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A reaction has a first order rate constant of 3.63x10-5 s-1 at 25 degrees and 0.00203...

A reaction has a first order rate constant of 3.63x10-5 s-1 at 25 degrees and 0.00203 s-1 at 75 degrees. What is the value of the rate constant at 53 degrees?

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Answer #1

rate constant k1 = 3.63x10^-5 s-1

temperature T1 = 25 + 273 = 298 K

rate constant k2 = 0.00203 s-1

temperature T1 = 75 + 273 = 348 K

ln (k2 / k1) = H / R [1/T1 - 1/ T2]

ln (0.00203 /3.63x10^-5) = H / 8.314 x 10^-3 [1 / 298 - 1/348]

H = 69.39 kJ/mol

ln (k3 / k1) = H / R [1/T1 - 1/ T3]

ln (k3 /3.63x10^-5) = 69.39 / 8.314 x 10^-3 [1 / 298 - 1/326]

k3 = 4.023 x 10^-4

rate constant at 53 degrees = 4.023 x 10^-4 s-1

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