Consider the following statements regarding the Arrhenius equation and reaction kinetics: I. A plot of k versus 1/T is a straight line with a slope of -E_a/R . II. For a reaction with zero activation energy, the rate constant is independent of temperature. III. The pre-exponential factor ( A ) has the same units as the rate constant ( k ). IV. For a given temperature increase, a reaction with a higher activation ener

Step-by-step solution

Statement I is correct: According to the Arrhenius equation, k = A - E_a RT . A plot of k versus 1/T gives a straight line with slope -E_a/R . Statement II is correct: If E_a = 0 , then e^ -E_a/RT = e^0 = 1 . The rate constant becomes k = A , which is independent of temperature. Statement III is correct: The exponential term e^ -E_a/RT is dimensionless, so the pre-exponential factor A must have the same units as the rate constant k . Statement IV is incorrect: The logarithmic ratio of rate constants at two temperat