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 $25^{0} C$ .
$[K_{s p} (A g C l) = 2.8 \times 10^{- 10}, K_{s p} (A g B r) = 3.3 \times 10^{- 13}]$

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Solution

$A g / A g C l$ (s), $K C l (0.2 M) ∥ K B r (0.001 M); A g B r$ (s) $/ A g$
${A g}_{(1)} ⟶ {A g}_{(1)}^{+} + e^{-}$ (at anode)
${A g}_{(2)} ⟶ {A g}_{(2)}^{+} + e^{-}$ (at cathode)
${A g}_{(1)} + {A g}_{(2)}^{+} ⟶ {A g}_{(2)} + {A g}_{(1)}^{+}$ (cell reaction)
According to Nemest Reaction,
$E_{c e l l} = E_{c e l l}^{0} + 0.06 l o g [\frac{r e a c t a n t s}{p r o d u c t}]$
$K s p [A g C l] = [{A g}_{(1)}^{+}] [{C l}^{-}] = 2.8 \times 10^{10}$
$K s p [A g B r] = [{A g}_{(2)}^{+}] [{B r}^{-}] = 3.3 \times 10^{- 13} [{A g}_{(2)}^{+}] = \frac{.3 \times 10^{- 13}}{0.001} = 3.3 \times 10^{- 10} M E_{c e l l} = 0.0591 l o g \frac{[2.3 \times 10^{- 10}]}{[1.4 \times 10^{- 9}]} = - 0.037 V$
$e m f < 0,$ cell eaction $(E_{c e l l} > 0)$ polarity of cell is to reversed, ie.
$A g / A g B r$ (s), $K B r (0.001 M) ∥ K C l (0.2 M), A g C l$ (s) $/ A g$

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Similar questions

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 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 =

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 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}

A g | A g {B r}_{(s)}, K B r (0.01 M) ∥ K C l (0.002 M), A g {C l}_{(s)} | {A g}_{(s)}

. Calculate the EMF of given cell at

25^{o} C

:
[Given:

K_{s p (A g C l)} = 4.8 \times 10^{- 10} M^{2}, K_{s p (A g B r)} = 2.4 \times 10^{- 14} M^{2}

and

\frac{2.303 R T}{F} = 0.06

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For the galvanic cell,Ag|AgCl(s),KCl(0.2M)||KBr(0.001M),AgBr(s)|Ag Calculate the emf generated and assign correct polarity to each electrode for a spontaneous process after taking into account the cell reaction at 250C.[Ksp(AgCl)=2.8×10−10,Ksp(AgBr)=3.3×10−13]