Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the following reaction equation. 2h202(aq) →2h20(/) + 02(g) the activation energy for this reaction is 75 kj/mol. in the presence of a metal catalyst the activation energy is lowered to 49 kj/mol. at what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25°c?

Answer : The temperature for non-catalyzed reaction needed will be 456 K

Explanation :

Activation energy : The energy required to initiate the reaction is known as activation energy.

According to the Arrhenius equation,

Since, the rate for both the reaction are equal.

..........(1)

where,

= activation energy for non-catalyzed reaction = 75 kJ/mol

= activation energy for catalyzed reaction = 49 kJ/mol

=  temperature for non-catalyzed reaction = ?

= temperature for catalyzed reaction =

Now put all the given values in the above formula 1, we get:

Therefore, the temperature for non-catalyzed reaction needed will be 456 K

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