Chapter 13, Problem 13.11PAE

The following oxidation−reduction reactions are used in electrochemical cells. Write them using cell notation.

(a) $2{\text{Ag}}^{+}\left(\text{aq}\right)\left(0.50\text{M}\right)+\text{Ni}\left(\text{s}\right)\to 2\text{Ag}\left(\text{s}\right)+{\text{Ni}}^{2+}\left(\text{aq}\right)\left(0.20\text{M}\right)$

(b) $\text{Cu}\left(\text{s}\right)+{\text{PtCl}}_{\text{6}}{}^{\text{2-}}\left(\text{aq}\right)\left(\text{0}\text{.10}\text{M}\right)\to {\text{Cu}}^{2+}\left(\text{aq}\right)\left(\text{0}\text{.20}\text{M}\right)+{\text{PtCl}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right)\left(\text{0}\text{.10}\text{M}\right)+2{\text{Cl}}^{-}\left(\text{aq}\right)\left(0.40\text{M}\right)$

(c) $\text{Pb}\left(\text{s}\right)+{\text{SO}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right)\left(\text{0}\text{.30}\text{M}\right)+2\text{AgCl}\left(\text{s}\right)\to {\text{PbSO}}_{\text{4}}\left(\text{s}\right)+2\text{Ag}\left(\text{s}\right)+2{\text{Cl}}^{-}\left(\text{aq}\right)\left(0.20\text{M}\right)$

(d) In a galvanic cell, one half-cell contains 0.010 M HCI and a platinum electrode, over which H₂ is bubbled at a pressure of 1.0 atm. The other half-cell is composed of a zinc electrode in a 0.125 M solution of Zn(NO₃)₂.