Calculate the useful work done during the reaction in kJ - mol- Ag S -1-2 Cl 2 g - AgCl s Given that E Cl 2 - Cl -0-1-36 Vand E Ag - AgCl - Cl -0-0-220 VP Cl 2-1 atm and T -298 K

For the cell reaction: Ag(s) + 1/2 Cl_2(g) → AgCl(s) E^0 = 1.36 0.22= nbsp;1.14 V or, E = E^0 0.0591log 1[Cl_2]^1/2 In standard conditions, P_Cl_2 = 1 atm ...

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Standard XII

Chemistry

Gibb's Energy and Nernst Equation

Calculate the...

Question

Calculate the useful work done during the reaction in kJ/mol.
$A g (S) + \frac{1}{2} C l_{2} (g) \to A g C l (s)$
Given that $E_{C l_{2} / {C l}^{-}}^{0} = + 1.36 V$
and $E_{A g^{+} | A g C l | C l^{-}}^{0} = + 0.220 V$
$P_{C l_{2}} = 1 atm$ and T = 298 K

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Solution

For the cell reaction:
$A g (s) + \frac{1}{2} C l_{2} (g) \to A g C l (s) E^{0} = 1.36 - 0.22 = 1.14 V$
or, $E = E^{0} - \frac{0.059}{1} log \frac{1}{[C l_{2}]^{\frac{1}{2}}}$
In standard conditions, $P_{C l_{2}} = 1 atm$
$∴$ log $[C l_{2}]^{\frac{1}{2}} = 0$
Useful work $= - W_{m a x} = △ G = - n E F = (1) \times (1.14) \times 96500 \times 10^{- 3} = 110 kJ/mol$

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Similar questions

Q. Calculate the useful work of the reaction

A g (s) + 1 / 2 C l_{2} (g) \to A g C l (s)

.
Given

E_{c l_{2} / C l^{-}}^{0} = + 1.36 V,

E_{A g | A g C l | C l^{-}}^{0} = 0.22 V

P_{C l_{2}} = 1 a t m

and

T = 298 K

Q. calculate

Δ G_{f}^{⊖}

of the reaction :

A g^{\oplus} (a q) + C l^{⊖} (a q) \to A g C l (s)

Given :

Δ G^{⊖_{A g C l}} = - 109 k J m o l^{- 1}

Δ G_{(C l^{⊖})}^{⊖} = - 129 k J m o l^{- 1}

Δ G_{(A g^{\oplus)}}^{⊖} = - 77 k J m o l^{- 1}

Q. For the reaction

A g^{+} (a q) + C l^{-} (a q) ⇌ A g C l (s)

; the

Δ G^{o}

values for

A g^{+} (a q), C l^{-} (a q)

and

A g C l (s)

are + 77, -129 and -109 kJ mol

^{- 1}

. Write the cell representation of above reaction and calculate

K_{s p}

of AgCl at 298 K.
(Multiply the ans by

10^{10}

)

Q. Calculate the cell EMF in mV for :

P t | H_{2} (1 a t m) | H C l (0.01 M) | A g C l (s) | A g (s) a t 298 K

Δ G_{t}^{o}

values are at 25

^{o}

- 109.56 \frac{k J}{m o l}

for AgCl(s) and

- 130.79 \frac{k J}{m o l}

for (H

^{+}

+ Cl

^{-}

) (aq)

Q. The standard free energy of formation for

A g C l

298 K

- 109.7 k J

{m o l}^{- 1}

Δ G^{o} ({A g}^{+}) = 77.2 k J / m o l

;

Δ G^{o} ({C l}^{-}) = - 131.2 k J / m o l

. Find the solubility of

A g C l

0.05 M

K C l

. Neglect any complication due to complexation.

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Calculate the useful work done during the reaction in kJ/mol. Ag(S)+12 Cl2(g)→AgCl(s) Given that E0Cl2/Cl−=+1.36V and E0Ag+|AgCl|Cl−=+0.220V PCl2=1 atm and T = 298 K

For the cell reaction: Ag(s)+12 Cl2(g)→AgCl(s)E0=1.36−0.22=1.14 V or, E=E0−0.0591log 1[Cl2]12 In standard conditions, PCl2=1 atm ∴ log [Cl2]12=0 Useful work=−Wmax=△G=−nEF=(1)×(1.14)×96500×10−3=110 kJ/mol

Calculate the useful work done during the reaction in kJ/mol.
$A g (S) + \frac{1}{2} C l_{2} (g) \to A g C l (s)$
Given that $E_{C l_{2} / {C l}^{-}}^{0} = + 1.36 V$
and $E_{A g^{+} | A g C l | C l^{-}}^{0} = + 0.220 V$
$P_{C l_{2}} = 1 atm$ and T = 298 K