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If the rate of a reaction doubles when the temperature is increased by 10°C, wha

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Question: If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?

Options:

  1. 20 kJ/mol
  2. 40 kJ/mol
  3. 60 kJ/mol
  4. 80 kJ/mol

Correct Answer: 40 kJ/mol

Solution: 

Using the Arrhenius equation, a rule of thumb states that for every 10°C increase in temperature, the rate doubles if Ea is around 40 kJ/mol.

If the rate of a reaction doubles when the temperature is increased by 10°C, wha

Practice Questions

Q1
If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?
  1. 20 kJ/mol
  2. 40 kJ/mol
  3. 60 kJ/mol
  4. 80 kJ/mol

Questions & Step-by-Step Solutions

If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?
  • Step 1: Understand that the rate of a reaction can change with temperature.
  • Step 2: Know that the Arrhenius equation relates temperature and reaction rate to activation energy (Ea).
  • Step 3: Recognize the rule of thumb: if the rate doubles with a 10°C increase, it suggests a specific activation energy.
  • Step 4: Remember that for an activation energy of around 40 kJ/mol, the rate will double with a 10°C increase.
  • Step 5: Conclude that the approximate activation energy (Ea) of the reaction is 40 kJ/mol.
  • Arrhenius Equation – The Arrhenius equation relates the rate of a chemical reaction to temperature and activation energy, indicating how temperature affects reaction rates.
  • Activation Energy (Ea) – The minimum energy required for a chemical reaction to occur, which can be estimated using temperature changes and reaction rate observations.
  • Temperature Dependence of Reaction Rates – The principle that reaction rates typically increase with temperature, often following a specific pattern that can be quantified.
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