Answer:
The rate constant for the reaction at 75 °C = 4.6 × 10^(-2) s^(-1)
Explanation:
By Arrhenius equitation
k = Ae^(-Ea/(RT))
Therefore
3.7 x 10-3 s-1 = A×e^(43600J/mol/(8.3145×298))
Therefore A = 160900.320
Therefore at 75 °C T = 348.15 K and k = 160900.320×e^(-43600/(8.314×348.15)
k = 4.6 × 10^(-2) s^(-1)
the rate constant for this reaction at 75 °C is k = 4.6 × 10^(-2) s^(-1)
Which shows that the rate of reaction increases as temperature increases that is the proportions of effective collisions with energy equal to or greater than the activation energy increases.
