Question

question 1 (1 point)
for an exothermic reaction, what does the activation energy of the reverse reaction equal?
the activation energy of the forward reaction
the heat of reaction minus the activation energy of the forward reaction
the activation energy of the forward reaction minus the heat of reaction
the heat of reaction plus the activation energy of the forward reaction
the heat of reaction minus the activation energy of the reverse reaction

Explanation:

For an exothermic reaction, the energy of the products is lower than that of the reactants. The activation energy of the forward reaction (\(E_{a,\text{forward}}\)) is the energy barrier from reactants to the transition - state. The heat of reaction (\(\Delta H\)) is negative (\(\Delta H=H_{\text{products}} - H_{\text{reactants}}<0\)).

The activation energy of the reverse reaction (\(E_{a,\text{reverse}}\)) is the energy barrier from products to the transition - state.

We know that \(E_{a,\text{reverse}}=E_{a,\text{forward}}-\Delta H\). Since \(\Delta H<0\) (exothermic), \(E_{a,\text{reverse}} = E_{a,\text{forward}}+|\Delta H|\)

Answer:

the heat of reaction plus the activation energy of the forward reaction