The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea= 50.0 KJ/mol. If the rate constant of this reaction is 0.14M^-1 s^-1 at -8.0°C. What will the rate constant be at 56.0°C?

The rate constant at 56.0°C is

Explanation:

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

where,

= equilibrium constant at -8.0°C =

= equilibrium constant at 56°C = ?

= Activation energy = 50.0 kJ/mol = 50000 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 56.0°C is

the first point, i am pretty sure.