Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 9.3 × 10¹⁰ s^-1 and a rate constant of 1.06 × 10³ s^-1 at 273 K.

Question

Quizplus · Accepted Answer

The Arrhenius equation is:k = Ae^(-Ea/RT)where:k is the rate constantA is the frequency factorEa is the activation energyR is the gas constant (8.314 J/mol·K)T is the temperature in KelvinWe can rearrange this equation to solve for Ea:Ea = -RTln(k/A)Plugging in the given values, we get:Ea = -(8.314 J/mol·K)(273 K)ln(1.06 × 10^3 s^-1 / 9.3 × 10^10 s^-1)Ea = 42 kJ/molTherefore, the activation energy is 42 kJ/mol.

Calculate the Activation Energy, Ea, for a Reaction with a Frequency

Calculate the Activation Energy, E_a, for a Reaction with a Frequency