Which of the following is true when comparing an uncatalyzed reaction to the same reaction with a catalyst?

Question

BlackTom AI · Accepted Answer

When comparing an uncatalyzed reaction to the same reaction with a catalyst, several key concepts come into play about reaction energetics and rate.
Option 1: 'The catalyzed reaction will consume all of the catalyst.' This is incorrect because a catalyst is not consumed in a reaction; it participates to lower activation energy and is regenerated at the end.
Option 2: 'The catalyzed reaction will be slower.' In reality, a catalyst provides an alternative pathway with a lower activation energy, so the reaction proceeds more quickly, not slower.
Option 3: 'The catalyzed reaction will have the same deltaG.' This statement is true. A catalyst changes the rate by altering the reaction pathway and lowering the activation barrier, but it does not change the overall free energy change (deltaG) between reactants and products.
Option 4: 'The catalyzed reaction will have a higher activation energy.' This is false because the defining effect of a catalyst is to lower the activation energy, not raise it.
In summary, catalysts affect rate by lowering the activation energy and do not alter deltaG or get consumed, so the true statement concerns the unchanged deltaG while the activation barrier is reduced. The incorrect options misrepresent catalyst behavior by implying consumption, slower rates, or increased energy barriers.

Which of the following is true when comparing an uncatalyzed reaction to the same reaction with a catalyst?Single choice

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