Two elementary reactions occur in separate flasks under identical temperature and pressure conditions.
• Reaction 1: X(g) → Y(g)
– ΔE=−15kJ mol−1
– Forward activation energy Ea,fwd=80kJ mol−1
• Reaction 2: P(g) → Q(g)
– ΔE=+25kJ mol−1
– Forward activation energy Ea,fwd=65kJ mol−1
(a) Calculate the activation energy for the reverse process of each reaction. Show your work and include appropriate units.
(b) For each reaction, determine whether reactants or products are favored at equilibrium based solely on the given energies. Provide a brief justification.
(c) For each reaction, identify which direction (forward or reverse) will exhibit a greater fractional increase in rate when the temperature is raised by the same amount. Support your answer with reference to the activation energies you calculated.