The rate at which a metal alloy oxidizes in an oxygen-containing atmosphere is a typical example of the practical utility of the Arrhenius equation. For example, the rate of oxidation of a magnesium alloy is represented by a rate constant, k. The value of k at 300°C is 1.05 * 10-8kg/(m4 # s). At 400°C, the value of k rises to 2.95 * 10-4kg/(m4 # s). Calculate the activation energy, Q, for this oxidation process (in units of kJ/mol).

The activation energy is  

Explanation:

From the question we are told that

      The rate constant is  k

       at the temperature

      The value of k is  

      at temperature

       The value of  k is  

The rate constant is mathematically represented as

Where Q is the activation energy

         R is the ideal gas constant with a value of  

          C is a constant

           T is the temperature

For the first  rate constant

For the second   rate constant

Now the ratio between the two given rate constant is  

  =>    

substituting values  

=>    

option number c is the right answer.