# If the activation energy for a given compound is found to be 42.0 kJ/mol, with a frequency factor of 8.0 x 10^10 s^(-1), what is the rate constant for this reaction at 298 K?

Jan 26, 2018

3.48 × 10^3

#### Explanation:

Rate constant can be calculated from Arrhenius equation

$k = A \times {e}^{- {E}_{a} / \left(R T\right)}$

Where,

k = Rate constant

A = Frequency factor

${E}_{a}$ = Activation energy

R = Gas constant

T = Absolute Temperature

k = 8.0 xx 10^10 s^-1 × e^-("42.0 kJ/mol × 1000 J/kJ"/("8.314 J/(mol K) × 298 K")) = 3.48 × 10^3