Represent the cell in which the following reaction takes place Mg s - 2Ag - 0-0001M - Mg2 - 0-130M - 2Ag s Calculate its E cell if E cello - 3-17V

Mg+2Ag+(0.0001M)⟶ Mg^2+(0.130M)+2Ag E_cell=E^o 0.05912log[(Mg^2+)(Ag^+)^2] E_cell=8.17 0.05912log[0.13010^ 8]=2.959 V ...

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Represent the...

Question

Represent the cell in which the following reaction takes place $M g (s) + 2 A g^{+} (0.0001 M) \to M g^{2 +} (0.130 M) + 2 A g (s)$
Calculate its $E_{(c e l l)} if E_{(c e l l)}^{o} = 3.17 V$

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M g_{(} s) + 2 A g^{+} (0.0001 M) ⇌ M g^{2 +} (0.130 M) + 2 A g_{(s)}

E_{(c e l l)} E_{(c e l l)}^{0} = 3.17 v o l t

M g_{(s)} + 2 A g^{+} (0.0001 M) \to M g^{+ 2} (0.120 M) + 2 A g (s) if E_{c e l l}^{\circ} = 3.17 v o l t

E_{c e l l}

(M g_{(s)}) + 2 A g^{+} (0.001 M) \to M g^{2 +} (0.130 M) + 2 A g_{(s)}

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E_{c e l l}^{o} = 3.17

M g_{(s)} + 2 A g_{(a q)}^{+} \to M g_{(a q)}^{2 +} + 2 A g_{(s)}

E_{M g^{2 +} / M g}^{0} = - 2.37 V

E_{A g^{+} / A g}^{0} = 0.80 V

[M g^{2 +}] = 0.001 M; [A g^{+}] = 0.0001 M

M g + 2 {A g}^{+} (0.0001 M) \to {M g}^{2 +} (0.01 M) + 2 A g

E_{c e l l}^{o} = 3.177 V

E_{c e l l}

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