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To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.
Correct answer is between '0.31,0.33'. Can you explain this answer?
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To find the standard potential of M3+/M electrode, the following cell ...
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To find the standard potential of M3+/M electrode, the following cell ...
/L)||M2 (unknown concentration)|Pt
The standard potential of the M3 /M electrode can be determined by measuring the cell potential (Ecell) of the above-mentioned cell and using the Nernst equation.
The cell potential can be measured using a voltmeter or a potentiometer. Let's assume that the measured cell potential is 0.56 V.
The Nernst equation relates the cell potential to the standard potential (E°) and the concentrations of the species involved in the cell reaction. For the given cell, the cell reaction is:
M3 + e- -> M2
The Nernst equation can be written as:
Ecell = E° - (RT/nF) ln(Q)
where R is the gas constant (8.314 J/mol-K), T is the temperature in Kelvin, n is the number of electrons transferred in the cell reaction, F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient.
For the given cell, n = 1 and Q = [M2]/[M3]. Since the concentration of M2 is unknown, we cannot calculate Q directly. However, we can assume that the cell is operating under standard conditions, which means that [M2] = 1 M and [M3] = 0.0018 M. This assumption is valid since the cell is constituted using standard hydrogen electrode (SHE) as the reference electrode, which is at standard conditions.
Substituting the values in the Nernst equation, we get:
0.56 = E° - (8.314*298/1*96485) ln(1/0.0018)
Solving for E°, we get:
E° = 0.56 + (8.314*298/1*96485) ln(1/0.0018)
E° = 0.56 + 0.238
E° = 0.798 V
Therefore, the standard potential of the M3 /M electrode is 0.798 V.
The standard potential of the M3 /M electrode can be determined by measuring the cell potential (Ecell) of the above-mentioned cell and using the Nernst equation.
The cell potential can be measured using a voltmeter or a potentiometer. Let's assume that the measured cell potential is 0.56 V.
The Nernst equation relates the cell potential to the standard potential (E°) and the concentrations of the species involved in the cell reaction. For the given cell, the cell reaction is:
M3 + e- -> M2
The Nernst equation can be written as:
Ecell = E° - (RT/nF) ln(Q)
where R is the gas constant (8.314 J/mol-K), T is the temperature in Kelvin, n is the number of electrons transferred in the cell reaction, F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient.
For the given cell, n = 1 and Q = [M2]/[M3]. Since the concentration of M2 is unknown, we cannot calculate Q directly. However, we can assume that the cell is operating under standard conditions, which means that [M2] = 1 M and [M3] = 0.0018 M. This assumption is valid since the cell is constituted using standard hydrogen electrode (SHE) as the reference electrode, which is at standard conditions.
Substituting the values in the Nernst equation, we get:
0.56 = E° - (8.314*298/1*96485) ln(1/0.0018)
Solving for E°, we get:
E° = 0.56 + (8.314*298/1*96485) ln(1/0.0018)
E° = 0.56 + 0.238
E° = 0.798 V
Therefore, the standard potential of the M3 /M electrode is 0.798 V.
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To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer?
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To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer?.
To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer?.
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ample number of questions to practice To find the standard potential of M3+/M electrode, the following cell is constituted. Pt|M|M3+ (0.0018 mol–1L) || Ag+ (0.01 mol–1L)|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the anode half (up to two decimal places). Given E0Ag+|Ag = 0.80 Volt.Correct answer is between '0.31,0.33'. Can you explain this answer? tests, examples and also practice Chemistry tests.
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