Unit 1 Kinetics Reaction Rates Read Hebdon Chapter 1.

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Presentation transcript:

Unit 1 Kinetics Reaction Rates Read Hebdon Chapter 1

Introduction Chemical Kinetics

Introduction Chemical Kinetics is the study of the rates of chemical reactions.

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate =

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of Reactant or ProductAmountUnit

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)mass

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volume

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq)

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq) concentration

Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq) concentrationM

Time Units

Time Unitssecondsminuteshours

Time Unitssecondsminuteshours Rate Units

Time Unitssecondsminuteshours Rate Unitsg/minmL/hmoles/s

Measuring Reaction Rates Reactants→Products

Measuring Reaction Rates Reactants→Products Decrease.

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

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massof CaCO 3(s)

CaCO 3(s) +HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massg

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease Concentration

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationM

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease Volume

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemL

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease Concentration

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationM

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease The water concentration does not change enough to measure. It increases as does a drop in a bucket.

1.Volume of H 2 Zn (s) + 2HCl (aq) → H 2(g) + ZnCl 2(aq) Diagram Volume (mL) Time (s)

1.Volume of H 2 Zn (s) + 2HCl (aq) → H 2(g) + ZnCl 2(aq) Diagram Volume (mL) Time (s)

Calculations Rate in mL H 2 /s= mL = 75 s

Calculations Rate in mL H 2 /s= mL =0.057 mL/s 75 s Rate in mole H 2 STP mL s

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x s 1000 mL

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole s 1000 mL 22.4 L

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= s 1000 mL 22.4 L 1 min

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x mole H 2 min

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x mole H 2 x 2 moles HCl min 1 mole H 2

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x mole H 2 x 2 moles HCl x 36.5 g min 1 mole H 2 1 mole

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x mole H 2 x 2 moles HCl x 36.5 g x 60 min min 1 mole H 2 1 mole1 h

Calculations Rate in mL H 2 /s= mL =0.057 ml/s 75 s Rate in mole H 2 STP mL x 1 L x 1 mole x 60 s= 1.5 x mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x mole H 2 x 2 moles HCl x 36.5 g x 60 min = 0.67 g/h min 1 mole H 2 1 mole1 h

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

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s.

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 s

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 x 1 mole s 44.0 g

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 x 1 mole x 1 mole CaCO 3 s 44.0 g 1 mole CO 2

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 x 1 mole x 1 mole CaCO 3 x g s 44.0 g 1 mole CO 2 1 mole

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 x 1 mole x 1 mole CaCO 3 x g x 3600 s s 44.0 g 1 mole CO 2 1 mole 1 h

2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=( ) g = g/s 75 s 2.Calculate the rate in grams CaCO 3 /h g CO 2 x 1 mole x 1 mole CaCO 3 x g x 3600 s = 48 g/h s 44.0 g 1 mole CO 2 1 mole 1 h

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

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

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH →

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole 98.1 g

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO 4

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO min

5. If g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO min =0.036 moles NaOH/min