1. Topic 1 Rate of Reaction

2. Introduction M concentration massg mLL volume (s) (g) (aq) UnitAmountState of Reactant Δ means change Δ in Time Δ in Amount of Reactant or Product Reaction Rate =

3. Time Units s min h moles/s M/min mL/h g/min Rate Units

4. Measuring Reaction Rates Reactants → Products Decrease Increase as you measure them

5. CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) The water concentration does not change- like a drop in a bucket, as the solution is mostly water. increase M / min Concentration / time increase mL / hVolume / time Concentration / time M / s decrease g / min decrease Mass / time Property MeasuredUnits Change

8. Two types of calculations 2. Measure rate of reaction of a substance from given information of other substance Mg + 2HCl  MgCl 2 + H 2 Given= 12 g Mg used in 30 second Find Rate of formation (mole/s) of H 2 ?

9. Two types of calculations 1.Measure rate of reaction of a single substance from given information of the substance Mg + 2HCl  MgCl 2 + H 2 Given= 12 g Mg used in 30 second Find Rate of Mg consumption per second

10. Discussion Time

11. A should tell B and B should rephrase I know how to 1. A.????? B. Do you mean --------- 2. A.????? B. Do you mean --------- 3. A.????? B. Do you mean --------- 4. A.????? B. Do you mean --------- 5. A.????? B. Do you mean ---------

12. A Tell B and B rephrase 1. Rate of reaction formula 2. units 3. Increase and decrease of reactant and product amount 4. Convert time units 5. Convert mass to mole, volume to mole 6. How to draw graph, dependent and independent variables

13. Measurable Changes MassVolume SizePressure ShapeColour TimeTemperature

14. 1. Volume Volume (mL) 4.05.15.96.87.68.3 Time (s) 01530456075 Zn (s) + 2HCl (aq) → H 2(g) + ZnCl 2(aq)

15. Rate in mL H 2 /s= 8.3 - 4.0 mL =0.057 ml/s 75 - 0 s Rate in mole H 2 /min @ STP 0.057 mL s x 1 L 1000 mL x 1 mole 22.4 L x 60 s 1 min = 1.5 x 10 -4 mole/min 1.5 x 10 -4 mole H 2 min x 2 moles HCl 1 mole H 2 x 36.5 gx 60 min = 0.67 g/h 1 mole1 h Rate in g HCl/h

16. 2.Mass of an open container Mass (g) 82.0781.8481.7181.6681.6481.63 Time (s) 01530456075 CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l)

17. 1. Calculate the rate in units of grams CO 2 /s. Rate= (82.07 - 81.63) g =0.0059 g/s 75 s x 1 molex 1 mole CaCO 3 x 100.1 gx 3600 s = 48 g/h 0.0059 g CO 2 s 44.0 g 1 mole CO 2 1 mole1 h 2.Calculate the rate in grams CaCO 3 /h Keep all sig figs on calculator Round final answer

18. 3.Pressure in a closed container Ca (s) +2HOH (l) → Ca(OH) 2(aq) + H 2(g) Diagram

19. 4.Colour of Solution Cu (s) +2AgNO 3(aq) →2Ag (s) +Cu(NO 3 ) 2(aq) clear blue

20. 5.If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 s, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → All 0.895 g is used up and some of the 0.50 M is consumed. Rate= 0.895 g H 2 SO 4 x 1 molex 2 moles NaOH 98.1 g 1 mole H 2 SO 4 0.500 min =0.0365 moles NaOH/min

21. Workbook Questions Page 2 Question 1-5

28. Average Last - First Instanteous

29. Average Last - First Instanteous

30. Average Last - First Instanteous

31. Design an experiment to measure reaction rate, take picture of this slide. Make electronic microsoft word copy send to mrusmanfarooq@hotmail.com Due By Monday mrusmanfarooq@hotmail.com 1.Find a reaction (write equation) use online resources to find. 2.Hypothesis (What measurable change will you be work on?) 3.Is it doable? Do we have equipment to do the reaction? 4.Independent variable 5.Dependent variable 6.Safety concerns 7.Material (What equipment and chemical are needed? ) 8.Procedure (write bulleted points) 9.Data Table (draw table but don’t fill in) 10.Empty graph with labelled variables 11.Discussion Part of hypothesis

32. A Tell B and B rephrase 1. Rate of reaction formula, rearrange formula 2. Units and prefix conversion 3. Increase and decrease of reactant and product amount 4. Convert time units 5. Convert mass to mole, volume to mole 6. How to draw graph, dependent and independent variables 7. Rate of reaction of single substance 8. Rate of reaction of a substance from other substance 9. Average and Instanteous reaction rate calculations