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In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason that
- a)collision frequency increases by a factor of 2 to 3.
- b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.
- c)Activation energy is lowered by a factor of 2 to 3.
- d)none of these
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
In most cases, for a rise of 10K temperature the rate constant is dou...
Explanation:
The rate constant, k, is a measure of the reaction rate and is dependent on temperature. The Arrhenius equation describes the relationship between the rate constant and temperature:
k = Ae^(-Ea/RT)
where A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.
For a rise of 10K temperature, the rate constant is doubled to tripled. This is due to the reason that the fraction of molecules possessing threshold energy increases by a factor of 2 to 3.
Collision Frequency:
The collision frequency is the number of collisions that occur per unit time. As the temperature increases, the collision frequency increases, but this is not the main reason for the increase in the rate constant.
Fraction of Molecules Possessing Threshold Energy:
The main reason for the increase in the rate constant with temperature is that the fraction of molecules possessing threshold energy increases. The threshold energy is the minimum energy required for a collision to result in a reaction. As the temperature increases, more molecules have sufficient energy to overcome the activation energy barrier and react. The fraction of molecules possessing threshold energy increases by a factor of 2 to 3 for a rise of 10K temperature, leading to a corresponding increase in the rate constant.
Activation Energy:
The activation energy is the minimum energy required for a reaction to occur. As the temperature increases, the activation energy is lowered due to the increased thermal energy of the molecules. However, the effect of the increase in the fraction of molecules possessing threshold energy is much larger than the effect of the decrease in activation energy.
Conclusion:
In summary, for a rise of 10K temperature, the rate constant is doubled to tripled due to the increase in the fraction of molecules possessing threshold energy. The collision frequency and activation energy also play a role, but to a lesser extent.
The rate constant, k, is a measure of the reaction rate and is dependent on temperature. The Arrhenius equation describes the relationship between the rate constant and temperature:
k = Ae^(-Ea/RT)
where A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.
For a rise of 10K temperature, the rate constant is doubled to tripled. This is due to the reason that the fraction of molecules possessing threshold energy increases by a factor of 2 to 3.
Collision Frequency:
The collision frequency is the number of collisions that occur per unit time. As the temperature increases, the collision frequency increases, but this is not the main reason for the increase in the rate constant.
Fraction of Molecules Possessing Threshold Energy:
The main reason for the increase in the rate constant with temperature is that the fraction of molecules possessing threshold energy increases. The threshold energy is the minimum energy required for a collision to result in a reaction. As the temperature increases, more molecules have sufficient energy to overcome the activation energy barrier and react. The fraction of molecules possessing threshold energy increases by a factor of 2 to 3 for a rise of 10K temperature, leading to a corresponding increase in the rate constant.
Activation Energy:
The activation energy is the minimum energy required for a reaction to occur. As the temperature increases, the activation energy is lowered due to the increased thermal energy of the molecules. However, the effect of the increase in the fraction of molecules possessing threshold energy is much larger than the effect of the decrease in activation energy.
Conclusion:
In summary, for a rise of 10K temperature, the rate constant is doubled to tripled due to the increase in the fraction of molecules possessing threshold energy. The collision frequency and activation energy also play a role, but to a lesser extent.
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Community Answer
In most cases, for a rise of 10K temperature the rate constant is dou...
For a 10 K rise in temperature, collision frequency increases merely by 1 to 2% but the number of effective collisions increases by 100 to 200%.
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In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer?
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In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer?.
In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason thata)collision frequency increases by a factor of 2 to 3.b)fraction of molecules possessing threshold energy increases by a factor of 2 to 3.c)Activation energy is lowered by a factor of 2 to 3.d)none of theseCorrect answer is option 'B'. Can you explain this answer?.
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