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Statement-1 : In a reversible endothermic reaction, Eact of forward reaction is higher than that of backward reaction
Statement-2 : The threshold energy of forward reaction is more than that of backward reaction
- a)If both the statements are true and statement-2 is the correct explanation of satement-1.
- b)If both the statements are true and statement-2 is not the correct explanation of satement-1.
- c)If statement-1 is True and statement-2 is False.
- d)If statement-1 is False and statement-2 is True.
Correct answer is option 'A'. Can you explain this answer?
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Statement-1: In a reversible endothermic reaction, Eactof forward reac...
Statement-1: In a reversible endothermic reaction, the activation energy of the forward reaction is higher than that of the backward reaction.
Statement-2: The threshold energy of the forward reaction is more than that of the backward reaction.
To determine the correctness and the relationship between the two statements, let's analyze each statement separately.
Statement-1: In a reversible endothermic reaction, the activation energy of the forward reaction is higher than that of the backward reaction.
Explanation: In a reversible reaction, reactants can form products, but products can also revert back to reactants. The forward reaction occurs when reactants convert into products, while the backward reaction occurs when products convert into reactants. In an endothermic reaction, energy is absorbed from the surroundings, resulting in an increase in the energy of the system.
For the forward reaction to occur, the reactant molecules need to overcome a certain energy barrier called the activation energy (Eact). This energy barrier represents the minimum energy required for the reactant molecules to reach the transition state, where the bonds are partially broken and partially formed.
Since the forward reaction in an endothermic reaction requires the reactant molecules to absorb energy and overcome a higher energy barrier, the activation energy of the forward reaction is indeed higher than that of the backward reaction. This is because the reactants have to absorb energy from the surroundings to reach the transition state and form products.
Statement-2: The threshold energy of the forward reaction is more than that of the backward reaction.
Explanation: The threshold energy (also known as the activation energy) is the minimum energy required for a reaction to occur. It represents the energy barrier that reactant molecules must overcome in order to form products.
If the threshold energy of the forward reaction is higher than that of the backward reaction, it means that the forward reaction requires more energy for the reaction to proceed. This is consistent with the concept of an endothermic reaction, where energy is absorbed from the surroundings.
Relationship between the Statements:
Statement-2 provides the correct explanation for Statement-1. The higher activation energy of the forward reaction in a reversible endothermic reaction is directly related to the fact that the forward reaction requires more energy (threshold energy) for the reaction to occur. Therefore, both statements are true, and Statement-2 is the correct explanation for Statement-1.
Conclusion:
The correct answer is option 'A': If both the statements are true and Statement-2 is the correct explanation of Statement-1.
Statement-2: The threshold energy of the forward reaction is more than that of the backward reaction.
To determine the correctness and the relationship between the two statements, let's analyze each statement separately.
Statement-1: In a reversible endothermic reaction, the activation energy of the forward reaction is higher than that of the backward reaction.
Explanation: In a reversible reaction, reactants can form products, but products can also revert back to reactants. The forward reaction occurs when reactants convert into products, while the backward reaction occurs when products convert into reactants. In an endothermic reaction, energy is absorbed from the surroundings, resulting in an increase in the energy of the system.
For the forward reaction to occur, the reactant molecules need to overcome a certain energy barrier called the activation energy (Eact). This energy barrier represents the minimum energy required for the reactant molecules to reach the transition state, where the bonds are partially broken and partially formed.
Since the forward reaction in an endothermic reaction requires the reactant molecules to absorb energy and overcome a higher energy barrier, the activation energy of the forward reaction is indeed higher than that of the backward reaction. This is because the reactants have to absorb energy from the surroundings to reach the transition state and form products.
Statement-2: The threshold energy of the forward reaction is more than that of the backward reaction.
Explanation: The threshold energy (also known as the activation energy) is the minimum energy required for a reaction to occur. It represents the energy barrier that reactant molecules must overcome in order to form products.
If the threshold energy of the forward reaction is higher than that of the backward reaction, it means that the forward reaction requires more energy for the reaction to proceed. This is consistent with the concept of an endothermic reaction, where energy is absorbed from the surroundings.
Relationship between the Statements:
Statement-2 provides the correct explanation for Statement-1. The higher activation energy of the forward reaction in a reversible endothermic reaction is directly related to the fact that the forward reaction requires more energy (threshold energy) for the reaction to occur. Therefore, both statements are true, and Statement-2 is the correct explanation for Statement-1.
Conclusion:
The correct answer is option 'A': If both the statements are true and Statement-2 is the correct explanation of Statement-1.
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Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer?
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Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. 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 Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer?.
Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. 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 Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer?.
Solutions for Statement-1: In a reversible endothermic reaction, Eactof forward reaction is higher than that of backward reactionStatement-2: The threshold energy of forward reaction is more than that of backward reactiona)If both the statements are true and statement-2 is the correct explanation of satement-1.b)If both the statements are true and statement-2 is not the correct explanation of satement-1.c)If statement-1 is True and statement-2 is False.d)If statement-1 is False and statement-2 is True.Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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