Electrochemistry Homework Problem Set
This problem set was developed by S.E. Van Bramer for Chemistry 146 at Widener University.
- Balance the following chemical equations. Assume the reactions occur in acidic solutions (add H1+ and/or H2O as necessary). For each reaction identify the oxidizing and reducing agent. Identify which reactant is oxidized and which is reduced. Write the appropriate half reactions. Determine [delta]G for the reaction and Eo for the reaction (If you can find the necessary thermodynamic data).
- Sn2+(aq) + Hg2+ (aq) + Cl1- (aq) --> Sn4+(aq) + Hg2Cl2 (s)
- Fe2+ (aq) + Cr2O72- (aq) --> Fe3+ (aq) + Cr3+ (aq)
- Hg2+ (aq) + Cu (s) --> Cu2+ (aq) + Hg (l)
- Zn(s) + HCl(aq) --> Zn2+(aq) + H2(g)
- CH4 + O2 --> CO2 + H2O
- V2O3(s) + H2(g) --> VO(s) + H2O(l)
- N2O4(g) + Br-(aq) --> NO21-(aq) + BrO31-(aq)
- V(s) --> HV10O285-(aq) + H2(g)
- Br2(aq) + Sn2+ (aq) --> Br1- (aq) + Sn4+(aq)
- Cu (s) + HNO3 (aq) --> Cu2+ + NO2 (g)
- Write a figure showing an electrochemical cell that will generate electricity based upon the oxidation of iron to iron (II), and the reduction of silver (I) to silver metal.
- Write a balanced chemical equation
- Write the cell notation for this system
- Write the half reactions for each cell
- Label the anode and the cathode
- Show the direction of electron motion through the external circuit
- Show the motion of ions in the solution
- Show the transfer of ions at the electrode surface
- Calculate the standard cell potential
- Is this cell spontaneous?
- Calculate the standard cell potential for the reverse reaction.
- Identify the anode, the cathode, the reduced species and the oxidized species for the following electrochemical cells. Write the half reactions for the anode and cathode, the overall reaction. Calculate the standard cell potential and the cell potential.
- Fe (s) | Fe2+ (aq) (0.2 M) || Ni2+ (aq) (0.1 M)
- Pt (s) | O2 (g)(0.2 atm) | H2O2 (aq) (0.01 M pH=4) || Cu2+ (aq) (1.0 x 10-4 M) | Cu (s)
- Zn (s) | Zn2+ (aq) (1.0 x 10-3 M)|| Cl1- (aq)(0.3 M) | Cl2 (g) (100 torr) | Pt (s)
- Pt (s) | Fe2+ (aq) (0.02 M), Fe3+ (aq) (2.3 x 10-3M) || H1+
(aq) (pH = 3), Cr2O72- (aq)(0.03 M), Cr3+ (aq, 0.003 M) | Pt (s)
- Pb (s) | Pb2+ (aq) (1.0 M) || Cu2+ (aq) (1.0 M) | Cu (s)
- Pb (s) | Pb2+ (aq) (0.210 M) || Cu2+ (aq) (0.0145 M) | Cu (s)
- Pb (s) | Pb2+ (aq) (1.0 x 10-5 M) || Cu2+ (aq) (1.0 x 10-2 M) | Cu (s)
- The following cell has a potential of 0.100 V. Calculate the pH at the anode:
Pt (s) | H2 (g, 1 atm) | H1+ (aq, ? M)) || H1+ (0.10 M) | H2 (g 1 atm) | Pt (s)
- On space craft, a H2/O2 fuel cell is used to produce electricity.
- The reactions
- What is the reaction at the anode?
- What is the reaction at the cathode?
- What is the balanced redox reaction?
- What is Ecell assuming Po2 = 2*atm, and PH2 = 2*atm.
- If two cylinders of H2 and 1 cylinder of O2 (cylinder: volume=200 liter, pressure = 3000 psi) are used.
- How many moles of electrons can be produced?
- How much energy (joules) is this?
- If this energy has to last for 1 week, what is the average power (watts) available?
- Compare the amount of energy produced by this fuel cell to the energy produced by the combustion of the same amount of H2 and O2 using [delta] Grxn.
- The following relationships may be useful:
- V = kg m2 s-3 A
- A = C s-1
- J = kg m2 s-2
- W = J s-1
- Electrochemical Analysis techniques are capable of detecting very small amounts of certain metals. In one type of analysis Cd2+ undergoes electrolysis. In this experiment it is possible to detect a signal from 1 pA of current, lasting only 1 ms.
- How many moles of Cd2+ does this correspond to?
- How many atoms is this?
Please send comments or suggestions to email@example.com
Scott Van Bramer
Department of Chemistry
Chester, PA 19013
© copyright 1996, S.E. Van Bramer
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Last Updated: Saturday, May 18, 1996