A first-order reaction has rate constants of 4.6 x 10 ^{-2} s^{-1} and 8.1 x 10^{-2} s^{-1} at 0°C and 20.°C, respectively. What is the value of the activation energy?

The **rate constant** of a chemical reaction** is a temperature dependent quantity**.

The relation between the rate constant and temperature is quantified by the **Arrhenius equation.**

We have the following data:

k_{1} = 4.6x10^{-2} s^{-1} at T_{1} = 0 ^{o}C

k_{2} = 8.1x10^{-2} s^{-1} 20 °C

R = 8.314 J/mol/K

**E**_{a}** = ?**

Arrhenius Equation

Arrhenius Equation

Arrhenius Equation

Arrhenius Equation