For the galvanic cell at $25^{o} C$ ,
$A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g$

Which of the following(s) is/are true for the given cell?
Given:
$K_{s p} (A g C l) = 2.8 \times 10^{- 10}$
$K_{s p} (A g B r) = 3.3 \times 10^{- 13}$

25^{o} C, E_{c e l l} = 0.122 V

, non-spontaneous cell reaction

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25^{o} C, E_{c e l l} = - 0.037 V

, non-spontaneous cell reaction

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25^{o} C, E_{c e l l} = - 0.037 V

, spontaneous cell reaction

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25^{o} C, E_{c e l l} = 0.122 V

, spontaneous cell reaction

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Solution

The correct option is B At $25^{o} C, E_{c e l l} = - 0.037 V$ , non-spontaneous cell reaction
From cell representation,
At anode,
$A g_{L . H . S} \to A g_{L . H . S}^{+}$

At cathode,
$A g_{R . H . S}^{+} + e^{-} \to A g_{R . H . S}$

The cell reaction is
$A g_{L . H . S} + A g_{R . H . S}^{+} \to A g_{L . H . S}^{+} + A g_{R . H . S}$

Nernst equation for the given concentration cell is
$E_{c e l l} = E_{c e l l}^{0} - 0.0591 l o g \frac{A g_{L . H . S}^{+}}{A g_{R . H . S}^{+}}$
For concentration cell,
$E_{c e l l}^{0} = 0$

$E_{c e l l} = 0.0591 l o g \frac{[A g^{+}]_{R H S}}{[A g^{+}]_{L H S}} . . . . . e q n (1)$

For
$A g C l ⇌ A g^{+} + C l^{-}$
$K_{s p} (A g C l) = 2.8 \times 10^{- 10}$
$K_{s p} (A g C l) = [A g^{+}] [C l^{-}]$
$[A g^{+}] = \frac{K_{s p} (A g C l)}{[C l^{-}]}$
Concentration of $K C l$ is $0.2 M$
$∴$
$[C l^{-}] = 0.2 M$
$[A g^{+}] = \frac{2.8 \times 10^{- 10}}{0.2}$

$[A g^{+}]_{L H S} = 14 \times 10^{- 10} M$

For
$A g B r ⇌ A g^{+} + B r^{-}$
$K_{s p} (A g B r) = 3.3 \times 10^{- 13}$
$K_{s p} (A g B r) = [A g^{+}] [B r^{-}]$
$[A g^{+}] = \frac{K_{s p} (A g B r)}{[B r^{-}]}$
Concentration of $K B r$ is $0.001 M$
$∴$
$[B r^{-}] = 0.001 M$
$[A g^{+}] = \frac{3.3 \times 10^{- 13}}{0.001}$

$[A g^{+}]_{R H S} = 3.3 \times 10^{- 10} M$

Substituting $A g^{+}$ concentrations in equation (1) gives,

$E_{c e l l} = 0.0591 l o g \frac{3.3 \times 10^{- 10}}{14 \times 10^{- 10}}$

$E_{c e l l} = 0.0591 l o g 0.235$

$E_{c e l l} \approx - 0.037 V$

The emf of cell is negative, hence, the cell reaction is non-spontaneous.

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Similar questions

Q. For the galvanic cell at

25^{o} C

A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g

Which of the following(s) is/are true for the given cell?
Given:

K_{s p} (A g C l) = 2.8 \times 10^{- 10}

K_{s p} (A g B r) = 3.3 \times 10^{- 13}

For the galvanic cell :

Ag 1 AgCl(s), KCl(0.2 M)II KBr (0.001 M), AgBr(s) I Ag, the EMF (in V) generated for a spontaneous process after taking into account the cell reaction at $25^{\circ} C$ will be $37 \times 10^{- x}$ , then what is the value of x?

$[K_{s p} (A g C l) = 2.8 \times 10^{- 10}, K_{s p} A g B r) = 3.3 \times 10^{- 13}]$

Q. For the galvanic cell,

A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g

Calculate the emf generated and assign correct polarity to each electrode for the spontaneous process after taking into account the cell reaction at

25^{\circ} C

.
Given,

K_{s p A g C l} = 2.8 \times 10^{- 10}; K_{s p A g B r} = 3.3 \times 10^{- 13}

Q. For the galvanic cell,

A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g

Calculate the emf generated and assign correct polarity to each electrode for a spontaneous process after taking into account the cell reaction at

25^{0} C

[K_{s p} (A g C l) = 2.8 \times 10^{- 10}, K_{s p} (A g B r) = 3.3 \times 10^{- 13}]

Q. For the galvanic cell :

A g | A g C l (s) | K C l (0.2 M) | | K B r (0.001 M) | A g B r (s) | A g

,Calculate the EMF in V, generated and assign correct polarity to each electrode for a spontaneous process after taking into account the cell reaction at

25^{\circ} C

[K_{s p} = 2.8 \times 10^{- 10}; K_{s p (A g B r)} = 3.3 \times 10^{- 13}]

The answer is -m.n

\times 10^{- 2}

Then n-m =

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For the galvanic cell at 25oC, Ag|AgCl(s),KCl(0.2 M)||KBr(0.001 M),AgBr(s)|Ag Which of the following(s) is/are true for the given cell? Given: Ksp(AgCl)=2.8×10−10 Ksp(AgBr)=3.3×10−13

For the galvanic cell at $25^{o} C$ ,
$A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g$

Which of the following(s) is/are true for the given cell?
Given:
$K_{s p} (A g C l) = 2.8 \times 10^{- 10}$
$K_{s p} (A g B r) = 3.3 \times 10^{- 13}$