- G- of the cell reaction-AgCls -12H2g- Ags-H-Cl- is -21-52 KJ- G-of 2AgCls-H2g- 2Ags-2H-2Cl- is-

AgCl(s)+12H_2(g)→ Ag(s)+H^++Cl^ , Δ G_1^0= 21.12 kJ 2AgCl(s)+H_2(g)→ 2Ag(s)+2H^++2Cl^ =2( 21.52) kJ= 43.04 kJ Therefore, the correct answer is (c). ...

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Standard XII

Chemistry

Collision Theory

Δ G∘ of the c...

Question

$Δ G^{\circ}$ 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:

- 21.52 kJ

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- 10.76 kJ

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- 43.04 kJ

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43.03 kJ

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Solution

The correct option is C $- 43.04 kJ$
$A g C l (s) + \frac{1}{2} H_{2} (g) \to A g (s) + H^{+} + C l^{-}, Δ G_{1}^{0} = - 21.12 kJ$
$2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} + 2 C l^{-}$
$= 2 (- 21.52) kJ = - 43.04 kJ$
Therefore, the correct answer is (c).

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Similar questions

Δ G^{o}

for the reaction:

A g C l (s) + 1 / 2 H_{2} (g) ⟶ A g (s) + H^{+} + C l^{-}

- 21.52 k J

Δ G^{o}

for the reaction:

2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} + 2 C l^{-}

is:

Δ G^{o}

of the cell reaction

A g C l (s) + 1 / 2 H_{2} (g) \to A g (s) + H^{+} (a q .) + {C l}^{-} (a q)

- 21.52 k J

Calculate the EMF for the cell reaction:

2 A g C l (c) + H_{2} (g) \to A g (s) + 2 H^{+} (a q .) + 2 {C l}^{-} (a q .)

Q. The standard free energy change for the reaction,

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

- 10.26 k c a l m o l^{- 1}

25^{\circ} C

. A cell using the above reaction is operated at

25^{\circ} C

under

P_{H_{2}} = 1 a t m . [H^{+}]

and

[C l^{-}] = 0.1

. Calculate the emf of the cell.

Q. Consider the following cell reaction:

2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} (a q) + 2 C l^{-} (a q); E^{o} = 0.19 V

[C l^{-}] = 10^{- 3} M

and

P_{H_{2}} = 0.01 atm

, if the cell potential is 0.43

V

25^{o} C

the

p H

is:

(Take \frac{2.303 R \times 298}{F} = 0.06)

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?

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ΔG∘ of the cell reaction, AgCl(s)+12H2(g)→Ag(s)+H++Cl−is −21.52KJ.ΔG∘of 2AgCl(s)+H2(g)→2Ag(s)+2H+2Cl− is:

The correct option is C −43.04 kJAgCl(s)+12H2(g)→Ag(s)+H++Cl−, ΔG01=−21.12 kJ 2AgCl(s)+H2(g)→2Ag(s)+2H++2Cl− =2(−21.52) kJ=−43.04 kJ Therefore, the correct answer is (c).

$Δ G^{\circ}$ 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:

The correct option is C $- 43.04 kJ$
$A g C l (s) + \frac{1}{2} H_{2} (g) \to A g (s) + H^{+} + C l^{-}, Δ G_{1}^{0} = - 21.12 kJ$
$2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} + 2 C l^{-}$
$= 2 (- 21.52) kJ = - 43.04 kJ$
Therefore, the correct answer is (c).