He rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy . If the rate constant of this reaction is at , what will the rate constant be at ?

The question is incomplete, here is the complete question:

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea = 71.0 kJ/mol . If the rate constant of this reaction is 6.7 M^(-1)*s^(-1) at 244.0 degrees Celsius, what will the rate constant be at 324.0 degrees Celsius?

The rate constant at 324°C is

Explanation:

To calculate rate constant at two different temperatures of the reaction, we use Arrhenius equation, which is:

where,

= equilibrium constant at 244°C =

= equilibrium constant at 324°C = ?

= Activation energy = 71.0 kJ/mol = 71000 J/mol   (Conversion factor:  1 kJ = 1000 J)

R = Gas constant = 8.314 J/mol K

= initial temperature =

= final temperature =

Putting values in above equation, we get:

Hence, the rate constant at 324°C is

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