Acertain reaction has an activation energy of 67.0 kj/mol and a frequency factor of a1 = 4.20×1012. what is the rate constant, k, of this reaction at 24.0 degrees c?

K = 7.00

Explanation:

1) Arrhenius equation

Arrhenius equation shows the relation between activation energy, temperature, and the equilibrium constant.

This is the equation:

       

Where:

K is the equilibrium constant,A is the frequency factor,Ea is the activation energy (in J/mol),T is the temperature in kelvins (K), andR is the universal constant.

2) Substitute, using the right units, and compute:

A = 4.20 × 10¹² (dimensionless)Ea = 67.0 kJ/mol = 67,000 J/molT = 24.0°C = 24.0 + 273.15 K = 297.15 KR = 8.314 J/K mol

K = 7.00

The answer would be