The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g)  2NO₂(g) + ¹/₂O₂(g)
The value of the rate constant (k) is 1.35  10^-4 s^-1 at 35°C. What is the value of k at 0°C?

Question

Quizplus · Accepted Answer

To calculate the value of k at 0°C, we need to use the Arrhenius equation:

k = A * exp(-Ea/RT)

Where A is the pre-exponential factor, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin. We have all the values except for A, which we can solve for by using the given rate constant at 35°C:

1.35 * 10^-4 = A * exp(-102,000/(8.314 * 308))

A = 2.67 * 10^5

Now we can use this value of A to calculate k at 0°C:

k = (2.67 * 10^5) * exp(-102,000/(8.314 * 273))

k = 8.2 * 10^-7 s^-1

Therefore, the best choice is (A) 8.2 * 10^-17 s^-1.

The Activation Energy for the Following First-Order Reaction Is 102