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Nernst Equation

For a cell, t...

Question

For a cell, the cell reaction is $M g (s) + C u^{2 +} (a q) \to M g^{2 +} (a q) + C u (s)$ . If the S.R.P. values of $M g$ and $C u$ are $- 2.37 V$ and $+ 0.34 V$ respectively, the EMF of the cell is:

+ 2.03 V

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- 2.03 V

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+ 2.71 V

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- 2.71 V

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Solution

The correct option is A $+ 2.71 V$
$M g^{+ 2} + 2 e \to M g; S R P = - 2.37 V$

$C u^{2 +} + 2 e \to C u; S R P = 0.34 V$

$∴$ For reaction, $M g + C u^{2 +} \to M g^{2 +} + C u$

$E_{c e l l}^{0} = E_{C u^{2 +} / C u}^{0} - E_{M g^{2 +} / M g}^{0}$
$E_{c e l l}^{0} = 0.34 - (- 2.37)$
$E_{c e l l}^{0} = 2.71 V$

Option C is correct.

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Similar questions

M g (s) + c u^{2 +} (a q) ⇌ C u (s) + M g^{2 +} (a q)

M g

C u

- 2.37

+ 0.34 V

△_{r} G^{0}

M g (s) + C u^{2 +} (a q) \to M g^{2 +} (a q) + C u (s)

E_{c e l l}^{0} = + 2.71 V, 1 F = 96500 C m o l^{- 1}

Δ_{r} G^{0}

M g (s) + {C u}^{2 +} (a q) \to {M g}^{2 +} (a q) + C u (s)

E_{c e l l}^{0} = 2.71 V, 1 F = 96500 C {m o l}^{- 1}

The voltage of a cell whose halfcells are given below is:

$M g^{2 +} + 2 e^{-} \to M g (s); E^{0} = - 2.37 V$

$C u^{2 +} + 2 e^{-} \to C u (s); E^{0} = + 0.34 V$ standard EMF of the cell is:

298 K

{M g}_{(s)} + {C u}^{2 +} (0.0001 M) \to {M g}^{2 +} (0.001 M) + {C u}_{(s)}

(E^{o})

2.71 V

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