The rate constant for a certain reaction is measured at two different temperatures: Temperature K
376.0°C 4.8 x 10^8
280°C 2.3 x 10^8

Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to significant digits.

22.78KJ/ mol

Explanation:

The computation of activation energy follows by formula:

Given:

Hence, the activation energy for this reaction =22.78KJ/ mol

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.