2$) is approximately double of $\Delta H$ of reaction.
Hence, for the given reaction energy profile (c) is correct.