If the activation energy of a reaction is increased, what happens to the rate co

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Question: If the activation energy of a reaction is increased, what happens to the rate constant k?

Options:

Correct Answer: Decreases

Solution:

According to the Arrhenius equation, an increase in activation energy results in a decrease in the rate constant k.

If the activation energy of a reaction is increased, what happens to the rate constant k?

If the activation energy of a reaction is increased, what happens to the rate constant k?

Step 1: Understand what activation energy is. It is the minimum energy required for a reaction to occur.
Step 2: Learn about the rate constant k. It is a number that tells us how fast a reaction happens.
Step 3: Familiarize yourself with the Arrhenius equation, which relates the rate constant k to activation energy (Ea) and temperature (T).
Step 4: Note that the Arrhenius equation shows that as activation energy (Ea) increases, the value of k decreases.
Step 5: Conclude that if the activation energy of a reaction is increased, the rate constant k will decrease.

Arrhenius Equation – The Arrhenius equation relates the rate constant k of a reaction to the activation energy (Ea) and temperature (T), showing that an increase in Ea leads to a decrease in k.