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Standard XII

Chemistry

Electrolytic Cell

The cell reac...

Question

The cell reaction of a cell is:
$M g (s) + c u^{2 +} (a q) ⇌ C u (s) + M g^{2 +} (a q)$
If the standard reduction potentials of $M g$ and $C u$ are $- 2.37$ 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 C $+ 2.71 V$
$E_{C e l l}^{\circ} = E_{C a t h o d e}^{\circ} - E_{A n o d e}^{\circ}$
$= E_{R e d u c e d s p e c i e s}^{\circ} - E_{O x i d i s e d s p e c i e s}^{\circ}$
$= 0.34 - (- 2.37) = + 2.71 V$ .

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Similar questions

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:

Q. The cell reaction of a cell is as follows:

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

. If the standard reduction potentials of

M g

and

C u

are

- 2.37

V and

+ 0.34

V respectively, the e.m.f. (in V) of the cell is:

Q. Calculate the e.m.f of the following cell reaction at

298 K

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

The standard potential

(E^{o})

of teh cell is

2.71 V

Q. (a) Calculate

△_{r} G^{0}

for the reaction.

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

Given:

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

(b) Name the type of cell which was used in Apollo space programme for providing electrical power.

Q. (a) Calculate

Δ_{r} G^{0}

for the reaction

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

.
Given:

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

(b) Name the type of cell that was used in Apollo space program for providing electrical power.

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The cell reaction of a cell is:Mg(s)+cu2+(aq)⇌Cu(s)+Mg2+(aq)If the standard reduction potentials of Mg and Cu are −2.37 and +0.34 V respectively. The emf of the cell is:

The correct option is C +2.71 VE∘Cell=E∘Cathode−E∘Anode=E∘Reduced species−E∘Oxidised species=0.34−(−2.37)=+2.71 V.

The cell reaction of a cell is:
$M g (s) + c u^{2 +} (a q) ⇌ C u (s) + M g^{2 +} (a q)$
If the standard reduction potentials of $M g$ and $C u$ are $- 2.37$ and $+ 0.34 V$ respectively. The emf of the cell is:

The correct option is C $+ 2.71 V$
$E_{C e l l}^{\circ} = E_{C a t h o d e}^{\circ} - E_{A n o d e}^{\circ}$
$= E_{R e d u c e d s p e c i e s}^{\circ} - E_{O x i d i s e d s p e c i e s}^{\circ}$
$= 0.34 - (- 2.37) = + 2.71 V$ .