Based on their activation energies and energy chan...

Question

Based on their activation energies and energy changes and
assuming that all collision factors are the same, which of the
following reactions would be fastest in the reverse direction?(a) Ea = 45 kJ/mol; ΔE = –25 kJ/mol(b) Ea = 35 kJ/mol; ΔE = –10 kJ/mol(c) Ea = 55 kJ/mol; ΔE = 10 kJ/mol

Jules Bruno · Accepted Answer

We are being asked to determine which of the following reactions would be fastest in the reverse direction.Recall the definitions Ea is the difference in energy between reactants and transition state.ΔE is the difference in energy between products and reactants[readmore]Let’s draw the energy diagrams for each choice to (a) Ea = 45 kJ/mol; ΔE = –25 kJ/mol favors the formation of the product more than the formation of the reactantfavor forward reactionslow reverse reaction(b) Ea = 35 kJ/mol; ΔE = –10 kJ/mol favors the formation of the product more than the formation of the reactantfavor forward reactionslow reverse reaction(c) Ea = 55 kJ/mol; ΔE = 10 kJ/molfavors the formation of the reactant more than the formation of the productfavor reverse reactionfast reverse reactionFor the reverse reaction, choice B and C will relatively occur at the same rate but choice A will be faster because it favors the formation of the reactant.Answer: The reaction with (c) Ea = 55 kJ/mol; ΔE = 10 kJ/mol would be fastest in the reverse direction

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