Chemical Energetics and Dynamics

1. Define or explain any of the chemical terms used in the course (i.e. anode, state function).
2. Solve problems of the following types, given a list of selected equations:
   • Determination of the amount of material produced in an electrolytic cell
   • Calculation of the e.m.f of a galvanic cell
   • Calculation of delta G from electrochemical data
   • Calculations involving use of the First Law of Thermodynamics
   • Enthalpy changes in a chemical or physical process
   • Hess’s Law
   • Calculation of delta S from absolute entropies
   • Calculation of delta G for a chemical reaction
   • Calculation of K from delta G°
   • Equilibria in gaseous systems
   • Equilibria in aqueous acid-base systems (pH, weak acids, hydrolysis, buffers)
   • Amounts of material involved in redox reactions
3. Determine the mass of a substance involved in a redox reaction.
4. State Faraday’s Law of Electrolysis.
5. Determine whether chemical reactions will occur spontaneously under standard conditions, given a table of standard electrode potentials.
6. Using a table of standard electrode potentials, compare the relative strengths of oxidizing agents or reducing agents.
7. Distinguish between various types of heats of reaction and write the corresponding chemical equation.
8. Interpret the signs of enthalpy changes.
9. Describe both qualitatively and quantitatively the contributions of delta H and delta S to reaction spontaneity.
10. Predict the sign of delta S for various chemical and physical processes.
11. Interpret equilibrium in terms of the thermodynamic driving forces.
12. Write the chemical equation for the equilibrium involving weak acids and bases in aqueous solution.
13. Classify various aqueous salt solutions as acidic, basic or neutral and write the corresponding equation.
14. Explain how an acid-base indicator works and choose suitable indicators for various acid-base reactions.

Laboratory Objectives

The student will be able to:

1. Give the name and describe the use of some of the more common laboratory equipment.
2. Accurately perform standard laboratory techniques using the accepted methods, such as titration, weighing, pipetting.
3. Give the random and systematic errors inherent in each of the common quantitative techniques which are used in the laboratory.
4. Given an experimental problem, state the series of steps and the accepted techniques required to solve that problem in the laboratory.
5. Write a report based on observations and data obtained in the laboratory using a standard report format.
6. Given a set of experimental data or using data obtained in the laboratory, apply the appropriate mathematical techniques (e.g. graphical analysis, solution of equations, etc.) necessary to obtain a numerical result.
7. Using the data, observations or results of an experiment, determine the relationship between experimental variables.
8. Analyze the overall laboratory experiment with respect to errors inherent in the method or techniques.
9. State the theory upon which the experiment is based.