The table lists energetic data for three elementary reactions that occur in different experimental setups at 298 K.
Reaction
Ea,fwd (kJ mol−1)
ΔE (kJ mol−1)
I
50
–40
II
95
–5
III
35
+30
(a) For each reaction, calculate the activation energy of the reverse process.
(b) Rank the three reactions in order of decreasing forward rate constant at 298 K. Justify your ranking qualitatively without performing Arrhenius calculations.
(c) For each reaction, state whether the equilibrium mixture at 298 K is expected to be product-favored or reactant-favored, and explain your reasoning.
(d) The temperature is increased to 800 K. Predict which reaction will show the largest change in product yield, and support your prediction by discussing both kinetic and thermodynamic factors.