For the reaction
$2 A g C l (s) + H_{2} (g) (1 a t m) \overset{}{\to} 2 A g (s) + 2 H^{+} (0.1 M) + 2 C l^{-} (0.1 M), ∆ G^{o} = - 43600 J a t 25^{o} C$
Calculate the e.m.f. of the cell.
[log 10^–n = – n]

Solution

$G i v e n : 2 A g C l (s) + H_{2} (g) (1 a t m) \overset{}{\to} 2 A g (s) + 2 H^{+} + 2 C l^{-} ∆ G^{o} = - 43600 J T = 25^{o} C = 298 K W e k n o w, ∆ G^{o} = - n F E_{c e l l}^{°} n = 2 ∴ E_{c e l l}^{°} = \frac{∆ G^{o}}{n F} = \frac{- (- 43600)}{2 x 96500} = 0.226 V E_{c e l l} = E_{c e l l}^{o} - \frac{0.059}{n} \log \frac{[H^{+}]^{2} [C l^{-}]^{2} [A g]}{[A g C l]^{2} [H_{2}]} = 0.226 - \frac{0.059}{2} \log {[H^{+}]}^{2} {[C l^{-}]}^{2} = 0.226 - \frac{0.059}{2} \log (0.1)^{2} (0.1)^{2} = 0.226 - \frac{0.059}{2} \log (0.1 x 0.1 x 0.1 x 0.1) = 0.226 - \frac{0.059}{2} \log 10^{- 4} = 0.226 - \frac{0.059}{2} (- 4) = 0.226 + 0.118 E_{c e l l} = 0.344 V$

Some More Questions From Electrochemistry Chapter

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Electrochemistry

For the reaction
$2 A g C l (s) + H_{2} (g) (1 a t m) \overset{}{\to} 2 A g (s) + 2 H^{+} (0.1 M) + 2 C l^{-} (0.1 M), ∆ G^{o} = - 43600 J a t 25^{o} C$
Calculate the e.m.f. of the cell.
[log 10^–n = – n]

Some More Questions From Electrochemistry Chapter

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

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Electrochemistry

For the reaction2AgCl (s) + H2 (g) (1 atm) → 2 Ag (s) + 2H+ (0.1 M) + 2Cl- (0.1 M),∆Go = - 43600 J at 25o CCalculate the e.m.f. of the cell.[log 10–n = – n]

Some More Questions From Electrochemistry Chapter

How would you determine the standard electrode potential of the system Mg2+/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°m value of water.

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

For the reaction
$2 A g C l (s) + H_{2} (g) (1 a t m) \overset{}{\to} 2 A g (s) + 2 H^{+} (0.1 M) + 2 C l^{-} (0.1 M), ∆ G^{o} = - 43600 J a t 25^{o} C$
Calculate the e.m.f. of the cell.
[log 10^–n = – n]

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.