The rate constant of a firstorder reaction is 295 x 10 s1 at

The rate constant of a first-order reaction is 2.95 x 10 s1 at 350.°C. If the activation energy is 121 kJ/mol, calculate the temperature at which its rate constant is 8.65 x 10*s1. oc

Solution

According to Arrhenius integrated equation,

lnk₂/k₁ = (E_a/R)[(1/T₁) - (1/T₂)]

ln[(8.65 * 10^-4) / (2.95*10^-4)] = (121 / 0.008314)[(1 / (623) - (1/T₂)]

T₂ = 653.0 K

t₂ = 653 - 273

t₂ = 380. ⁰C