The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K. Determine the activation energy for this reaction.

Question

Quizplus · Accepted Answer

The Arrhenius equation is:k = Ae^(-Ea/RT)where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature.We can take the natural logarithm of both sides of the equation to get:ln(k) = ln(A) - (Ea/RT)If we plot ln(k) versus 1/T, we will get a straight line with a slope of -Ea/R.We can use the given data to plot the following graph:[Image of graph of ln(k) versus 1/T]The slope of the graph is -Ea/R = -160 kJ mol^-1.Therefore, the activation energy is 160 kJ mol^-1.

The First-Order Rearrangement of CH3NC Is Measured to Have a Rate

The First-Order Rearrangement of CH₃NC Is Measured to Have a Rate