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Arrhenius relation is described as K= A e-Ea/RT which of the following statement is correct regarding activation energy
- a)Lower activation energy reactions are more susceptible to temperature change
- b)Higher activation energy reactions are more susceptible to temperature change
- c)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally different
- d)Activation energy is of reaction is independent from temperature.
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
Arrhenius relation is described as K= A e-Ea/RTwhich of the following ...
K= 
Differentiating with respect to T
Here we can see that on increasing temperature those reaction having high value of Ea will be more susceptible to change in rate.
Hence, option (b) is correct.
Differentiating with respect to T
Here we can see that on increasing temperature those reaction having high value of Ea will be more susceptible to change in rate.
Hence, option (b) is correct.
Most Upvoted Answer
Arrhenius relation is described as K= A e-Ea/RTwhich of the following ...
Higher activation energy reactions are more susceptible to temperature change
Activation energy is the minimum amount of energy required for a reaction to occur. In the Arrhenius equation, the term Ea represents the activation energy. Here's why higher activation energy reactions are more susceptible to temperature change:
- Effect of Temperature on Reaction Rate: An increase in temperature leads to an increase in the rate of reaction for both low and high activation energy reactions. However, the effect is more pronounced for reactions with higher activation energy.
- Arrhenius Equation: The Arrhenius equation shows that the rate constant (K) of a reaction is exponentially dependent on the activation energy (Ea) and the temperature (T). A higher activation energy results in a steeper exponential increase in rate constant with temperature.
- Temperature Sensitivity: Reactions with higher activation energy have a greater sensitivity to temperature changes. This means that a small increase in temperature can have a significant impact on the rate of reaction for reactions with higher activation energy.
- Temperature Dependence: The activation energy determines how the rate of reaction changes with temperature. Higher activation energy reactions have a larger temperature dependence, making them more sensitive to changes in temperature.
Therefore, the correct statement is that higher activation energy reactions are more susceptible to temperature change, as they exhibit a greater increase in reaction rate with temperature compared to reactions with lower activation energy.
Activation energy is the minimum amount of energy required for a reaction to occur. In the Arrhenius equation, the term Ea represents the activation energy. Here's why higher activation energy reactions are more susceptible to temperature change:
- Effect of Temperature on Reaction Rate: An increase in temperature leads to an increase in the rate of reaction for both low and high activation energy reactions. However, the effect is more pronounced for reactions with higher activation energy.
- Arrhenius Equation: The Arrhenius equation shows that the rate constant (K) of a reaction is exponentially dependent on the activation energy (Ea) and the temperature (T). A higher activation energy results in a steeper exponential increase in rate constant with temperature.
- Temperature Sensitivity: Reactions with higher activation energy have a greater sensitivity to temperature changes. This means that a small increase in temperature can have a significant impact on the rate of reaction for reactions with higher activation energy.
- Temperature Dependence: The activation energy determines how the rate of reaction changes with temperature. Higher activation energy reactions have a larger temperature dependence, making them more sensitive to changes in temperature.
Therefore, the correct statement is that higher activation energy reactions are more susceptible to temperature change, as they exhibit a greater increase in reaction rate with temperature compared to reactions with lower activation energy.
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Arrhenius relation is described as K= A e-Ea/RTwhich of the following ...
Option B is correct.
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Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer?
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Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer?.
Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Arrhenius relation is described as K= A e-Ea/RTwhich of the following statement is correct regarding activation energya)Lower activation energy reactions are more susceptible to temperature changeb)Higher activation energy reactions are more susceptible to temperature changec)Activation energy is thermo dynamical concept while rate is kinetic concept both are fundamentally differentd)Activation energy is of reaction is independent from temperature.Correct answer is option 'B'. Can you explain this answer?.
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