## How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant? [ENDORSED]

Arrhenius Equation: $\ln k = - \frac{E_{a}}{RT} + \ln A$

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### How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?

This was a self-test question in the book:
How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?
Could someone please explain in simple terms? Thank you!

Matthew 1C
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### Re: How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?

for part a) since catalysts speed up the rate of a reaction the rate law would be affected in that the value of the rate would be larger than the rate of the reaction without the presence of a catalyst. for part b) the lowered activation energy means that the constant is greatly increased, which is what accounts for the increased rate

Patricia Macalalag 2E
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### Re: How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?

For part b) isn't the answer no effect? The textbook says catalysts have no effect on the equilibrium composition.

Chem_Mod
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### Re: How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?  [ENDORSED]

I will discuss this in class this week.

Catalysts have no effect on thermodynamic parameters (equilibrium constant, etc.).

Timothy Kim 1B
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### Re: How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?

I believe it decreases the activation energy which will in turn increase the rate constant and rate of the reaction.

Christina Bedrosian 1B
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### Re: How does a homogeneous catalyst affect (a) the rate law; (b) the equilibrium constant?

part a increases because catalysts increase the rate of the reaction in general