Identify the statement that is not correct.

The activation energy of the forward process is equal to that of the reverse process.
In a reversible reaction, raising the temperature increases the rates of both the forward and backward reactions.
For a second-order reaction, a higher starting concentration of reactant leads to a smaller half-life.
If the change in A is infinitesimally small, the average rate is equal to the instantaneous rate.

Correct answer: The activation energy of the forward process is equal to that of the reverse process.

Solution

Ea(forward) - Ea(reverse) = delta H of reaction, so they are equal only if delta H = 0; in general they differ, making this statement the incorrect one. The other three statements are true.

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