The rate constant k for a certain reaction is measured at two different temperatures temperature 376.0 °c 4.8 x 108 280.0 °c 2.3 x 10 8 assuming the rate constant obeys the arrhenius equation, calculate the activation energy e for this reaction. round your answer to 2 significant digits. kj x10 mol

The activation energy for this reaction = 23 kJ/mol.

Explanation:

Using the expression,

Where,

is the activation energy

R is Gas constant having value = 8.314×10⁻³ kJ / K mol  

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (280 + 273.15) K = 553.15 K  

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (376 + 273.15) K = 649.15 K  

So,  

The activation energy for this reaction = 23 kJ/mol.