If a catalyst changes the activation energy of a forward reaction from 28.0 kcal/mol to 23.0 kcal/mol, what effect does it have on the reverse reaction?

Verified step by step guidance

1. Understand that a catalyst lowers the activation energy for both the forward and reverse reactions equally.
2. Recognize that the activation energy for the reverse reaction will also decrease by the same amount as the forward reaction.
3. Calculate the change in activation energy for the forward reaction: 28.0 kcal/mol - 23.0 kcal/mol.
4. Apply the same change in activation energy to the reverse reaction.
5. Conclude that the activation energy for the reverse reaction is reduced by the same amount as the forward reaction.

Key Concepts

Activation Energy

Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to transform into products. A lower activation energy means that more molecules have sufficient energy to react, thus increasing the reaction rate.

Catalysts

Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They work by providing an alternative reaction pathway with a lower activation energy. Importantly, catalysts affect both the forward and reverse reactions equally, thereby influencing the overall reaction dynamics.

Equilibrium and Reaction Rates

In a reversible reaction, the rates of the forward and reverse reactions are equal at equilibrium. The activation energy for the reverse reaction can be determined by the difference in energy between the reactants and products. If a catalyst lowers the activation energy for the forward reaction, it will similarly lower the activation energy for the reverse reaction, maintaining the balance of reaction rates.