For one reversible reaction, the backward reaction is endothermic. The activation energy of the backward reaction is $160\ \text{kJ mol}^{-1}$. It may be assumed that the backward reaction follows a mechanism that is exactly the reverse of the mechanism for the forward reaction. Which statement about the activation energy of the forward reaction is correct?
- AThe activation energy of the forward reaction is equal to $-160\ \text{kJ mol}^{-1}$.
- BThe activation energy of the forward reaction is $0\ \text{kJ mol}^{-1}$ but less than $+160\ \text{kJ mol}^{-1}$.
- CThe activation energy of the forward reaction is equal to $+160\ \text{kJ mol}^{-1}$.
- DThe activation energy of the forward reaction is greater than $+160\ \text{kJ mol}^{-1}$.