Represent the cell in which the following reaction takes place:Mg(s) + 2Ag+ (0.0001 M) → Mg2+(0.130 m) + 2Ag(s)Calculate its E(cell), if E°cell = 3.17 V. - Zigya

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Represent the cell in which the following reaction takes place:
Mg(s) + 2Ag⁺ (0.0001 M) → Mg²⁺(0.130 m) + 2Ag(s)
Calculate its E_(cell), if E°_cell = 3.17 V.

The cell is
Mg(s) | Mg²⁺(aq) (0.130 M) || Ag⁺(aq) (0.0001 M) | Ag(s)
The Nernst equation is

E_{(cell)} = E °_{cell} - \frac{RT}{2 F} \ln \frac{[{Mg}^{2 +}]}{[{Ag}^{+}]} E_{cell} = 3.17 V - \frac{0.059 V}{n} \log [\frac{0.130}{(0.0001)^{2}}] E_{cell} = 3.17 V - \frac{0.059 V}{n} \times 7.114 E_{cell} = 3.17 V - 0.21 V E_{cell} = + 2.96 V .

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