Chemistry
Chemistry
Problem
The multistep conversion X → Y occurs through three elementary steps with these potential-energy values relative to the reactants (in kJ·mol⁻¹): • transition state 1 = 60, • intermediate 1 = 15, • transition state 2 = 70, • intermediate 2 = 30, • transition state 3 = 45, • products = −10. Calculate the activation energy for each of the three forward elementary steps.Intuitive explanation
The activation energy for each step is the energy difference between the transition state and the reactants at the start of that step—not the original reactants. Sketch an energy diagram: each intermediate becomes the new "starting point" for the next step, so you subtract its energy from the transition state energy that follows it. The first step uses the original reactants (energy = 0) as its baseline, but steps 2 and 3 use their respective intermediates as baselines.
Intuitive explanation
The activation energy for each step is the energy difference between the transition state and the reactants at the start of that step—not the original reactants. Sketch an energy diagram: each intermediate becomes the new "starting point" for the next step, so you subtract its energy from the transition state energy that follows it. The first step uses the original reactants (energy = 0) as its baseline, but steps 2 and 3 use their respective intermediates as baselines.