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An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k?
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An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) an...
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An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) an...
Reactions taking Place at Each Electrode
At the copper electrode: Cu(s) → Cu2+(aq) + 2e-
At the silver electrode: Ag+(aq) + e- → Ag(s)
Overall Reaction Representing the Electrochemical Cell
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
Determining the Potential of Cell at 298 K
The standard reduction potentials for the half-reactions involved are:
Ag+(aq) + e- → Ag(s) E°red = +0.80 V
Cu2+(aq) + 2e- → Cu(s) E°red = +0.34 V
The standard cell potential, E°cell, can be calculated using the formula:
E°cell = E°reduction (cathode) - E°reduction (anode)
E°cell = E°red (Ag+) - E°red (Cu2+)
E°cell = (+0.80 V) - (+0.34 V)
E°cell = +0.46 V
The cell potential at 298 K can be calculated using the Nernst equation:
Ecell = E°cell - (0.0592/n) log Q
where Q is the reaction quotient and n is the number of electrons transferred.
At equilibrium, Q = [Cu2+]/[Ag+]^2
Ecell = +0.46 V - (0.0592/2) log ([Cu2+]/[Ag+]^2)
At 298 K, [Cu2+] = 0.1 M and [Ag+] = 0.1 M
Ecell = +0.46 V - (0.0296) log (0.1/0.1^2)
Ecell = +0.46 V - 0.0296
Ecell = +0.43 V
Therefore, the potential of the cell at 298 K is +0.43 V.
At the copper electrode: Cu(s) → Cu2+(aq) + 2e-
At the silver electrode: Ag+(aq) + e- → Ag(s)
Overall Reaction Representing the Electrochemical Cell
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
Determining the Potential of Cell at 298 K
The standard reduction potentials for the half-reactions involved are:
Ag+(aq) + e- → Ag(s) E°red = +0.80 V
Cu2+(aq) + 2e- → Cu(s) E°red = +0.34 V
The standard cell potential, E°cell, can be calculated using the formula:
E°cell = E°reduction (cathode) - E°reduction (anode)
E°cell = E°red (Ag+) - E°red (Cu2+)
E°cell = (+0.80 V) - (+0.34 V)
E°cell = +0.46 V
The cell potential at 298 K can be calculated using the Nernst equation:
Ecell = E°cell - (0.0592/n) log Q
where Q is the reaction quotient and n is the number of electrons transferred.
At equilibrium, Q = [Cu2+]/[Ag+]^2
Ecell = +0.46 V - (0.0592/2) log ([Cu2+]/[Ag+]^2)
At 298 K, [Cu2+] = 0.1 M and [Ag+] = 0.1 M
Ecell = +0.46 V - (0.0296) log (0.1/0.1^2)
Ecell = +0.46 V - 0.0296
Ecell = +0.43 V
Therefore, the potential of the cell at 298 K is +0.43 V.
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An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k?
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An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k? 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 An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k?.
An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k? 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 An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An electrochemical cell is set up by dipping Cu in (0.1m) CuSo4(aq) and ag in( 0.1m) AgNo3(aq) write the reaction taking place at each electrode and over all reaction represent the electrochemical cell and determine the potential of cell at 298 k?.
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