If the rate of a reaction doubles when the temperature increases by 10°C, what i

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Question: If the rate of a reaction doubles when the temperature increases by 10°C, what is the approximate activation energy? (2020)

Options:

Correct Answer: 40 kJ/mol

Solution:

Using the Arrhenius equation, if the rate doubles for a 10°C increase, Ea is approximately 40 kJ/mol.

If the rate of a reaction doubles when the temperature increases by 10°C, what is the approximate activation energy? (2020)

If the rate of a reaction doubles when the temperature increases by 10°C, what is the approximate activation energy? (2020)

Step 1: Understand that the Arrhenius equation relates the rate of a reaction to temperature and activation energy (Ea).
Step 2: Recognize that if the rate of a reaction doubles, it indicates a significant change in the reaction's speed due to temperature increase.
Step 3: Note that a 10°C increase in temperature is the condition given in the question.
Step 4: Use the rule of thumb that for many reactions, a 10°C increase in temperature can double the reaction rate if the activation energy is around 40 kJ/mol.
Step 5: Conclude that since the rate doubles with a 10°C increase, the approximate activation energy (Ea) is about 40 kJ/mol.

Arrhenius Equation – The Arrhenius equation relates the rate of a chemical reaction to temperature and activation energy, showing how reaction rates increase with temperature.
Activation Energy (Ea) – The minimum energy required for a chemical reaction to occur, which can be estimated using the temperature dependence of reaction rates.
Temperature Dependence of Reaction Rates – Understanding how small changes in temperature can significantly affect the rate of a reaction, often modeled by the Arrhenius equation.