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 constantA is the pre-exponential factorEa is the activation energyR is the gas constantT is the temperatureWe can use this equation to solve for the activation energy:Ea = -RTln(k/A)We can plug in the given values to get:Ea = -8.314 J/mol*K * 298 K * ln(3.61 × 10^-15 s^-1 / 8.66 × 10^-7 s^-1)Ea = 160 kJ/molTherefore, the activation energy for this reaction is 160 kJ/mol.

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

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