MDCAT Chemistry MCQ #5142

The activation energy for a reaction is 50 kJ/mol. If the rate constant at 300 K is 2 × 10^(-3) s^(-1), what is the rate constant at 320 K?

MDCAT Chemistry MCQ #5142

  1. Question 1

    Q1. The activation energy for a reaction is 50 kJ/mol. If the rate constant at 300 K is 2 × 10^(-3) s^(-1), what is the rate constant at 320 K?

    • A) 8.34 × 10^(-3) s^(-1)
    • B) 4.23 × 10^(-3) s^(-1)
    • C) 1.04 × 10^(-2) s^(-1)
    • D) 6.45 × 10^(-3) s^(-1)

    Answer: 8.34 × 10^(-3) s^(-1)

    Explanation: Using Arrhenius equation, k2 = k1 exp(Ea/R(1/T1 - 1/T2)) = 8.34 × 10^(-3) s^(-1).