Consider the voltaic cell
Write the half-cell reactions and the overall cell reaction. Make a sketch of this cell and label it. Include labels showing the anode, cathode, and direction of electron flow.
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A voltaic cell that uses the reaction
PdCl42- (aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq), 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° red for the reaction involving Pd. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.
Voltaic cell that uses the reaction
T13+(aq) + 2Cr2+(aq)→T1+(aq) + 2Cr3+(aq), has a measured standard cell potential of +1.19 V.
(a) Write the two half-cell reactions. (b) By using data from Appendix E, determine E°red for the reduction of T13+(aq) to T1+(aq).
(c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.
Sketch a voltaic cell for this redox reaction: Ni2+(aq) + Mg (s) ----> Ni (s) + Mg2+(aq)
a.Label the anode and cathode.
b.Write the half reactions.
c.Indicate the direction of electron flow.
d.Calculate Eocell.
e.Write the line notation for the cell.