Solved: Use the following half-reactions to write three

Chapter 22, Problem 37P

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Use the following half-reactions to write three spontaneous reactions and calculate \(E_{\text {cell }}^{\circ}\) for each reaction:

(1) \(2 \mathrm{HClO}(a q)+2 \mathrm{H}^{+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

\(E^{\circ}=1.63 \mathrm{~V}\)

(2) \(\mathrm{Pt}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pt}(s) \quad E^{\circ}=1.20 \mathrm{~V}\)

(3) \(\mathrm{PbSO}_{4}(s)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pb}(s)+\mathrm{SO}_{4}{ }^{2-}(a q) \quad E^{\circ}=-0.31 \mathrm{~V}\)

Equation Transcription:

Text Transcription:

E_cel^circ    

2HClO(aq)+2H^+(aq)+2e^- longrightarrow Cl_2 (g)+2H_2 O(l)  

E^circ =1.63 V  

Pt^2+(aq)+2e^- longrightarrowPt(s) E=1.20 V  

PbSO_4(s)+2e^- longrightarrow Pb(s)+SO_4^ 2-(aq) E^circ=-0.31 V