Consider the following reaction -Mg -2 Ag - 2 Ag - Mg 2-E 0 Mg 2- Mg -2-36 V - E 0 Ag - Ag -0-80 V- The cell potential for this cell will be-A- 1-56 VB- -3-16 VC- 3-16 VD- -1-56 V

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Consider the ...

Question

Consider the following reaction :

Mg + 2Ag⁺ â†" 2 Ag + Mg²⁺

_E⁰_Mg2+/Mg= -2.36 V,_E⁰_Ag+/Ag= 0.80 V. The cell potential for this cell will be:

-3.16 V

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1.56 V

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3.16 V

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-1.56 V

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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_{(} 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 + 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}

M g (s) + 2 A g^{+} (a q .) ⇌ M g^{2 +} (a q .) + 2 A g (s)

E_{c e l l}^{\circ}

+ 3.17 V

298 K

E_{c e l l}, △ G^{\circ}

Q

A g^{+}

M g^{2 +}

0.001 M

0.02 M

M g (s) + 2 A g^{+} (0.0001 M) \to M g^{2 +} (0.130 M) + 2 A g (s)

E_{(c e l l)} if E_{(c e l l)}^{o} = 3.17 V

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