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Standard XII

Chemistry

Nernst Equation

The e.m.f. of...

Question

The e.m.f. of the cell $A g | A g C l | | K C l (a q .) | H_{2} C l_{2} | H g$ is 0.0455 K at 298 K and the temperature coefficient is $3.38 \times 10^{- 4} V K^{- 1}$ . The reaction is taking place is:

H g_{2} C l_{2} (s) + 2 A g (s) \to 2 A g C l (s) + 2 H g (l)

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H g_{2} C l_{2} (s) + 3 A g (s) \to 3 A g C l (s) + 4 H g (l)

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H g_{2} C l_{2} (s) + A g (s) \to 2 A g C l (s) + 4 H g (l)

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none of these

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Solution

The correct option is A $H g_{2} C l_{2} (s) + 2 A g (s) \to 2 A g C l (s) + 2 H g (l)$
$A g (s) | A g B r (s) | | K B r (a q .) | | H g_{2} B r_{2} (s) | H g (l)$
for the given cell, reaction of cell is
$H g_{2} B r_{2} (s)) + 2 A g (s) \to 2 H g (l) + 2 A g B r (s)$

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Similar questions

Q. What is cell entropy change of the following cell?

P t (x) | H_{2} (g) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g

P = 1 atm 0.1 M 0.1 M
Emf of the cell is found to be 0.045 V at 298 K and temperature coefficient is

3.4 \times 10^{- 4} V K^{- 1}

[Given :

K_{a (C H_{3} C O O H)} = 10^{- 5} M

]

Q. What is the cell entropy change of the following cell ?

P t (s) | H_{2} (g, 1 a t m) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g

EMF of the cell is found to be

0.0045 V

at 298 K and temperature coefficient is

3.4 \times 10^{- 4} V K^{- 1}

The electrical work done during the reaction at 298 K:
$2 H g_{(l)} + C l_{2 (g)} \to H g_{2} C l_{2 (s)}, i s G i v e n t h a t E_{\frac{C l_{2}}{C l^{-}}}^{\circ} = 1.36 V; E_{\frac{H g_{2} C l_{2}}{H g, C l^{-}}}^{\circ} = 0.27 V; P_{C l_{2}} = 1 a t m,$

Q. The standard emf of the cell

C d (s) / C d C l_{2} (a q) (0.1 M) | | A g C l (s) | A g (s)

in which the cell-reaction is

C d (s) + 2 A g C l (s) \to 2 A g (s) + C d^{2 +} (a q) + 2 C l^{-} (a q)

0.6915

V at

273

K and

0.6573

V at

298

K. Calculate enthalpy change of the reaction at

298

K is?

Δ G^{\circ}

of the cell reaction,

A g C l (s) + \frac{1}{2} H_{2} (g) \to A g (s) + H^{+} + C l^{-} is - 21.52 K J . Δ G^{\circ} of 2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} 2 C l^{-}

is:

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The e.m.f. of the cell Ag|AgCl||KCl(aq.)|H2Cl2|Hg is 0.0455 K at 298 K and the temperature coefficient is 3.38×10−4VK−1. The reaction is taking place is:

The correct option is A Hg2Cl2(s)+2Ag(s)→2AgCl(s)+2Hg(l)Ag(s)|AgBr(s)||KBr(aq.)||Hg2Br2(s)|Hg(l) for the given cell, reaction of cell is Hg2Br2(s))+2Ag(s)→2Hg(l)+2AgBr(s)

The e.m.f. of the cell $A g | A g C l | | K C l (a q .) | H_{2} C l_{2} | H g$ is 0.0455 K at 298 K and the temperature coefficient is $3.38 \times 10^{- 4} V K^{- 1}$ . The reaction is taking place is:

The correct option is A $H g_{2} C l_{2} (s) + 2 A g (s) \to 2 A g C l (s) + 2 H g (l)$
$A g (s) | A g B r (s) | | K B r (a q .) | | H g_{2} B r_{2} (s) | H g (l)$
for the given cell, reaction of cell is
$H g_{2} B r_{2} (s)) + 2 A g (s) \to 2 H g (l) + 2 A g B r (s)$