The energy change accompanying the equilibrium reaction `A hArrB` is `-33.0kJ mol^(-1)`. Calculate Equilibrium constant `K_a` for the reaction at 300 K

Explanation

To calculate the equilibrium constant \( K_a \) for the reaction \( A \rightleftharpoons B \) at 300 K given that the energy change (\( \Delta H \)) is \(-33.0 \, \text{kJ mol}^{-1}\), we can follow these steps:

### Step 1: Understand the relationship between \( \Delta H \) and activation energies
The change in enthalpy (\( \Delta H \)) for the reaction is related to the activation energies of the forward (\( E_f \)) and backward (\( E_b \)) reactions by the equation:
\[ \Delta H = E_f - E_b \]
Given that \( \Delta H = -33.0 \, \text{kJ mol}^{-1} \), we can express this as:
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