Ag -AgCl-Cl-C2-Cl-C1-AgCl-Ag for this cell - G is negative if-

Given cell is electrolyte concentration cell E_cell = RT/F nbsp;ln [Ag^+]_cathode/[Ag^+]_anode Where [Ag^+] = K_sp/[Cl^ ] For spontaneous chemical change con ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard X

Chemistry

Application of Electrolysis

Ag |AgCl|Cl-C...

Question

$A g | A g C l | C l^{-} (C_{2}) | | C l^{-} (C_{1}) | A g C l | A g for this cell Δ G$ is negative if:

$C_{1} = C_{2}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$C_{1} > C_{2}$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

$C_{2} > C_{1}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Both (a) and (c)

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B
$C_{1} > C_{2}$

Given cell is electrolyte concentration cell
$E_{c e l l} = \frac{R T}{F} l n \frac{[A g^{+}]_{c a t h o d e}}{[A g^{+}]_{a n o d e}}$

Where $[A g^{+}] = \frac{K_{s p}}{[C l^{-}]}$
For spontaneous chemical change conc. of $A g^{+}$ of cathodic compartment must be greater than anodic compartment.

Suggest Corrections

Similar questions

A g | A g C l | C l^{-} (C_{2}) ∥ C l^{-} (C_{1}) | A g C l | A g

for this cell

Δ G

is negative if:

$A g | A g C l | C l^{-} (C_{2}) | | C l^{-} (C_{1}) | A g C l | A g for this cell Δ G$ is negative if:

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. If

A g^{+} + 2 N H_{3} ⇌ A g (N H_{3})_{2}^{+}; K_{1} = 1.7 \times 10^{7}

A g^{+} + C l^{-} ⇌ A g C l; K_{2} = 5.4 \times 10^{9}

For

A g C l + 2 N H_{3} ⇌ [A g (N H_{3})_{2}]^{+} + C l^{-}

, the equilibrium constant is :

Q. If

A g^{+} + 2 N H_{3} ⇌ {[A g (N H_{3})_{2}]}_{3}^{+}

;

K_{1} = 1.7 \times 10^{7}

;

A g^{+} + C l^{-} ⇌ A g C l

;

K_{2} = 5.4 \times 10^{9}

Then for

A g C l + 2 N H_{3} ⇌ [A g (N H_{3})_{2}]^{+} C l^{-}

; equilibrium constant will be?

Join BYJU'S Learning Program

Ag|AgCl|Cl−(C2)||Cl−(C1)|AgCl|Ag for this cell ΔG is negative if:

The correct option is B C1>C2 Given cell is electrolyte concentration cell Ecell=RTFln[Ag+]cathode[Ag+]anode Where [Ag+]=Ksp[Cl−] For spontaneous chemical change conc. of Ag+ of cathodic compartment must be greater than anodic compartment.

$A g | A g C l | C l^{-} (C_{2}) | | C l^{-} (C_{1}) | A g C l | A g for this cell Δ G$ is negative if: