Solve this-The standard emf of the following cell-Cd-s-CdCl2-aq- -0-10 M-Cl- AgCl-s-Ag-s-In which the cell reaction is 2AgCl-s- - Cd-s- -8594-2Ag-s- -Cd2- - 2Cl-aq- is 0-6915 V at 100 C and 0-6753 V at 250C- The -8710-H of reaction at 250C is-A- -192-5 kJ nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- -B- -234-7 kJ-C- 123-5 kJ nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- -D- -167-26 kJ

Dear Student, 1. The formula used is Gibbs nbsp;Helmoltz nbsp;equation : nbsp; nbsp; nbsp; nbsp; #8710;G= #8710;H T #8710;S2. #160;F ...

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Byju's Answer

Standard XII

Chemistry

Factors Affecting Rate of Reaction

Solve this: ...

Question

Solve this:
The standard emf of the following cell:
Cd(s)|CdCl₂(aq) (0.10 M)||Cl^-| AgCl(s)|Ag(s)
In which the cell reaction is 2AgCl(s) + Cd(s) $\to$ 2Ag(s) +Cd²⁺ + 2Cl^-(aq) is 0.6915 V at 10⁰ C and 0.6753 V at 25⁰C. The $∆$ H of reaction at 25⁰C is
(A) -192.5 kJ (B) -234.7 kJ
(C) 123.5 kJ (D) -167.26 kJ

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Solution

Dear Student,

1. The formula used is Gibbs Helmoltz equation :

$∆ G = ∆ H - T ∆ S 2 . F r o m t h e d a t a i n q u e s t i o n : ∆ G_{1} (283 K) = - n F E^{\circ} = - 2 \times 96500 \times 0.6195 = 11.96 k J ∆ G_{2} (298 K) = - n F E^{\circ} = - 2 \times 96500 \times 0.6753 = 13.03 k J 3 . U \sin g e q u a t i o n 1 : 11.96 k J = ∆ H - 283 ∆ S . . . (1) - 13.03 k J = - ∆ H + 298 ∆ S . . . (2) w e g e t, ∆ S = - 572 J K^{- 1} ∆ H = 123.5 k J$
Regards,

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Similar questions

Q. The 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 0°C and

0.6753 V

at 25°C. The

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and

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Take,

F = 96485 C m o l^{- 1}

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

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0.6573

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Q. The standard emf of the cell,

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

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C d_{(s)} + 2 A g C l_{(s)} \Rightarrow 2 A g_{(s)} + C d_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}

0.6915 V

0^{o} C

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0.6573

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The enthalpy change of the reaction at

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The EMF of the above cell is 0.6315 V at

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Q. For the reaction:

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25^{\circ} C

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