Objectives:
After having completed this unit, students should be able to:
- Define and identify oxidation and reduction – Review from Unit 3
- Identify oxidation-reduction (redox) reactions – Review from Unit 3
- Assign oxidation states to the elements in a compound or ion. – Review from Unit 3
- Identify oxidizing and reducing agents. – Review from Unit 3
- Diagram and describe and explain voltaic (or galvanic) and electrolytic cells: indicate the cathode, anode, salt bridge, direction of flow of electrons, direction of migration of ions and the half-cell reaction involved at each electrode.
- Write voltaic cells using standard line notation.
- Define cell potential and explain how it is measured.
- Define standard reduction potential.
- Explain how standard reduction potentials are assigned in terms of the standard hydrogen electrode.
- Using tabulated standard reduction potential calculate the standard cell potential (standard EMF) of a galvanic cell and predict whether the reaction is spontaneous.
- Given the components of the electrodes and observations on what happens at the electrodes in a voltaic cell, write the balanced oxidation and reduction half reactions, write the balanced overall spontaneous reaction, and calculate the cell voltage
- Using standard reduction potentials predict the strength of various oxidizing and reducing agents.
- Explain the relationship between the maximum cell potential and the free energy difference between cell reactants and products.
- Know and be able to use the equations that relate ΔG°, K and E° for cell reactions.
- Explain the basis for concentration cells.
- Qualitatively predict the effect of concentration and gas pressure on cell potential.
- Use the Nernst equation to calculate the EMF under nonstandard conditions or to calculate a concentration of reactant or product required to give a certain voltage.
- Explain with the aid of the balanced equation the operation of fuel cells and of the lead-acid, alkaline, the nickel-cadmium, nickel-metal hydride, and lithium-ion batteries.
- Distinguish between batteries and fuel cells.
- Explain the electrochemical nature of corrosion and describe some methods of preventing it.
- Explain the difference in product at each electrode for molten salts compared to aqueous solutions of the salt.
- Using standard reduction potentials predict the most likely product at each electrode in the electrolysis of aqueous solutions and write the equation for the reaction.
- Given two of the three following variables: time, current or amount of substances reacting in an electrolytic cell, calculate the third variable. Amount can be indicated by grams, volume, moles, concentration, pH, pOH, molar mass, or oxidation state
- Explain how electrolysis can be used in the application of metal plating.
Reading and Homework Exercises
Table of Contents from: OpenStax Chemistry 2e:
Introduction
17.1 Review of Redox Chemistry
17.2 Galvanic Cells
An electrochemical cell has a solid zinc anode in Zn(NO3)2 and a solid copper cathode in Cu(NO3)2. Answer the following questions about this cell:
Question 1:
Question 2:
Question 3:
A galvanic cell is based on the reaction:
8 H+ + 5 Fe2+ + MnO4– → 5 Fe3+ + Mn2+ + 4 H2O
Answer the following questions:
Question 4:
Question 5:
Question 6:
Question 7:
17.3 Electrode and Cell Potentials
An electrochemical cell has a solid zinc anode in Zn(NO3)2 and a solid copper cathode in Cu(NO3)2. Answer the following question about this cell using data in Table 17.1
Question 8:
A galvanic cell is based on the reaction:
8 H+ + 5 Fe2+ + MnO4– → 5 Fe3+ + Mn2+ + 4 H2O
Answer the following question about this cell using data in Table 17.1
Question 9:
A galvanic cell (spontaneous) is set up with the Pb/Pb2+ and Ag/Ag+ couples. Answer the following questions (use data in Table 17.1)
Question 10:
Question 11:
Question 12:
Question 13:
Answer the following 3 questions for the following redox reaction:
2 Au3+ + 3 Ni(OH)2 + 6 OH– → 2 Au + 3 NiO2 + 6 H2O
Question 14:
Question 15:
Question 16:
Use a table of standard reduction potentials to answer the following two questions:
Question 17:
Question 18:
17.4 Potential, Free Energy, and Equilibrium
A galvanic cell is based on the reaction:
8 H+ + 5 Fe2+ + MnO4– → 5 Fe3+ + Mn2+ + 4 H2O
Answer the following question:
Question 19:
Answer the following question for the following redox reaction:
2 Au3+ + 3 Ni(OH)2 + 6 OH– → 2 Au + 3 NiO2 + 6 H2O
Question 20:
Answer the following 2 questions for the following redox reaction:
3 Cu2+ + 2 NO + 4 H2O → 3 Cu + 8 H+ + 2 NO3–
Question 21:
Question 22:
Calculate the Ecell in volts of a Zn-Ag+ cell under the following nonstandard conditions as listed in the problem below::
Zn(s) + 2Ag+ (aq) —-> Zn2+ (aq) + 2Ag(s)
Question 23:
For the same cell, answer the following question:
Question 24:
17.5 Batteries and Fuel Cells
Question 25:
Question 26:
Question 27:
Question 28:
17.6 Corrosion
Question 29:
Question 30:
17.7 Electrolysis
Question 31:
Question 32:
Question 33:
Question 34:
Question 35:
Question 36:
Question 37:
Question 38:
Question 39:
Question 40:
Question 41: