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If the activation energy of a reaction is 50 kJ/mol, what is the effect of incre

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Question: If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?

Options:

  1. Rate constant decreases
  2. Rate constant remains the same
  3. Rate constant increases
  4. Rate constant doubles

Correct Answer: Rate constant increases

Solution: 

According to the Arrhenius equation, an increase in temperature generally increases the rate constant, as it provides more energy to overcome the activation energy barrier.

If the activation energy of a reaction is 50 kJ/mol, what is the effect of incre

Practice Questions

Q1
If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
  1. Rate constant decreases
  2. Rate constant remains the same
  3. Rate constant increases
  4. Rate constant doubles

Questions & Step-by-Step Solutions

If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
  • Step 1: Understand what activation energy is. It is the minimum energy required for a reaction to occur.
  • Step 2: Know that the rate constant (k) of a reaction is influenced by temperature.
  • Step 3: Familiarize yourself with the Arrhenius equation, which shows the relationship between temperature and the rate constant.
  • Step 4: Recognize that increasing the temperature from 300 K to 350 K means the molecules have more energy.
  • Step 5: Realize that with more energy, more molecules can overcome the activation energy barrier.
  • Step 6: Conclude that as a result, the rate constant (k) will increase when the temperature is raised.
  • Arrhenius Equation – The Arrhenius equation relates the rate constant of a reaction to the temperature and activation energy, indicating that higher temperatures generally lead to higher rate constants.
  • Activation Energy – Activation energy is the minimum energy required for a reaction to occur, and it influences how temperature changes affect reaction rates.
  • Temperature Effect on Reaction Rate – Increasing temperature typically increases the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the reaction rate.
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