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Electrochemical Cells, Galvanic Cells

Which of the ...

Question

Which of the following reaction is correct for a given electrochemical cell at $25^{\circ} C$ ?
$P t (s) | B r^{-} (a q) | B r_{2} (g) | | C l_{2} (g) | C l^{-} (a q) | P t (s)$

2 B r^{-} (a q) + C l_{2} (g) \to 2 C l^{-} (a q) + B r_{2} (g)

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B r_{2} (g) + 2 C l^{-} (a q) \to 2 B r^{-} (a q) + C l_{2} (g)

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B r_{2} (g) + C l_{2} (g) \to 2 B r^{-} (a q) + 2 C l^{-} (a q)

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2 B r^{-} (a q) + 2 C l^{-} (a q) \to B r_{2} (g) + C l_{2} (g)

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Solution

The correct option is A $2 B r^{-} (a q) + C l_{2} (g) \to 2 C l^{-} (a q) + B r_{2} (g)$
For a given electrochemical cell at $25^{\circ} C$
$P t (s) | B r^{-} (a q) | B r_{2} (g) | | C l_{2} (g) | C l^{-} (a q) | P t (s)$
LHS denotes anode ,oxidation takes place:
So, anode half cell reaction :
$2 B r^{-} (a q) \to B r_{2} (g) + 2 e^{-} e q (i)$
RHS denotes cathode ,reduction takes place:
So, cathode half cell reaction :
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q) e q (i i)$
Adding both the equations:
$C l_{2} (g) + 2 B r^{-} (a q) \to 2 C l^{-} (a q) + B r_{2} (g)$

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Similar questions

25^{o} C

P t | {B r}_{2} (g) | {B r}^{-} (a q) | | {C l}^{-} (a q) | {C l}_{2} (g) | P t

P t | C l_{2} (g, 0.4 b a r) | C l^{-} (a q, 0.1 M) | | C l^{-} (a q, 0.01 M) | C l_{2} (g, 0.2 b a r) | P t

298 K

P t (s) | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | M^{4 +} (a q), M^{2 +} (a q) | P t (s)

E_{c e l l} = 0.092

\frac{[M^{2 +} (a q)]}{[M^{4 +} (a q)]} = 10^{x}

: E_{M^{4 +} / M^{2 +}}^{0} = 0.151 V; 2.303 \frac{R T}{F} = 0.059 V

25^{o} C

C l^{-} (a q) | C l_{2} (g, 1 a t m) | P t (s)

P t (s) | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | M^{4 +} (a q), M^{2 +} (a q) | P t (s)

E_{c e l l} = 0.092 V w h e n \frac{[M^{2 +} + (a q)]}{[M^{4 +} (a q)]} = 10^{x}

G i v e n : E_{M^{4 +} / M^{2 +}}^{\circ} = 0.151 V; 2.303 \frac{R T}{F} = 0.059 V

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