1、Physical chemistry物理化学物理化学Physical Chemistry is the branch of chemistry that studies the physical and chemical properties of matter,and it is also essential for developing the modern techniques used to determine the structure and properties of matter,such as new synthetic materials and biological ma
2、cromolecules.Thermodynamic parameter Thermodynamic variable Thermodynamic equilibrium Thermodynamic probability Thermodynamic temperature Thermodynamic property Extensive property volume weight heat capacity internal energy (内能)Intensive property temperature pressure density viscosity System Equilib
3、rium system Nonequilibrium system Homogeneous system Heterogeneous system Open system Closed system Isolated system Adiabatic system One-compound system Isenthalpic process Isentropic process Entropy Adiabatic process Cyclic process Quasistatic process Reversible process Irreversible procesbs Sponta
4、neous process Nonspotaneous process n Work:work is done when an object is moved against an opposing force.it is equivalent to a change in the height of a weight somewhere in the surroundings.n Heat:when the energy of a system changes as a result of a temperature difference between it and its surroun
5、dings,we say that energy has been transferred as heat.n Energy:the energy of a system is its capacity to do work.Heat Heat effect Hesss law Thermochemistry Thermochemistry equationbb Thermochemistry cycle Exothermic reaction Endothermic reaction Heat of reaction Heat of formation Heat of combustion
6、Heat of solution Integral heat of solution Differential heat of solution Heat of sublimation Heat of liquefaction Heat of neutralization Heat of mixing Heat of hydration Heat of fusion Heat of vaporization Heat of dilution Heat capacity C=Q/(T2-T1)Heat capacity at constant pressure(Cp)Heat capacity
7、at constant volume(Cv)Molar heat capacity Calorimeter Calorimetry Energy Bond energy Internal energy(U)Molar internal energy Law of conservation of energy First law of thermodynamics U=U2-U1=Q-WEnthalpy H=U+pVp is the pressure of the system and V is its volume.As U,p and V are all state functions,th
8、e enthalpy is also a state function.The change of enthalpy,H,between any pair of initial and final states is independent of the path between them.Carnot cycle Efficiency of engine Entropy S=SB-SA=(Q/T)R Clausius inequality Principle of entropy increase Thermal entropy Configuration entropy Molar ent
9、ropy Statistical entropy Boltzmann equation Boltzmann constant Gibbs free energy G=H-TS(吉布斯自由能)Second law of thermodynamics S I 0 or S I=0 G T.P 0 or G T.P=0deal gas Nonideal gasFugacity Fugacity coefficientColligative properties of solution Boiling point elevation Freezing point depression Vapor pr
10、essure lowering Osmosis Osmotic pressure Osmotic coefficient Phase equilibrium Number of components K=S-R-R Degree of freedom(f)Phase rule,number of phase=K+2-f Phase change,phase transition Phase diagram Triple point Critical state(超临界状态)Critical phenomenon(超临界现象)Critical constant(超临界常数)Critical po
11、int(超临界点 Critical temperature(超临界温度)Thermochemical kinetics Molecular reaction dynamics Kinetic parameter Reaction path Extent of reaction Reaction time Reaction rate Rate equation Rate constant Overall reaction Elementary reaction Reaction order Zeroth order reaction First order reaction,-dc/dt=k1c
12、 Pseudo first order reaction Second order reaction,-dc/dt=k2c2 Third order reaction Unimolecular reaction Bimolecular reaction Termolecular reaction Activation energy Activation state Thermal activation Photoactivation Reaction mechanism Rate controlling step Simple collision theory Transition state
13、 theory Liquid phase reaction Diffusion controlled reactionl reaction order （反应级数）反应级数）=kAaBbthe overall order of a reaction with a rate law is the sum of the individual order,a+b+Factors that affect the rate of reaction:vThe concentration of the reactants vThe particle size in heterogeneous reactio
14、nsvThe temperature of the reacting system-typically the rate doubles for every 10 degree rise in temperature.（some reactions are affected by light energy instead of heat.）Arrhenius equation lnk=lnA-Ea/RTvThe addition of a suitable catalyst The collision theory:l This states that to react a.particles
15、 must collide b.with enough energy to break existing bonds c.and with the correct orientation to bring reactive sites close together.Increasing the temperature of the system:1.increases the range of kinetic energies;2.increases the average kinetic energy;3.increases the population of particles with
16、more than the activation energy.addition of a catalyst can decrease the required activation energy so that a greater population of particles will collide successfully.A catalyst increases the rate without being used up.it does this by providing a reaction pathway with a lower activation energy through:1.making more collisions have favorable orientation;2.locally increasing concentrations on its surfaces;3.providing a series of simple steps rather than one high energy one;4.providing a better attacking group which is regenerated later;5.increasing the reactivity of the reactive site.
