1. §9.2 Reaction rate and rate equation

2. The rate (r): concentration change of a reactant or a product per unit time. 2.1 expression of reaction rate mean rate instantaneous rate: Physical meaning: t1t1 t c t c t1t1 t2t2 c1c1 c2c2 Initial instantaneous rate? N 2 + 3H 2 == 2NH 3

3. Extent of reaction or advancement (  ) where i is the stoichiometric coefficient of the reaction. True rate of the reaction or rate of conversion (J): Unit? For general reaction: aA + bB  gG + hH When the extent of reaction is d 

4. When the reaction takes place in a container with constant volume Define rate Unit?

5. 2.2 measurement of reaction rate Physical meaning: slope of the c ~ t curve kinetic curve tt = 0t = t c (1) How to record time? (2) How to measure instantaneous concentration?

6. The concentration of the species can be measured using either chemical or physical methods. CH 3 COOC 2 H 5 + NaOH  CH 3 COONa + C 2 H 5 OH The reaction can be stopped by removing of CH 3 COOC 2 H 5, and the consumption of NaOH can be determined by chemical titration. For example: t = 0 t = t 1 t = t 2

7. The change in physical properties of the reaction system which relates to the concentration of reactants or products can be usually chosen as indicator of the progress of the reaction.

8. C 12 H 22 O 11 + H 2 O  C 12 H 22 O 11 + C 12 H 22 O 11 sucrose glucose fructose Substancesucroseglucosefructose [  ] D 25 +66.5 o +52 o - 92 o The rotation angle of the 1:1 mixture of glucose and fructose is –20 o We still use in it in our physical chemistry laboratory t1t1 t2t2  20 [][] []2[]2 []1[]1 66.5 t Wilhelmy in 1850.

9. CH 3 COOC 2 H 5 + NaOH  CH 3 COONa + C 2 H 5 OH CH 3 COOC 2 H 5 + NaOH  CH 3 COONa + C 2 H 5 OH the rate of which can be monitored using pH meter or conductometer. N 2 O 5 = N 2 O 4 + 0.5 O 2 When this reaction takes place in a container with constant volume, the rate of the reaction can be monitored by measuring the pressure change. And when this reaction takes place under constant pressure, the advance of the reaction can be monitored by measuring the volume increase. dilatometer.

10. Stretch of epoxy group FTIR spectroscopy

11. The physical parameters usually used for monitoring reaction process includes volume, pressure, electric conductance, pH, refractive index, thermal conductivity, polarimetry, spectrometry, chromatography, etc. Analyzing methods: 1)Static method 2) Flow method 1) Real time analysis 2) Quenching All the above methods are valid only for reactions with half-lives of at least a few seconds, i.e., “slow” reaction. For fast reaction of half-lives ranging between 10 0 ~ 10 -11 s, special methods are required.

12. Stable flow: l  t Flow method Difficulties in study on kinetics Mixerdetector Moving direction

13. 2.3 Rate equation and the law of mass action The concentration-dependence of rate: r = r(c i ) = r(c A, c B, c C …) Where c i represents concentration of individual specie present in rate equation. In many instances, the rate of a reaction is proportional to the concentrations of the reactants raised to some power. rate equation Rate law

14. For example: H 2 + I 2 = 2 HI H 2 + Cl 2 = 2 HCl Where rate coefficient/constant (k) is a proportionality constant /coefficient independent of concentration. The exponent shows the effect of concentration on the reaction rate. In 1895, Noyes defined them as partial order of the reactant.

15. ,  is the partial order of the reaction with respect to A or B, respectively. This implies that the reaction obeying rate law is first-order in H 2 and 0.5-order in Cl 2. the sum of the partial order n =  +  +  +… is the overall order of the reaction, or more simply, the reaction order. The overall order is 1.5.

16. 2SO 2 + O 2  2SO 3 is first-order in SO 2, -0.5-order in SO 3 and 0.5 order overall. n, , , , etc., different from the stoichiometric coefficient, may be integers, decimals, of plus or minus values. Rate law must be determined from measurements of reaction rate and cannot be deduced from the reaction stoichiometry.

17. For elementary reaction,  = a,  = b, etc. Partial order = stoichiometric coefficient Reaction order = number of molecules involved in the reaction For example: 2I + H 2 = 2HI Law of mass action valid only for elementary reaction

18. An exercise

19. Group work: Write the differential form of rate equation and deduce the integration rate equations of reactions with simple orders. A member of a chosen group will be asked to deduce the equation on blackboard this Thursday.