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Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be?
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Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potent...
Understanding Delta G Not (ΔG°) and Standard Potential
To determine the standard Gibbs free energy change (ΔG°) for the reaction involving silver (Ag) and hydrogen (H2), we can use the relationship between ΔG° and the standard cell potential (E°).
Key Formula
- The formula is given by:
ΔG° = -nFE°
Where:
- n = number of moles of electrons exchanged
- F = Faraday's constant (approximately 96485 C/mol)
- E° = standard electrode potential (in volts)
Identifying Parameters
- E° for Silver Half-Cell:
Given as 0.8 V for the reduction of Ag+ to Ag.
- Electrons Transferred (n):
For the reaction:
1/2 H2 + Ag+ → H+ + Ag
The transfer of electrons involves 1 mole of electrons.
Calculating ΔG°
1. Substituting Values:
Using n = 1, F = 96485 C/mol, and E° = 0.8 V:
ΔG° = - (1)(96485)(0.8)
2. Final Calculation:
ΔG° = - 77188 J/mol
(or -77.2 kJ/mol after converting from J to kJ)
Conclusion
- The ΔG° for the reaction Ag + 1/2 H2 → H + Ag is approximately -77.2 kJ/mol.
- A negative ΔG° indicates that the reaction is spontaneous under standard conditions.
This relationship between Gibbs free energy and cell potential is crucial in electrochemistry, highlighting the spontaneity of redox reactions.
To determine the standard Gibbs free energy change (ΔG°) for the reaction involving silver (Ag) and hydrogen (H2), we can use the relationship between ΔG° and the standard cell potential (E°).
Key Formula
- The formula is given by:
ΔG° = -nFE°
Where:
- n = number of moles of electrons exchanged
- F = Faraday's constant (approximately 96485 C/mol)
- E° = standard electrode potential (in volts)
Identifying Parameters
- E° for Silver Half-Cell:
Given as 0.8 V for the reduction of Ag+ to Ag.
- Electrons Transferred (n):
For the reaction:
1/2 H2 + Ag+ → H+ + Ag
The transfer of electrons involves 1 mole of electrons.
Calculating ΔG°
1. Substituting Values:
Using n = 1, F = 96485 C/mol, and E° = 0.8 V:
ΔG° = - (1)(96485)(0.8)
2. Final Calculation:
ΔG° = - 77188 J/mol
(or -77.2 kJ/mol after converting from J to kJ)
Conclusion
- The ΔG° for the reaction Ag + 1/2 H2 → H + Ag is approximately -77.2 kJ/mol.
- A negative ΔG° indicates that the reaction is spontaneous under standard conditions.
This relationship between Gibbs free energy and cell potential is crucial in electrochemistry, highlighting the spontaneity of redox reactions.
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Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be?
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Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be? 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 Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be?.
Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be? 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 Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Delta G not for reaction Ag 1/2 H2 gives H Ag where standard potential for silver half cell reaction is 0.8V will be?.
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