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 TimeΔ means change

State of Reactant or Product Amount Unit 

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

Δ in TimeΔ means change

State of Reactant Amount Unit 

(s)

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

Δ in TimeΔ means change

State of Reactant Amount Unit 

(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 TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

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

Δ in TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(g)

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

Δ in TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(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 TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(g) volume mL, 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 TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(g) volume mL, 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 TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(g) volume mL, 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 TimeΔ means change

State of Reactant Amount Unit 

(s) mass g  

(g) volume mL, or L 

(aq) concentration M

Time Units

Time Units seconds minutes hours  

Time Units seconds minutes hours  

Rate Units

Time Units seconds minutes hours  

Rate Units g/min mL/h moles/s

Measuring Reaction Rates  Reactants → Products 

   

Measuring Reaction Rates Reactants → Products 

Decrease .   

Measuring Reaction Rates Reactants → Products 

Decrease Increase as you measure them.   

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass of CaCO3(s)

CaCO3(s)+ HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration M

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration M increase

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration M increase

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration M increase

CaCO3(s)+ 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Property Measured Units Change

Mass g decrease

Concentration M decrease

Volume mL increase

Concentration M increase

The water concentration does not change enough to measure. It increases as does a drop in a bucket.

1. Volume of H2

Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)

 Diagram

Volume (mL)

Time (s) 0 15 30 45 60 75

1. Volume of H2

Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)

 Diagram

Volume (mL) 4.0 5.1 5.9 6.8 7.6 8.3

Time (s) 0 15 30 45 60 75

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL =  75 s

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 mL/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL s

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x s 1000 mL

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole s 1000 mL 22.4 L  

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = s 1000 mL 22.4 L 1 min 

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min 

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

1.5 x 10-4 mole H2

min

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

1.5 x 10-4 mole H2 x 2 moles HCl

min 1 mole H2

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

1.5 x 10-4 mole H2 x 2 moles HCl x 36.5 g

min 1 mole H2 1 mole

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

1.5 x 10-4 mole H2 x 2 moles HCl x 36.5 g x 60 min

min 1 mole H2 1 mole 1 h

Calculations

Rate in mL H2 /s = 8.3 - 4.0 mL = 0.057 ml/s  75 s

 Rate in mole H2/min @ STP

 0.057 mL x 1 L x 1 mole x 60 s = 1.5 x 10-4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

1.5 x 10-4 mole H2 x 2 moles HCl x 36.5 g x 60 min = 0.67 g/h

min 1 mole H2 1 mole 1 h

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

Mass (g) 82.07 81.84 81.71 81.66 81.64 81.63

Time (s) 0 15 30 45 60 75

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2

s

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2 x 1 mole

s 44.0 g

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2 x 1 mole x 1 mole CaCO3

s 44.0 g 1 mole CO2

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2 x 1 mole x 1 mole CaCO3 x 100.1 g

s 44.0 g 1 mole CO2 1 mole

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2 x 1 mole x 1 mole CaCO3 x 100.1 g x 3600 s s 44.0 g 1 mole CO2 1 mole 1 h

2. Mass of an open container CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

Diagram

1. Calculate the rate in units of grams CO2/s.

Rate = (82.07 - 81.63) g = 0.0059 g/s75 s

2. Calculate the rate in grams CaCO3/h

0.0059 g CO2 x 1 mole x 1 mole CaCO3 x 100.1 g x 3600 s = 48 g/h s 44.0 g 1 mole CO2 1 mole 1 h

3. Pressure in a closed container Ca(s) + 2HOH(l) → Ca(OH)2(aq) + H2(g)

 Diagram

4. Colour of Solution Cu(s) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq)

  clear blue

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate =

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate = 0.895 g H2SO4

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate = 0.895 g H2SO4 x 1 mole

98.1 g

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate = 0.895 g H2SO4 x 1 mole x 2 moles NaOH

98.1 g 1 mole H2SO4

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate = 0.895 g H2SO4 x 1 mole x 2 moles NaOH

98.1 g 1 mole H2SO4

0.500 min

5. If 0.895 g of H2SO4 is neutralized with 0.50 M NaOH

in 30.0 seconds, what is the reaction rate in moles NaOH /min.

H2SO4 + 2NaOH →

The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed.

Rate = 0.895 g H2SO4 x 1 mole x 2 moles NaOH

98.1 g 1 mole H2SO4

0.500 min

= 0.036 moles NaOH/min