Lectures:
1. The subject introduction. Chemical thermodynamics – the First Law. Heat capacity and its temperature dependence. The conservation of energy. Internal energy and enthalpy. The standard enthalpy. Temperature dependence of enthalpy.
2. Chemical thermodynamics – application of the First Law. Chemical change: reaction enthalpies, enthalpies of combustion, standard enthalpies of formation, the variation od reaction enthalpy with temperature. Physical change: the enthalpy of phase transition.
3. Chemical thermodynamics – the Second Law: Entropy. Entropy and the Second Law. The direction of spontaneous change. The entropy accompanying heating, cooling and a phase transformation. The standard reaction entropy and the spontaneity of chemical reactions.
4. Chemical thermodynamics – the Second Law: the Gibbs energy. Properties of the Gibbs energy. Combination of the First and the Second Law. The variation of the Gibbs energy with pressure and temperature.
5. Chemical thermodynamics – application of the Second Law: the properties of mixture. Partial molar properties. Chemical potential and the equilibrium in heterogeneous systems.
6. Chemical thermodynamics – application of the Second Law: chemical equilibrium. The reaction Gibbs energy. Reactions in equilibrium – the equation of reaction isotherm. Equilibrium constants, expression for homogeneous and heterogeneous chemical reactions. The effect of temperature on chemical equilibrium.
7. Chemical thermodynamics – application of the Second Law: physical equilibria. The phase rule and its application for a one-component system. Phase diagram of pure substance, the triple point. Clapeyron and Clausius Clapeyron equation.
8. Chemical kinetics – reaction rates. The definition of rate, rate laws and constants. Reaction order. The determination of the rate law. First-order integrated rate laws, half-life.
9. Chemical kinetics – reaction mechanisms and the temperature dependence of reaction rates. Elementary reactions. Consecutive reactions. The formulation of rate laws. The rate-determining step. The Arrhenius equation, the Arrhenius parameters. The effect of catalyst.
10. Chemical kinetics – heterogeneous kinetics: diffusion. Physical and chemical steps of heterogeneous process. Diffusion, the Fick’s Laws. Diffusion coefficient, effect of temperature, effect of viscosity in fluids. The rate determining step – reaction control, diffusion control.
11. Chemical kinetics – heterogeneous kinetics: adsorption. Physisorption and chemisorption. Adsorption isotherms, the Freundlich and Langmuir isotherm.
Laboratory:
Laboratory 1: Determination of partial molar quantities.
Laboratory 2: Determination of calorimeter heat capacity.
Laboratory 3: Determination of temperature dependence of pressure of saturated vapours of the liquid and of its molar enthalpy of vaporization.
Laboratory 4: Thermal dissociation.
1. The subject introduction. Chemical thermodynamics – the First Law. Heat capacity and its temperature dependence. The conservation of energy. Internal energy and enthalpy. The standard enthalpy. Temperature dependence of enthalpy.
2. Chemical thermodynamics – application of the First Law. Chemical change: reaction enthalpies, enthalpies of combustion, standard enthalpies of formation, the variation od reaction enthalpy with temperature. Physical change: the enthalpy of phase transition.
3. Chemical thermodynamics – the Second Law: Entropy. Entropy and the Second Law. The direction of spontaneous change. The entropy accompanying heating, cooling and a phase transformation. The standard reaction entropy and the spontaneity of chemical reactions.
4. Chemical thermodynamics – the Second Law: the Gibbs energy. Properties of the Gibbs energy. Combination of the First and the Second Law. The variation of the Gibbs energy with pressure and temperature.
5. Chemical thermodynamics – application of the Second Law: the properties of mixture. Partial molar properties. Chemical potential and the equilibrium in heterogeneous systems.
6. Chemical thermodynamics – application of the Second Law: chemical equilibrium. The reaction Gibbs energy. Reactions in equilibrium – the equation of reaction isotherm. Equilibrium constants, expression for homogeneous and heterogeneous chemical reactions. The effect of temperature on chemical equilibrium.
7. Chemical thermodynamics – application of the Second Law: physical equilibria. The phase rule and its application for a one-component system. Phase diagram of pure substance, the triple point. Clapeyron and Clausius Clapeyron equation.
8. Chemical kinetics – reaction rates. The definition of rate, rate laws and constants. Reaction order. The determination of the rate law. First-order integrated rate laws, half-life.
9. Chemical kinetics – reaction mechanisms and the temperature dependence of reaction rates. Elementary reactions. Consecutive reactions. The formulation of rate laws. The rate-determining step. The Arrhenius equation, the Arrhenius parameters. The effect of catalyst.
10. Chemical kinetics – heterogeneous kinetics: diffusion. Physical and chemical steps of heterogeneous process. Diffusion, the Fick’s Laws. Diffusion coefficient, effect of temperature, effect of viscosity in fluids. The rate determining step – reaction control, diffusion control.
11. Chemical kinetics – heterogeneous kinetics: adsorption. Physisorption and chemisorption. Adsorption isotherms, the Freundlich and Langmuir isotherm.
Laboratory:
Laboratory 1: Determination of partial molar quantities.
Laboratory 2: Determination of calorimeter heat capacity.
Laboratory 3: Determination of temperature dependence of pressure of saturated vapours of the liquid and of its molar enthalpy of vaporization.
Laboratory 4: Thermal dissociation.