Electrochemical Cells
- Page ID
- 283128
1.) Consider this overall redox process: Cu2+(aq)+Ba(s)→Cu(s)+Ba2+(aq)
a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.
b.) Construct a cell diagram.
c.) Give the line notation for this cell.
d.) Calculate E°cell, the standard cell potential, which is given by E°red - E°ox.
2.) Consider this overall redox process: Al(s)+Sn2+(aq)→Al3+(aq)+Sn(s)
a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.
b.) Construct a cell diagram.
c.) Give the line notation for this cell.
d.) Calculate E°cell.
3.) Consider a galvanic cell with Zn(s) and 0.25 M Zn(NO3)2(aq) in one compartment and Cu(s) and 0.25 M Cu(NO3)2(aq) in the other compartment.
a.) Give the half-reactions and their standard reduction potentials.
b.) Give the net, overall cell reaction and the standard cell potential:
c.) Now calculate the overall cell potential at the specific concentrations given. You’ll need to use the Nernst equation: Ecell = Eocell – (0.0592/n)log Q
d.) What would be the cell potential if the concentration of Zn(NO3)2 was increased to 2.5 M?
4.) Consider a voltaic cell with Cr(s) and Cr3+(aq) in one compartment and Zn(s) and Zn2+(aq) in the other compartment.
a.) Draw and label a diagram of this cell.
b.) Calculate the standard cell potential for the overall reaction.
c.) If zinc is the anode and [Cr3+] = 0.010 M, what must the [Zn2+] be in order to achieve 0.050V?
5.) A Zn/Zn2+ half-cell was coupled to a hydrogen electrode in which PH2 = 1 bar. The [Zn2+] in the anode compartment was 0.10 M and the cell potential was 0.542 V. Calculate the pH in the cathode compartment.
Contributors and Attributions
- Molly McGuire, Bucknell University (mmcguire@bucknell.edu)
- Sourced from the Analytical Sciences Digital Library