Question

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 ∆G.
C) The catalyzed reaction will have higher activation energy.
D) The catalyzed reaction will consume all of the catalyst.

Answer 1

The answer is; B

The catalysts do not change the free energy of the free Gibbs energy of the reaction which is potential of a thermodynamic system at a constant temperature and pressure. Catalyst only lowers the activation energy of the reactant to the reaction occurs faster to form products that it would occur naturally. Otherwise, the catalyst does not change the reaction in any way.

Answer 2

The catalyzed reaction will have the same ∆G is true when comparing an uncatalyzed reaction to the same reaction with a catalyst.

• Catalytic reactions are simply known to be chemical reactions where catalyst increases the rate of reaction whe non-catalytic reactions are chemical reactions is one that a catalyst is not involve in the reaction process.

• A catalyst is to lower the activation energy of the reaction, it deoes not affect enthalpy and the entropy and temperature remain the same therefore there it has no effect on Gibbs free energy and so the catalyzed reaction will have the same ∆G.

Conclusively, we can therefore say that

option b is the best answer that fit the statement above.

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