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Enthalpy of Solution

Consider the ...

Question

Consider the following redox reaction
$M g (s) + S n^{2 +} (a q) \to M g^{2 +} (a q) + S n (s)$
Calculate $E_{c e l l}$ for the reaction at $25^{o} C$ if $[M g^{2 +}] = 0.035 M, [S n^{2 +}] = 0.025 M$ . Calculate $Δ G$ for the cell reaction.

2.23 V & -430.39 kJ

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3.23 V & -430.39 KJ

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2.23 V & - 330.39 KJ

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None of these

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Solution

The correct option is D 2.23 V & -430.39 kJ
$M g (s) + S n^{+ 2} (a q) ⟶ M g^{2 +} (a q) + S n (s)$
$n = 2$
$E_{M g / M g^{2 +}}^{o} = 2.37$ $V$
$E_{S n^{+ 2} / S n}^{o} = - 0.14$
$E_{c e l l}^{o} = 2.37 - 0.14 = 2.23$ $V$
$E_{c e l l} = E_{c e l l}^{o} - \frac{0.06}{2} log (\frac{M g^{2 +}}{S n^{+ 2}})$
$E_{c e l l} = 2.23 - 0.03 log 1.4 \approx 2.23$ $V$
$Δ G_{r x n} = - n F E_{c e l l} = - 2 \times 96500 \times 2.23 = - 430..39$ $K J$

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Similar questions

E_{c e l l}

Δ

28^{o}

M g (s) + S n^{2 +} (0.025 M) \to M g^{2 +} (0.06 M) + S n_{(s)}

E_{c e l l}^{0} = 2.23

25^{o}

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

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

E_{{S r}^{2} + / S r}^{o} = - 2.89

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

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

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

Q is reaction quotient

l o g 2 = 0.301

25^{o} C

M g (s) | M g^{2 +} (a q, 1 \times 10^{- 4} M) E_{M g / M g^{^{2 +}}}^{0} = + 2.36 V

25^{o} C

M g (s) | M g^{2 +} (a q, 1 \times 10^{- 4} M); E_{M g / M g^{^{2 +}}}^{0} = + 2.36 V

C l_{2} (g) | C l^{-} (a q, 2 \times 10^{- 5} M); E_{C l_{2} / C l^{-}}^{0} = + 1.36 V

l o g 2 = 0.301

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