We’re being asked to determine the activation energy for the reverse reaction.
We’re given the following information:
ΔH = 28 kJ/mol: Recall that the change in enthalpy (ΔH) is the difference in energy between products and reactants. ΔH for the reaction is positive, which means we have an endothermic reaction. This signifies that the products are higher in energy than the reactants.
For the first-order reaction 1/2 N2O4(g) → NO2(g); ∆H = 28 kJ/mol
the activation energy is 53 kJ/mol. What is the activation energy for the reverse reaction?
A) -25 kJ/mol
B) 81 kJ/mol
C) –53 kJ/mol
D) 25 kJ/mol
E) 53 kJ/mol