The standard electrode potentials for the reactionsAg+ (a) + e– ⎯⎯→ Ag(s) Sn2+ (a) + 2e– ⎯⎯→ Sn (s)at 25 °C are 0.80 volt and –0.14 volt, respectively. The standard emf of the cell formed by thesehalf-cells is
Question
The standard electrode potentials for the reactionsAg+ (a) + e– ⎯⎯→ Ag(s) Sn2+ (a) + 2e– ⎯⎯→ Sn (s)at 25 °C are 0.80 volt and –0.14 volt, respectively. The standard emf of the cell formed by thesehalf-cells is
Solution
To find the standard emf of the cell formed by these half-cells, we can use the formula:
Ecell = Ered(cathode) - Ered(anode)
where Ered(cathode) is the reduction potential of the cathode and Ered(anode) is the reduction potential of the anode.
Given that the reduction potential of Ag+ (a) + e– ⎯⎯→ Ag(s) is 0.80 volt and the reduction potential of Sn2+ (a) + 2e– ⎯⎯→ Sn (s) is -0.14 volt, we can substitute these values into the formula:
Ecell = 0.80 V - (-0.14 V) Ecell = 0.94 V
Therefore, the standard emf of the cell formed by these half-cells is 0.94 volts.
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