Math  /  Algebra

Question6 N .12 (a) The standard potential of the reduction of Ag2CrO4\mathrm{Ag}_{2} \mathrm{CrO}_{4} to Ag(s)\mathrm{Ag}(\mathrm{s}) and chromate ions is +0.446 V . Write the balanced half-reaction for the reduction of silver chromate. (b) Using the data from part (a) and Appendi 2B\underline{2 B}, calculate the solubility product of Ag2CrO4( s)\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{~s}).
6N. 13 Calculate the reaction quotient, QQ, for the following cell reactions, given the measured values of the cell potential. Balance the chemical equations by using the smallest whole-number coefficients. (a) Pt(s)Sn4+(aq),Sn2+(aq)Pb4+(aq),Pb2+(aq)C(gr),Ecell =+1.33 V\mathrm{Pt}(\mathrm{s})\left|\mathrm{Sn}^{4+}(\mathrm{aq}), \mathrm{Sn}^{2+}(\mathrm{aq})\right|\left|\mathrm{Pb}^{4+}(\mathrm{aq}), \mathrm{Pb}^{2+}(\mathrm{aq})\right| \mathrm{C}(\mathrm{gr}), E_{\text {cell }}=+1.33 \mathrm{~V}.

Studdy Solution
The balanced half-reaction is Ag2CrO4(s)+2e2Ag(s)+CrO42(aq)\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s}) + 2e^{-} \longrightarrow 2\mathrm{Ag}(\mathrm{s}) + \mathrm{CrO}_{4}^{2-}(\mathrm{aq}).
The solubility product of Ag2CrO4\mathrm{Ag}_{2} \mathrm{CrO}_{4} is approximately 1.110151.1 \cdot 10^{-15}.
The balanced chemical equation for the second reaction is Sn4+(aq)+Pb2+(aq)Sn2+(aq)+Pb4+(aq)\mathrm{Sn}^{4+}(\mathrm{aq}) + \mathrm{Pb}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Sn}^{2+}(\mathrm{aq}) + \mathrm{Pb}^{4+}(\mathrm{aq}), and the reaction quotient is approximately 1.11071.1 \cdot 10^{7}.

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