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A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :
- a)Both ∆H and ∆S are negative.
- b)Both ∆H and ∆S are positive.
- c)∆H is positive while ∆S is negative.
- d)∆H is negative while ∆S is positive
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
A reaction at 1 bar is non-spontaneous at low temperature but becomes ...
Explanation:
In order to understand why option B is the correct answer, we need to examine the relationship between enthalpy (H) and entropy (S) in determining the spontaneity of a reaction.
Gibbs Free Energy (G) and Spontaneity:
The spontaneity of a reaction can be determined by calculating the change in Gibbs free energy (ΔG). The equation for ΔG is as follows:
ΔG = ΔH - TΔS
Where:
ΔG is the change in Gibbs free energy
ΔH is the change in enthalpy
T is the temperature in Kelvin
ΔS is the change in entropy
If ΔG is negative, the reaction is spontaneous. If ΔG is positive, the reaction is non-spontaneous. And if ΔG is zero, the reaction is at equilibrium.
Effect of Temperature on Spontaneity:
Temperature plays a crucial role in determining the spontaneity of a reaction. The relationship between temperature and spontaneity can be understood by examining the ΔG equation.
At low temperatures, the TΔS term in the equation dominates, as temperature is relatively small. Therefore, for a reaction to be spontaneous at low temperatures, the ΔS term must be positive (ΔS > 0).
However, at high temperatures, the TΔS term becomes significant, and the ΔH term also plays a role. In order for the reaction to become spontaneous at high temperatures, the TΔS term must be greater than the ΔH term, meaning that both terms must be positive (ΔH > 0 and ΔS > 0).
Conclusion:
Based on the information provided, we can conclude that option B is correct, which states that both H and S are positive. This is because the reaction is non-spontaneous at low temperatures, indicating a negative ΔG, which requires a positive ΔS term. And at high temperatures, the reaction becomes spontaneous, indicating a positive ΔG, which requires both a positive ΔH and ΔS term.
Therefore, it can be inferred that the reaction has a positive enthalpy change (H) and a positive entropy change (S), leading to the correct answer being option B.
In order to understand why option B is the correct answer, we need to examine the relationship between enthalpy (H) and entropy (S) in determining the spontaneity of a reaction.
Gibbs Free Energy (G) and Spontaneity:
The spontaneity of a reaction can be determined by calculating the change in Gibbs free energy (ΔG). The equation for ΔG is as follows:
ΔG = ΔH - TΔS
Where:
ΔG is the change in Gibbs free energy
ΔH is the change in enthalpy
T is the temperature in Kelvin
ΔS is the change in entropy
If ΔG is negative, the reaction is spontaneous. If ΔG is positive, the reaction is non-spontaneous. And if ΔG is zero, the reaction is at equilibrium.
Effect of Temperature on Spontaneity:
Temperature plays a crucial role in determining the spontaneity of a reaction. The relationship between temperature and spontaneity can be understood by examining the ΔG equation.
At low temperatures, the TΔS term in the equation dominates, as temperature is relatively small. Therefore, for a reaction to be spontaneous at low temperatures, the ΔS term must be positive (ΔS > 0).
However, at high temperatures, the TΔS term becomes significant, and the ΔH term also plays a role. In order for the reaction to become spontaneous at high temperatures, the TΔS term must be greater than the ΔH term, meaning that both terms must be positive (ΔH > 0 and ΔS > 0).
Conclusion:
Based on the information provided, we can conclude that option B is correct, which states that both H and S are positive. This is because the reaction is non-spontaneous at low temperatures, indicating a negative ΔG, which requires a positive ΔS term. And at high temperatures, the reaction becomes spontaneous, indicating a positive ΔG, which requires both a positive ΔH and ΔS term.
Therefore, it can be inferred that the reaction has a positive enthalpy change (H) and a positive entropy change (S), leading to the correct answer being option B.
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A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer?
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A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer?.
A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :a)Both H and S are negative.b)Both H and S are positive.c)H is positive while S is negative.d)H is negative while S is positiveCorrect answer is option 'B'. Can you explain this answer?.
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