Consider the following electrochemical cell at 298 K Ag(.s.)|.AgI(.s.)|.I-(.aq.)|.|.Cl-(.aq.)|.Hg2Cl2|.Hg(.l.)Pt(.s.) [Given EC l- |. H g2 C l2 |. H go=0.26V.EA g+ / A go=0.8V,Ks p(.AgI.)=10- 16 and (2.303 R T/F)=0.06 ] The overall reaction occurring in the above cell is

Question

Consider the following electrochemical cell at 298 K Ag(.s.)|.AgI(.s.)|.I-(.aq.)|.|.Cl-(.aq.)|.Hg2Cl2|.Hg(.l.)Pt(.s.) [Given EC l- |. H g2 C l2 |. H go=0.26V.EA g+ / A go=0.8V,Ks p(.AgI.)=10- 16 and (2.303 R T/F)=0.06 ] The overall reaction occurring in the above cell is (A) (1/2)Hg2Cl2(.s.)+Ag(.s.)+I-(.aq.) arrow Hg(.l.)+Cl-(.aq.)+AgI(.s.) (B) Ag+(.aq.)+I-(.aq.) arrow AgI(.s.) (C) Hg22 +(.aq.)+I2Cl-(.aq.) arrow Hg2Cl2(.s.) (D) Cell reaction is not possible

Tardigrade Admin · Accepted Answer

Anode Ag+I- arrow AgI+e- Cathode Hg2Cl2+2e arrow 2Hg+2Cl- Hence, The overall reaction occurring in the above cell is (1/2)Hg2Cl2(.s.)+Ag(.s.)+I-(.aq.) arrow Hg(.l.)+Cl-(.aq.)+AgI(.s.)

$\frac{1}{2} H g_{2} C l_{2} (s) + A g (s) + I^{-} (a q) \to H g (l) + C l^{-} (a q) + A g I (s)$

$A g^{+} (a q) + I^{-} (a q) \to A g I (s)$

$H g_{2}^{2 +} (a q) + I_{2} C l^{-} (a q) \to H g_{2} C l_{2} (s)$

Cell reaction is not possible

Anode $A g + I^{-} \to A g I + e^{-}$

Cathode $H g_{2} C l_{2} + 2 e \to 2 H g + 2 C l^{-}$

Hence, The overall reaction occurring in the above cell is

$\frac{1}{2} H g_{2} C l_{2} (s) + A g (s) + I^{-} (a q) \to H g (l) + C l^{-} (a q) + A g I (s)$

Q. Consider the following electrochemical cell at 298 K Ag(s)∣AgI(s)∣I−(aq)∣∣Cl−(aq)∣Hg2​Cl2​∣Hg(l)Pt(s) [Given ECl−∣Hg2​Cl2​∣Hgo​=0.26V.EAg+/Ago​=0.8V,Ksp​(AgI)=10−16 and F2.303RT​=0.06 ] The overall reaction occurring in the above cell is

21​Hg2​Cl2​(s)+Ag(s)+I−(aq)→Hg(l)+Cl−(aq)+AgI(s)

Ag+(aq)+I−(aq)→AgI(s)

Hg22+​(aq)+I2​Cl−(aq)→Hg2​Cl2​(s)

Cell reaction is not possible

Anode Ag+I−→AgI+e− Cathode Hg2​Cl2​+2e→2Hg+2Cl− Hence, The overall reaction occurring in the above cell is 21​Hg2​Cl2​(s)+Ag(s)+I−(aq)→Hg(l)+Cl−(aq)+AgI(s)

$\frac{1}{2} H g_{2} C l_{2} (s) + A g (s) + I^{-} (a q) \to H g (l) + C l^{-} (a q) + A g I (s)$

$A g^{+} (a q) + I^{-} (a q) \to A g I (s)$

$H g_{2}^{2 +} (a q) + I_{2} C l^{-} (a q) \to H g_{2} C l_{2} (s)$

Anode $A g + I^{-} \to A g I + e^{-}$

Cathode $H g_{2} C l_{2} + 2 e \to 2 H g + 2 C l^{-}$

Hence, The overall reaction occurring in the above cell is

$\frac{1}{2} H g_{2} C l_{2} (s) + A g (s) + I^{-} (a q) \to H g (l) + C l^{-} (a q) + A g I (s)$