Which of the following is true when comparing an uncatalyzed reaction to the same reaction with a catalyst?
A) The catalyzed reaction will be slower.
B) The catalyzed reaction will have the same â†G.
C) The catalyzed reaction will have higher activation energy.
D) The catalyzed reaction will consume all of the catalyst.

Catalysts are molecules that speed up chemical reactions.
They increase the rate of chemical reactions such that the rate at which reactants are converted to products increases.
Catalysts increase the rate of reaction by lowering the activation energy of the reactants.
Activation energy refers to the minimum energy required by the reactants for a reaction to occur.
Therefore, the rate of catalyzed reactions will be higher due to a decrease in the activation energy of the reactants.
However, catalysts do not affect delta G of a reaction and thus, delta G of an uncatalyzed reaction is the same as that of a catalyzed reaction.

topeadeniran2 topeadeniran2 · Answer 2 · 2021-10-28T15:13:19+02:00

The option that is true when comparing an uncatalyzed reaction to the same reaction with a catalyst is B. The catalyzed reaction will have the same â†G.

It should be noted that catalysts do not change the free energy of the Gibbs energy. Catalysts can only lower the activation energy of the reactant.

In such a situation, the enthalpy is not affected and the temperature remains the same. Therefore, the uncatalyzed reaction will be the same reaction as a catalyst.

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