If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

Question

Quizplus · Accepted Answer

The rate constant can be calculated using the Arrhenius equation:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin.

Plugging in the values given:

k = (8.0 × 10^13 s^-1) * e^(-42000 J/mol / (8.314 J/mol*K * 298 K))

k = 3.5 × 10^-13 s^-1

Therefore, the best choice is E.

If the Activation Energy for a Given Compound Is Found