Chemical Kinetics and Nuclear ChemistryHard

Question

For the reversible reaction A$\rightleftharpoons$B; ΔH = −2 kcal, the pre-exponential factors are same for the forward and backward reactions. If the activation energy of backward reaction is 8 kcal/mol, then which of the following statements is/are correct about the reaction?

Options

A.The activation energy of forward reaction is 6 kcal/mol
B.At 500 K, the fraction of ‘A’ molecules crossing the energy barrier for forward reaction is e−6.
C.At 500 K, the fraction of ‘B’ molecules crossing the energy barrier for forward reaction is e−8.
D.Equilibrium constant for the reaction is e−2 at 500 K.

Solution

$\Delta H = E_{af} - E_{a_{b}}$

$\Rightarrow - 2 = E_{a_{f}} - 8 $$$\Rightarrow E_{a_{f}} = 6\text{ kcal/mol}$$

Now, the fraction of molecules crossing energy barrier $= e^{- E_{a}/RT}$and $K_{eq} = e^{- \Delta H/RT}$.

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