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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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The rate of chemical reaction is doubled for every 10oC rise in temper...
Doubling the temperature of a solvent will increase the temperature of the reaction mixture which will increase the rate of the reaction. ... Increasing the concentration of reactants increases the rate of reaction. However, the amount of magnesium might be the limiting factor.
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The rate of chemical reaction is doubled for every 10oC rise in temper...
Reason for the rate of chemical reaction doubling for every 10oC rise in temperature:
Increasing the temperature of a reaction leads to an increase in the rate of the reaction. This phenomenon can be explained by the concept of activated molecules.
Activating Molecules:
- When a reaction takes place, the molecules need to overcome a certain energy barrier known as the activation energy.
- At higher temperatures, the molecules possess more kinetic energy, which increases the likelihood of them reaching the activation energy.
- As the temperature increases, the number of molecules with energy equal to or greater than the activation energy also increases. These molecules are referred to as activated molecules.
Doubling Effect:
- With every 10oC rise in temperature, the number of activated molecules doubles due to the exponential nature of the Arrhenius equation.
- This doubling effect occurs because the rate of reaction is proportional to the number of activated molecules.
- As a result, the rate of the chemical reaction doubles for every 10oC rise in temperature.
Conclusion:
- Therefore, the correct answer is an increase in the number of activated molecules (option D) as the reason behind the rate of chemical reaction doubling for every 10oC rise in temperature.
Increasing the temperature of a reaction leads to an increase in the rate of the reaction. This phenomenon can be explained by the concept of activated molecules.
Activating Molecules:
- When a reaction takes place, the molecules need to overcome a certain energy barrier known as the activation energy.
- At higher temperatures, the molecules possess more kinetic energy, which increases the likelihood of them reaching the activation energy.
- As the temperature increases, the number of molecules with energy equal to or greater than the activation energy also increases. These molecules are referred to as activated molecules.
Doubling Effect:
- With every 10oC rise in temperature, the number of activated molecules doubles due to the exponential nature of the Arrhenius equation.
- This doubling effect occurs because the rate of reaction is proportional to the number of activated molecules.
- As a result, the rate of the chemical reaction doubles for every 10oC rise in temperature.
Conclusion:
- Therefore, the correct answer is an increase in the number of activated molecules (option D) as the reason behind the rate of chemical reaction doubling for every 10oC rise in 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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