Question

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 5×105-fold increase in the reaction rate?

Answer 1

Answer:

By the same amount

Explanation:

The activation energy and the rate of a reaction rate is closely related to each other. The higher is the activation energy, the lower will the rate of chemical reaction.

Thus, if rate is to be increased by 5×105-fold then the activation energy must be lowered by the same factor as these two entities are inversely proportional to each other

Answer 2

The difference in activation energy is 33821 kJ/mol.

Now we know that the physiological temperature is 37°. The activation energy is the energy that colliding reactant particles must possess in order to be converted to products.

Since k2/k1 = 5×10^5

So;

5×10^ 5 = k2/k1 = E1/RT = E2/RT

Taking natural logarithm of both sides;

E2 - E1 = ln(5×10^5) × 8.314 × 310 K

E2 - E1 = 33821 kJ/mol

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