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The rate of chemical reaction is doubled for every 10oC rise in temperature because of
- a)increase in the activation energy
- b)decrease in the activation energy
- c)increase in the number of molecular collision
- d)increase in the number of activated molecules
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
The rate of chemical reaction is doubled for every 10oC rise in temper...
Explanation:
Activation Energy:
- The rate of a chemical reaction is determined by the activation energy required for the reaction to occur.
- Activation energy is the minimum amount of energy required for a reaction to take place.
Effect of Temperature on Activation Energy:
- When the temperature is increased, the average kinetic energy of the molecules also increases.
- This results in more molecules having energy equal to or greater than the activation energy.
- Therefore, the number of activated molecules increases with an increase in temperature.
Impact on Reaction Rate:
- The rate of a chemical reaction is directly proportional to the number of activated molecules.
- When the number of activated molecules doubles, the rate of reaction also doubles.
- This is because there are more molecules capable of overcoming the activation energy barrier and participating in the reaction.
Conclusion:
- Therefore, the rate of a chemical reaction is doubled for every 10oC rise in temperature due to an increase in the number of activated molecules.
- This phenomenon is described by the Arrhenius equation, which shows the exponential relationship between reaction rate and temperature.
Activation Energy:
- The rate of a chemical reaction is determined by the activation energy required for the reaction to occur.
- Activation energy is the minimum amount of energy required for a reaction to take place.
Effect of Temperature on Activation Energy:
- When the temperature is increased, the average kinetic energy of the molecules also increases.
- This results in more molecules having energy equal to or greater than the activation energy.
- Therefore, the number of activated molecules increases with an increase in temperature.
Impact on Reaction Rate:
- The rate of a chemical reaction is directly proportional to the number of activated molecules.
- When the number of activated molecules doubles, the rate of reaction also doubles.
- This is because there are more molecules capable of overcoming the activation energy barrier and participating in the reaction.
Conclusion:
- Therefore, the rate of a chemical reaction is doubled for every 10oC rise in temperature due to an increase in the number of activated molecules.
- This phenomenon is described by the Arrhenius equation, which shows the exponential relationship between reaction rate and temperature.
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The rate of chemical reaction is doubled for every 10oC rise in temperature because ofa)increase in the activation energyb)decrease in the activation energyc)increase in the number of molecular collisiond)increase in the number of activated moleculesCorrect answer is option 'D'. Can you explain this answer?
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