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For a reaction with an activation energy of 50 kJ/mol, what will happen to the r

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Question: For a reaction with an activation energy of 50 kJ/mol, what will happen to the rate if the temperature is increased by 20°C? (2022)

Options:

  1. Rate decreases
  2. Rate remains the same
  3. Rate increases significantly
  4. Rate increases slightly

Correct Answer: Rate increases significantly

Solution: 

Increasing the temperature generally increases the rate of reaction significantly due to higher kinetic energy.

For a reaction with an activation energy of 50 kJ/mol, what will happen to the r

Practice Questions

Q1
For a reaction with an activation energy of 50 kJ/mol, what will happen to the rate if the temperature is increased by 20°C? (2022)
  1. Rate decreases
  2. Rate remains the same
  3. Rate increases significantly
  4. Rate increases slightly

Questions & Step-by-Step Solutions

For a reaction with an activation energy of 50 kJ/mol, what will happen to the rate if the temperature is increased by 20°C? (2022)
  • Step 1: Understand that activation energy is the minimum energy required for a reaction to occur.
  • Step 2: Recognize that increasing the temperature gives molecules more kinetic energy.
  • Step 3: Realize that with more kinetic energy, more molecules can overcome the activation energy barrier.
  • Step 4: Conclude that as a result, the rate of the reaction will increase when the temperature is raised by 20°C.
  • Activation Energy – The minimum energy required for a chemical reaction to occur.
  • Effect of Temperature on Reaction Rate – Increasing temperature typically increases the kinetic energy of molecules, leading to a higher reaction rate.
  • Arrhenius Equation – A formula that shows the relationship between temperature and the rate constant of a reaction, indicating that rate increases exponentially with temperature.
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