In a reversible reaction, how does the activation energy required for the exothermic change compare with the activation energy required for the endothermic change?
2007-05-25 13:19:40 · 3 answers · asked by Rosy 2 in Science & Mathematics ➔ Chemistry
activation energy for the exothermic reaction is less than the activation energy for the endothermic reaction
2007-05-25 13:27:04 · answer #1 · answered by Alex 2 · 0⤊ 0⤋
The position of the activated complex does not change, but relative to the position of the products and reactants, the energy difference between the activated complex and the reactants will be lower for the exothermic reaction than it will be for the endothermic reaction.
2007-05-25 13:27:24 · answer #2 · answered by TheOnlyBeldin 7 · 0⤊ 0⤋
if you have a reaction lets say
A+B =>C
if that reaction is endothermic and requires Q1 Joules then the reaction
C=>A+B
is exothermic and Q2 is the amount of energy released
so we have Q1=-Q2
2007-05-25 23:18:25 · answer #3 · answered by james01gr 2 · 0⤊ 0⤋