Given the following data for the reaction A B, determine the activation energy, E_a, of the reaction.

Question

Quizplus · Accepted Answer

To determine the activation energy, we can use the Arrhenius equation:
k = Ae^(-Ea/RT)
Taking the natural logarithm of both sides:
ln(k) = ln(A) - Ea/RT
We can plot ln(k) vs. 1/T and the slope of the line will be -Ea/R, where R is the gas constant (8.314 J/(mol*K)).

Using the given data, we can calculate ln(k) for each temperature:
ln(k1) = ln(2.04) = 0.714
ln(k2) = ln(6.78) = 1.915

Then we can plot ln(k) vs. 1/T (in K^-1):
slope = (-1)*(1.915 - 0.714)/(1/400 - 1/250) = 19.4 kJ/mol

Therefore, the activation energy is 19.4 kJ/mol (choice B).

Given the Following Data for the Reaction a B