Physical chemistry, signification, classification.
Chemical thermodynamics. Heat capacities, heating and cooling of substances. The first law of thermodynamics. Enthalpy, variation of the reaction enthalpy with temperature.
The second law of thermodynamics. Entropy and its interpretation. Helmholtz and Gibbs free energy. Chemical potential, activity.
Chemical equilibriums, equilibrium constant for homogeneous nad heterogeneous chemical reactions, Van´t Hoff reaction isotherm and isobare. The Le Chatelier’s principle.
Phase equilibrium - conditions of phase equilibrium. Gibbs phase rule, one-component system (Clapeyron and Clausius-Clapeyron equation), two-component (binary) system (ideal and real solutions, Raoult’s law and Henry’s law). Colligative properties of nonelectrolyte solutions - solutions with non-volatile solute. Phase diagram for two-component liquid mixtures (miscible liquids, partially miscible liquids, totally immiscible liquids). Distribution equilibrium.
The chemical kinetics - rate of chemical reaction, order of reaction, molecularity, rate constant, reaction mechanism. Integrated forms of the kinetic equation. The temperature dependence of the rate constant, Arrhenius equation. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions.
Electrochemistry – electrolytes and theory of electrolytic dissociation. Strong electrolytes - activity and activitiy coefficient, Debye-Hückel limiting law. Solubility product. Equilibrium and dissociation in solutions of weak electrolytes - dissociation of week monobasic acids and bases, hydrolysis of salt, buffer solutions. Electrolysis, transport number, electric conductivity of electrolytes. Electrochemistry potentials, electrodes, galvanic cells.
Colloid chemistry - classification of dispersion systems, degree of dispersion. Selected kinetic, electrical and optical properties of colloid systems. Heterogeneous dispersion systems (lyophobic sols, emulsion, foam, aerosol).
Chemical thermodynamics. Heat capacities, heating and cooling of substances. The first law of thermodynamics. Enthalpy, variation of the reaction enthalpy with temperature.
The second law of thermodynamics. Entropy and its interpretation. Helmholtz and Gibbs free energy. Chemical potential, activity.
Chemical equilibriums, equilibrium constant for homogeneous nad heterogeneous chemical reactions, Van´t Hoff reaction isotherm and isobare. The Le Chatelier’s principle.
Phase equilibrium - conditions of phase equilibrium. Gibbs phase rule, one-component system (Clapeyron and Clausius-Clapeyron equation), two-component (binary) system (ideal and real solutions, Raoult’s law and Henry’s law). Colligative properties of nonelectrolyte solutions - solutions with non-volatile solute. Phase diagram for two-component liquid mixtures (miscible liquids, partially miscible liquids, totally immiscible liquids). Distribution equilibrium.
The chemical kinetics - rate of chemical reaction, order of reaction, molecularity, rate constant, reaction mechanism. Integrated forms of the kinetic equation. The temperature dependence of the rate constant, Arrhenius equation. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions.
Electrochemistry – electrolytes and theory of electrolytic dissociation. Strong electrolytes - activity and activitiy coefficient, Debye-Hückel limiting law. Solubility product. Equilibrium and dissociation in solutions of weak electrolytes - dissociation of week monobasic acids and bases, hydrolysis of salt, buffer solutions. Electrolysis, transport number, electric conductivity of electrolytes. Electrochemistry potentials, electrodes, galvanic cells.
Colloid chemistry - classification of dispersion systems, degree of dispersion. Selected kinetic, electrical and optical properties of colloid systems. Heterogeneous dispersion systems (lyophobic sols, emulsion, foam, aerosol).