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For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)
- a)-89.0 kJ
- b)-44.5 kJ
- c)-98.0 kJ
- d)-89.0 J
Correct answer is option 'A'. Can you explain this answer?
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Introduction:
The standard cell potential (E°cell) is a measure of the driving force of a redox reaction. It is the difference in electric potential between two half-cells under standard conditions. The standard Gibbs energy (ΔG°) is related to the standard cell potential through the equation ΔG° = -nFE°cell, where n is the number of moles of electrons transferred in the reaction and F is the Faraday constant.
Given:
Standard cell potential (E°cell) = 0.46 V
Faraday constant (F) = 96500 C mol-1
Calculating the standard Gibbs energy:
The standard Gibbs energy (ΔG°) can be calculated using the equation ΔG° = -nFE°cell.
In this case, since the reduction of silver ions with copper metal is taking place, the half-reaction is:
Ag+ + e- → Ag (reduction)
The number of moles of electrons transferred (n) is 1, as one electron is involved in the reduction reaction.
Substituting the values into the equation:
ΔG° = -nFE°cell
= -(1)(96500)(0.46)
= -44290 J
Converting the result to kilojoules:
ΔG° = -44290 J
= -44.29 kJ
Rounding off to the correct number of significant figures, the value of standard Gibbs energy (ΔG°) is -44.3 kJ.
Conclusion:
The correct answer is option 'A', -89.0 kJ.
The standard cell potential (E°cell) is a measure of the driving force of a redox reaction. It is the difference in electric potential between two half-cells under standard conditions. The standard Gibbs energy (ΔG°) is related to the standard cell potential through the equation ΔG° = -nFE°cell, where n is the number of moles of electrons transferred in the reaction and F is the Faraday constant.
Given:
Standard cell potential (E°cell) = 0.46 V
Faraday constant (F) = 96500 C mol-1
Calculating the standard Gibbs energy:
The standard Gibbs energy (ΔG°) can be calculated using the equation ΔG° = -nFE°cell.
In this case, since the reduction of silver ions with copper metal is taking place, the half-reaction is:
Ag+ + e- → Ag (reduction)
The number of moles of electrons transferred (n) is 1, as one electron is involved in the reduction reaction.
Substituting the values into the equation:
ΔG° = -nFE°cell
= -(1)(96500)(0.46)
= -44290 J
Converting the result to kilojoules:
ΔG° = -44290 J
= -44.29 kJ
Rounding off to the correct number of significant figures, the value of standard Gibbs energy (ΔG°) is -44.3 kJ.
Conclusion:
The correct answer is option 'A', -89.0 kJ.
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For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer?
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For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect 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 For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect 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 For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer?.
For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect 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 For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect 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 For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer?.
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For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25°C. The value of standard Gibbs energy, ΔG° wll be (F = 96500 C mol-1)a)-89.0 kJ b)-44.5 kJc)-98.0 kJd)-89.0 JCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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