Two elementary gas-phase reactions are being studied in the same laboratory.
• Reaction 1: NO₂(g) + CO(g) → NO(g) + CO₂(g); experimental activation energy 132 kJ mol⁻¹.
• Reaction 2: O₃(g) → O₂(g) + O(g); experimental activation energy 12 kJ mol⁻¹.
On a cool morning the laboratory temperature is 298 K. Later in the day the thermostat is adjusted and the temperature rises uniformly to 308 K while the reactions are still running under otherwise identical conditions.
(a) Identify which reaction will experience the larger proportional increase in its rate constant when the temperature rises from 298 K to 308 K.
(b) Using the concepts of activation energy and the distribution of molecular kinetic energies, explain in detail why the reaction you selected in part (a) is more sensitive to the 10 K temperature increase.
(c) Sketch a qualitative reaction energy profile for Reaction 1 on appropriately labeled axes. Clearly label the reactants, products, transition state, and the activation energy for the forward reaction.