Arrhenius Equation

Question

The activation energy for the gas phase decomposition of ethyl chloroformate is 123 kJ.

ClCOOC₂H₅C₂H₅Cl + CO₂

The rate constant at 462 K is 5.91×10^-4 /s. The rate constant will be _____  /s at 502 K.

please include steps on how to solve for K2

Answer 1

One more time...

ln (k2/k1) = -Ea/R (1T2 - 1/T1) ARRHENIUS EQUATION

k1 = 5.91x10^-4 s^-1

k2 = ?

Ea = 123 kJ/mol

R = 0.008314 kJ/Kmol

T1 = 462K

T2 = 502K

ln (k2/5.91x10^-4) = - 123/0.008314 (1/502 - 1/462)

ln (k2/5.91x10^-4) = -14,794 (0.00199 - 0.00216)

ln (k2/5.91x10^-4) = 2.51

(k2/5.91x10^-4) = 12.3

k2 = 7.27x10^-3 s^-1