ElectrochemistryHard
Question
Consider the cell: Ag(s), AgCl(s)|KCl (0.1 M)|Hg2Cl2(s), Hg(l). The cell potential
Options
A.increases on increasing concentration of Cl− ions.
B.decreases on decreasing concentration of Cl− ions.
C.is independent of concentration of Cl− ions.
D.is independent of amounts of AgCl and Hg2Cl2.
Solution
Left electrode: Ag(s) + Cl− (aq) → Ag Cl (s) + e− 1 × 2
Right electrode: Hg2Cl2(s) + 2e− → 2Hg(l) + 2 Cl− (aq)
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Net reaction: 2Ag(s) + Hg2Cl2(s) → 2Ag Cl(s) + 2Hg (l)
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