Respuesta :
Answer:
3.17 V
Explanation:
The cell is operating under standard conditions. These standard conditions include; that the reaction takes place at 298 Kelvin (room temperature), the pressure of the system is 1 atmosphere (standard pressure), and the solutions have a Molarity of 1.0 M for both the anode and cathode solutions. All these conditions are satisfied in the cell under review in the question.
Hence;
EĀ°anode (magnesium)= -2.37 V
EĀ°cathode (silver) = 0.80 V
EĀ°cell= EĀ°cathode -EĀ°anode
EĀ°cell= 0.80-(-2.37)
EĀ°cell= 0.80 + 2.37
EĀ°cell= 3.17 V
Hence the standard cell potential of this cell at 25Ā°C is 3.17 V
Answer:
The standard potential at 25ĀŗC is 3.17 V.
Explanation:
The anode in Ā a galvanic cell is the electrode at which oxidation occurs and the cathode is the electrode Ā at which reduction occurs.
The overall cell reaction Ā will be the sum of two half-cell reactions. The standard reduction potentials are:
MgĀ²āŗ (1.0 M) + 2eā» Ā ā Ā Mg (s) Ā Ā Ā Ā Ā EĀŗ = -2.37
Agāŗ (1.0 M) + eā» ā Ag (s) Ā Ā Ā Ā Ā Ā Ā Ā EĀŗ= +0.80
Since the reactants are in their standard states (1.0 M) and at 25ĀŗC we can write the half-cell reactions as follows:
Anode (oxidation): Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Mg (s) ā MgĀ²āŗ (1.0 M) + 2eā»
Cathode (reduction): Ā Ā 2Agāŗ (1.0 M) + 2eā» ā 2Ag (s)
Overall: Ā Ā Ā Ā Ā Ā Mg (s) +2 Agāŗ (1.0 M) + 2eā» ā 2Ag (s) + MgĀ²āŗ (1.0 M) + 2eā»
In order to balance the overall equation we multiply the reduction of Ā Agāŗ by 2. We can do so because, as an intensive property, EĀ° is not affected by Ā this procedure.
The standard emf of the cell, EĀ°cell , which is composed of a contribution Ā from the anode and a contribution from the cathode, is given by:
[tex] EĀŗ cell = EĀŗ cathode - EĀŗ anode [/tex]
[tex] EĀŗ cell = EĀŗAgāŗ/Ag - EĀŗ MgĀ²āŗ/Mg [/tex]
[tex] EĀŗ cell =0.80 V - (-2.37 V) [/tex]
EĀŗ cell = 3.17 V
