A certain reaction has an activation energy of 28.90 kJ / mol. At what Kelvin temperature will the reaction proceed 5.00 times faster than it did at 313 K?

365 K

Explanation:

According to the Arrhenius equation,

or,

where,

= rate constant at = 1.00

= rate constant at = 5.00

= activation energy for the reaction = 28.90 kJ/mol= 28900 j/mol

R = gas constant = 8.314 J/mole.K

= initial temperature = 313 K

= final temperature = ?

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

Therefore, 365 K is required to increase the reaction rate by 5.00 times.