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Assuming that the collision factor remains the same, by how much must an enzyme lower the activation energy of the reaction in order to achieve a 3×105-fold increase in the reaction rate?.

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pstnonsonjoku

The activation energy must be lowered by 32490 kJ/mol.

What is activation energy?

The term activation energy refers to the energy that reactant particles must posses in order for their collision to result in chemical reaction.

Given that for the reactions;

k2/k1 = [tex]3*10^5[/tex]

So;

[tex]3*10^5[/tex] = k2/k1 = E1/RT = E2/RT

Taking natural logarithm of both sides;

E2 - E1 = ln([tex]3*10^5[/tex]) × 8.314 × 310.15 = 32490 kJ/mol

Learn more about activation energy:  https://brainly.com/question/11334504

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