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For a reaction with an activation energy of 50 kJ/mol, what is the effect of a 1

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Question: For a reaction with an activation energy of 50 kJ/mol, what is the effect of a 10 kJ/mol increase in activation energy on the rate constant at a constant temperature?

Options:

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

Correct Answer: Rate constant decreases

Solution: 

An increase in activation energy decreases the rate constant according to the Arrhenius equation, k = Ae^(-Ea/RT), where an increase in Ea results in a smaller k.

For a reaction with an activation energy of 50 kJ/mol, what is the effect of a 1

Practice Questions

Q1
For a reaction with an activation energy of 50 kJ/mol, what is the effect of a 10 kJ/mol increase in activation energy on the rate constant at a constant temperature?
  1. Rate constant increases
  2. Rate constant decreases
  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 a 10 kJ/mol increase in activation energy on the rate constant at a constant temperature?
  • Step 1: Understand what activation energy (Ea) is. It is the minimum energy required 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: Familiarize yourself with the Arrhenius equation: k = A * e^(-Ea/RT). Here, A is a constant, e is the base of natural logarithms, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.
  • Step 4: Recognize that if the activation energy (Ea) increases, the exponent (-Ea/RT) becomes more negative.
  • Step 5: Understand that a more negative exponent means that e^(-Ea/RT) becomes smaller.
  • Step 6: Conclude that if the value of k decreases, the reaction rate slows down when activation energy increases.
  • Arrhenius Equation – The Arrhenius equation relates the rate constant (k) of a reaction to its activation energy (Ea), temperature (T), and a pre-exponential factor (A).
  • Effect of Activation Energy on Rate Constant – An increase in activation energy leads to a decrease in the rate constant, indicating that the reaction becomes slower.
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