At a certain temperature, the first order rate constant k1 is found to be smaller than the second order rate constant k2. If the energy of activation E1 of the first order reaction is greater than energy of activation E2 of the second order reaction, then with increase in temperature.a)k1 will increase faster than k2, but always will remain less than k2.b)k2 will increase faster than k1c)k1 will increase faster than k2 and becomes equal to k2.d)k1 will increase faster k2 and becomes greater than k2.Correct answer is option 'A'. Can you explain this answer?

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At a certain temperature, the first order rate constant k₁ is found to be smaller than the second order rate constant k₂. If the energy of activation E₁ of the first order reaction is greater than energy of activation E₂ of the second order reaction, then with increase in temperature.

a)
k₁ will increase faster than k₂, but always will remain less than k₂.
b)
k₂ will increase faster than k₁
c)
k₁ will increase faster than k₂ and becomes equal to k₂.
d)
k₁ will increase faster k₂ and becomes greater than k₂.

Correct answer is option 'A'. Can you explain this answer?

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Introduction:
The rate constant is a measure of the speed of a chemical reaction. It is influenced by factors such as temperature and activation energy. In this question, we are given that the first order rate constant (k1) is smaller than the second order rate constant (k2) at a certain temperature. We are also told that the energy of activation (E1) for the first order reaction is greater than the energy of activation (E2) for the second order reaction. We need to determine how these rate constants will change with an increase in temperature.

Explanation:
When the temperature is increased, the rate constant for a reaction generally increases. This is because an increase in temperature leads to an increase in the kinetic energy of the reactant molecules, which in turn increases the frequency and energy of successful collisions.

Effect of temperature on rate constants:
- As the temperature increases, the rate constant for a first order reaction (k1) will increase at a faster rate compared to the rate constant for a second order reaction (k2). This is because the increase in temperature has a greater effect on the rate of a first order reaction than on the rate of a second order reaction.
- However, even with the increase in temperature, the first order rate constant (k1) will always remain less than the second order rate constant (k2). This is because the energy of activation (E1) for the first order reaction is greater than the energy of activation (E2) for the second order reaction.
- Therefore, option 'A' is the correct answer.

Reasoning:
- The rate constant for a first order reaction is given by the Arrhenius equation: k1 = Ae^(-E1/RT), where A is the pre-exponential factor, E1 is the energy of activation, R is the gas constant, and T is the temperature.
- The rate constant for a second order reaction is given by the Arrhenius equation: k2 = Ae^(-E2/RT), where A is the pre-exponential factor, E2 is the energy of activation, R is the gas constant, and T is the temperature.
- As the temperature increases, the exponential term in both equations becomes larger, leading to an increase in the rate constants.
- However, since the energy of activation for the first order reaction is greater than the energy of activation for the second order reaction (E1 > E2), the increase in temperature has a bigger effect on the rate constant for the first order reaction (k1) compared to the rate constant for the second order reaction (k2).
- Therefore, with an increase in temperature, k1 will increase faster than k2, but it will always remain less than k2.

Conclusion:
- The rate constant for a first order reaction will increase faster than the rate constant for a second order reaction with an increase in temperature.
- However, the first order rate constant will always remain less than the second order rate constant due to the difference in energy of activation between the two reactions.

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At a certain temperature, the first order rate constant k1 is found to be smaller than the second order rate constant k2. If the energy of activation E1 of the first order reaction is greater than energy of activation E2 of the second order reaction, then with increase in temperature.a)k1 will increase faster than k2, but always will remain less than k2.b)k2 will increase faster than k1c)k1 will increase faster than k2 and becomes equal to k2.d)k1 will increase faster k2 and becomes greater than k2.Correct answer is option 'A'. Can you explain this answer?

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At a certain temperature, the first order rate constant k1 is found to be smaller than the second order rate constant k2. If the energy of activation E1 of the first order reaction is greater than energy of activation E2 of the second order reaction, then with increase in temperature.a)k1 will increase faster than k2, but always will remain less than k2.b)k2 will increase faster than k1c)k1 will increase faster than k2 and becomes equal to k2.d)k1 will increase faster k2 and becomes greater than k2.Correct answer is option 'A'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about At a certain temperature, the first order rate constant k1 is found to be smaller than the second order rate constant k2. If the energy of activation E1 of the first order reaction is greater than energy of activation E2 of the second order reaction, then with increase in temperature.a)k1 will increase faster than k2, but always will remain less than k2.b)k2 will increase faster than k1c)k1 will increase faster than k2 and becomes equal to k2.d)k1 will increase faster k2 and becomes greater than k2.Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At a certain temperature, the first order rate constant k1 is found to be smaller than the second order rate constant k2. If the energy of activation E1 of the first order reaction is greater than energy of activation E2 of the second order reaction, then with increase in temperature.a)k1 will increase faster than k2, but always will remain less than k2.b)k2 will increase faster than k1c)k1 will increase faster than k2 and becomes equal to k2.d)k1 will increase faster k2 and becomes greater than k2.Correct answer is option 'A'. Can you explain this answer?.

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