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The activation energy of a reaction is 3.5 kJ/mol and the change in enthalpy for the forward reaction is -67.2 kJ/mol. What is the activation energy of the reverse reaction?
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15. Chemical Kinetics
Energy Diagrams
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In an energy diagram for a chemical reaction, what does the 'energy hill' represent?
A
The total energy released by the reaction
B
The energy of the reactants at the start of the reaction
C
The activation energy required for the reaction to proceed
D
The energy difference between products and reactants
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Understand that an energy diagram for a chemical reaction plots the potential energy of the system as the reaction progresses from reactants to products.
Recognize that the 'energy hill' in the diagram corresponds to the highest point on the curve, which represents the energy barrier that must be overcome for the reaction to proceed.
This energy barrier is known as the activation energy, which is the minimum energy required to convert reactants into the transition state before forming products.
Note that the total energy released by the reaction is represented by the difference in energy between reactants and products, not the 'energy hill'.
Therefore, the 'energy hill' specifically represents the activation energy required for the reaction to proceed.
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