Physical Chemistry III (Chemical Thermodynamics)

GENERAL OBJECTIVES:

1. Understand the basic concepts of thermodynamics

2. Understand the heat changes in reactions

3. Understand the concepts and applications of the second law of thermodynamics

1.1 Explain the scope of thermodynamics.

1.2 Define universe, system and surroundings.

1.3 Classify thermodynamic systems as open, closed and isolated.

1.4 Define internal energy, heat and work.

1.5 State the first law of thermodynamics.

1.6 Calculate the work done when gas expands against an external pressure.

1.7 Explain thermodynamic reversibility.

1.8 Define isothermal process and adiabatic process.

1.9 Calculate the work done during the isothermal expansion of an ideal gas.

1.10 Calculate the change in internal energy during the isothermal reversible expansion of an ideal gas

1.11 Define heat capacity.

1.12 Define enthalpy.

1.13 Relate changes of enthalpy in a system to the heat transferred at constant pressure.

1.14 Define extensive and intensive properties.

1.15 Define state function and path dependent function.

1.16 Explain the terms: exact differentials and in-exact differentials.

1.17 Relate changes of internal energy to changes in volume and temperature.

1.18 Deduce expressions for the dependence of the internal energy on the temperature at constant pressure using the properties of partial derivatives.

1.19 Deduce expressions for he dependence of the enthalpy on the temperature at constant volume using the properties of partial derivatives.

1.20 Define isobaric expansivity and isothermal compressibility.

1.21 Derive the relation between heat capacities at constant volume and constant pressure.

1.22 Calculate the work one by an ideal gas during adiabatic change.

1.23 Calculate the final volume, pressure and temperature of an ideal gas after a reversible, adiabatic change of volume.

2.1 Define the terms endothermic reaction, exothermic reaction and reaction enthalpy.

2.2 Define standard state.

2.3 State Hess’s law of constant heat summation.

2.4 Use Hess’s law to calculate the various heats of reaction.

2.5 Relate reaction enthalpy to change in internal energy.

2.6 Define enthalpy of sublimation, enthalpy of combustion, enthalpy of solution and enthalpy of neutralization.

2.7 Calculate the various enthalpies in 2. 6 above.

2.8 Define enthalpy of hydrogenation, bond enthalpy, enthalpy of atomization and enthalpy of phase transition.

2.9 Construct the Born-Haber cycle and use it to determine enthalpies from other data.

3.1 State the criteria for the direction of spontaneous change.

3.2 Define thermodynamic entropy.

3.3 Derive the expression  for the change of the entropy on isothermal expansion of an ideal gas.

3.4 State the second law of thermodynamics.

3.5 Calculate the change of entropy when a system is heated.

3.6 Calculate the entropy change during a phase transition.

3.7 Calculate the entropy change during irreversible processes.


3.8 Calculate the changes of entropy in the surroundings of a system.

3.9 Define the Helmholtz function.

3.10 Define the Gibb’s function.

3.11 Relate the Helmhotz function to the maximum amount of work available from a changing system.

3.12 Relate the Gibb’s function to the maximum amount of non-pV work available from a changing system

3.13 Evaluate the entropy of a system from thermo chemical data.

3.14 State the third law of thermodynamics.

3.15 State how the internal energy changes when the entropy changes.

3.16 State how the internal energy changes when the volume changes.

3.17 Indicate mathematically how the Gibb’s function depends on the pressure and temperature.

3.18 Derive the Gibb’s - Helmholtz equation.

3.19 Use 3.18 above in calculations.

3.20 State how the Gibb’s function of solids and liquids varies with pressure.

3.21 Derive an expression for the pressure dependence of the Gibb’s function and the chemical potential of an ideal gas.

3.22 Define the fugacity of a gas.

3.23 Relate the fugacity of a gas to the pressure of the gas.

3.24 Define the standard state of a real gas.

3.25 State how the Gibb’s function changes when the composition of a system changes.