A reaction has a rate constant of 2.08 × 10−4 s−1 at 26 oC and 0.394 s−1 at 79 oC . Determine the activation barrier for the reaction. Enter your answer numerically and in terms of kJ/mol

The activation energy of the reaction is 124.6 kJ/mol

Explanation:

To calculate activation energy of the reaction, we use Arrhenius equation, which is:

where,

= equilibrium constant at 79°C =

= equilibrium constant at 26°C =

= Activation energy of the reaction = ?

R = Gas constant = 8.314 J/mol K

= initial temperature =

= final temperature =

Putting values in above equation, we get:

Hence, the activation energy of the reaction is 124.6 kJ/mol

b) mutualism

hope this : )

8 m/s because for him to get the same amount of energy as ray is putting out, bobby, who weighs half as much as ray, needs to run twice as fast.