Question

For a first order reaction, $A⟶$ Product, the temperature dependent rate constant (k) was found to follow the equation $logk=-\frac{2000}{T}+6$ calculate the pre-exponential factor (A) and activation energy for the reaction.

Answer 1

Multiply the Equation by 2.303

$2.303logk=-\frac{4606}{T}+13.818$

$lnk-ln(1.002\times {10}^6)=-\frac{4606}{T}$

$k=1.002\times {10}^6\times e^{-4606/T}$

$k=1.002\times {10}^6$ $e^{-9212/RT}$

A = $1.002\times {10}^6$ and $E_a=9212$ in Cal