In an exergonic reaction pathway, how does an increase in temperature affect the rate constant k according to the Arrhenius equation (k = A e^(-Ea/RT))?
Answer and explanation
Correct answer: B. The rate constant k increases as more colliding molecules possess kinetic energy >= Ea
According to the Arrhenius equation, increasing temperature T decreases the magnitude of the exponent (-Ea/RT), which increases the value of e^(-Ea/RT). Physically, higher temperature broadens the Maxwell-Boltzmann kinetic energy distribution, exponentially increasing the fraction of molecular collisions that possess sufficient kinetic energy to overcome the activation energy barrier (Ea), thereby increasing the rate constant k.
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