A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6s^-1 at 275 K,what is the rate constant at 366 K?

Question

Quizplus · Accepted Answer

We can use the Arrhenius equation to relate the rate constants at two temperatures:

k2 = A * exp(-Ea/R * (1/T2 - 1/T1))

where k1 and T1 are given, Ea is the activation energy (108 kJ/mol), R is the gas constant (8.31 J/mol*K), and T2 is the new temperature (366 K).

Plugging in the values, we get:

k2 = (4.60 × 10^-6) * exp(-108000/(8.31 * 366) * (1/366 - 1/275))

k2 = 0.58 s^-1

Therefore, the answer is C, 0.58 s^-1.

A Reaction Is Found to Have an Activation Energy of 108