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For a reaction with an activation energy of 50 kJ/mol, what is the effect of inc

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Question: For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?

Options:

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

Correct Answer: Rate constant increases

Solution: 

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

For a reaction with an activation energy of 50 kJ/mol, what is the effect of inc

Practice Questions

Q1
For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?
  1. Rate constant decreases
  2. Rate constant increases
  3. Rate constant remains the same
  4. Rate constant becomes zero

Questions & Step-by-Step Solutions

For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?
  • Step 1: Understand that the activation energy (Ea) is the energy needed for a reaction to occur.
  • Step 2: Know that the rate constant (k) is a number that tells us how fast a reaction happens.
  • Step 3: Learn about the Arrhenius equation, which shows the relationship between temperature and the rate constant: k = A * e^(-Ea/(RT)).
  • Step 4: Recognize that 'A' is a constant, 'R' is the gas constant, and 'T' is the temperature in Kelvin.
  • Step 5: Realize that as temperature (T) increases, the value of -Ea/(RT) becomes less negative, which makes e^(-Ea/(RT)) larger.
  • Step 6: Conclude that a larger value of e^(-Ea/(RT)) means a larger rate constant (k), indicating that the reaction will happen faster.
  • Arrhenius Equation – The Arrhenius equation relates the rate constant of a reaction to the temperature and activation energy, indicating that higher temperatures increase the rate constant.
  • 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 Rates – Increasing temperature generally increases the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the rate constant.
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