?A voltaic cell that uses the reaction \(\mathrm{PdCl}_{4}{ }^{2-}(a q)+\mathrm{Cd}(s) \longrightarrow \mathrm{Pd}(s)+4 \mathrm{Cl}^{-}(a q)+\

Chapter 20, Problem 20.36

(choose chapter or problem)

A voltaic cell that uses the reaction

\(\mathrm{PdCl}_{4}{ }^{2-}(a q)+\mathrm{Cd}(s) \longrightarrow \mathrm{Pd}(s)+4 \mathrm{Cl}^{-}(a q)+\mathrm{Cd}^{2+}(a q)\)

has a measured standard cell potential of +1.03 V.

(a) Write the two half-cell reactions.

(b) By using data from Appendix E, determine \(E_{\text {red }}^{\circ}\) for the reaction involving Pd.

(c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.

Text Transcription:

PdCl4 2-(aq) + Cd(s) \longrightarrow Pd(s) + 4 Cl -(aq) + Cd2+(aq)

E_red ^{\circ}