Areaction is found to have an activation energy of 108 kj/mol. if the rate constant for this reaction is 4.60 x 10-6 s-1 at 275 k, what is the rate constant at 366 k? 0.58 1/s

Explanation:

According to the Arrhenius equation,

or,

where,

=rate constant at =

= rate constant at = ?

= activation energy for the reaction = 108kJ/mol=108000 J/mol

R = gas constant = 8.314 J/moleK

= initial temperature =

= final temperature =

Now put all the given values in this formula, we get

Therefore, the rate constant at 366 K is

2b2t

explanation:

2b2t