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Nernst Equation

Mg in the sol...

Question

Mg in the solid state $(M g_{(s)}) + 2 A g^{+} (0.001 M) \to M g^{2 +} (0.130 M) + 2 A g_{(s)}$ represent the cell. Calculate the emf of the cell at $298$ K.
Given: $E_{c e l l}^{o} = 3.17$ V.

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Solution

$M g (s) + 2 A g^{+} (0.001 M) \to M g^{+ 2} (0.130 M) + 2 A g (s)$
$T = 298 K$
$n = 2$
$E_{c e l l}^{o} = 3.17$
$E m f = E_{c e l l}^{o} - \frac{0.0591}{n} l o g \frac{[P]}{[R]}$
$E m f = 3.17 - \frac{0.0591}{2} l o g \frac{0.130}{0.001}$
$= 3.17 - \frac{0.0591}{2} (2.11)$
$= 3.17 - (0.0295) \times 2.11$
$= 3.17 - 0.0622$
$= 3.1078 V$
The EMF of the cell is $3.10 V$

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Similar questions

Q. 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)

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

Q. The following reactions occurs in the cell

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

Q. Answer the following questions:

a) Calculate the EMF of the cell for the reaction

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

b) What are fuel cells?

Q. For the cell reaction,

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 +}

concentrations of

0.001 M

0.02 M

respectively are:

Q. For the cell reaction at

25^{\circ} C

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

E_{c e l l}^{0} = + 3.17 V

E_{c e l l}, Δ G^{0} and Q

respectively , at

[A g^{+}] = 10^{- 3} M

[M g^{2 +}] = 0.02 M

Q is reaction quotient

l o g 2 = 0.301

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