1. Chapter 5 Chemical Quantities and Reactions
5.5
Types of Reactions

2. 5.5 Types of Reactions Chemical reactions can be classified as
combination reactions.
decomposition reactions.
single replacement reactions.
double replacement reactions.
Combustion reactions

3. Combination In a combination reaction,
two or more elements form one product.
or simple compounds combine to form one product. +
2Mg(s) + O2(g) 2MgO(s)
2Na(s) + Cl2(g) 2NaCl(s)
SO3(g) + H2O(l) H2SO4(aq) A B

4. Decomposition In a decomposition reaction,
one substance splits into two or more simpler substances. +
2HgO(s) Hg(l) + O2(g)
2KClO3(s) KCl(s) + 3 O2(g) A B A B

5. Examples Classify the following reactions as
1) combination or 2) decomposition.
___A. H2(g) + Br2(g) HBr(l)
___B. Al2(CO3)3(s) Al2O3(s) + 3CO2(g)
___C. 4Al(s) + 3C(s) Al4C3(s)

6. Single Replacement In a single replacement reaction,
one element takes the place of a different element in another reacting compound.
Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)
Fe(s) + CuSO4(aq) FeSO4(aq) + Cu(s)

7. Double Replacement In a double replacement,
two elements in the reactants exchange places.
AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
ZnS(s) HCl(aq) ZnCl2(aq) + H2S(g)

8. Combustion Reactions
In a combustion reaction, a carbon-containing compound, usually a fuel, burns in oxygen from the air to produce carbon dioxide (CO2), water (H2O), and energy in the form of heat or a flame.
CH4(g) + 2O2(g) Δ CO2(g) H2O(g) + energy

9. Examples Identify each reaction as 1) combination, 2) decomposition,
3) single replacement, 4) double replacement or, 5) combustion.
A. 3Ba(s) + N2(g) Ba3N2(s)
2Ag(s) + H2S(aq) Ag2S(s) + H2(g)
C2H4(g) + 3O2(g) CO2(g) + 2H2O(g) + energy
C. SiO2(s) + 4HF(aq) SiF4(s) + 2H2O(l)
D. PbCl2(aq) + K2SO4(aq) KCl(aq) + PbSO4(s)
E. K2CO3(s) K2O(aq) + CO2(g)

10. 5.6 Oxidation-Reduction Reactions
An oxidation-reduction reaction
provides us with energy from food.
provides electrical energy in batteries.
occurs when iron rusts.
4Fe(s) + 3O2(g) Fe2O3(s)

11. Electron Loss and Gain An oxidation-reduction reaction involves
a transfer of electrons from one reactant to another.
oxidation as a loss of electrons (OIL).
reduction as a gain of electrons (RIG).

12. Oxidation and Reduction
Copyright © by Pearson Education, Inc.

13. Zn and Cu2+ Zn(s) Zn2+(aq) + 2e- oxidation silver metal
Cu2+(aq) + 2e Cu(s) reduction
blue solution orange

14. Electron Transfer from Zn to Cu2+
Oxidation: loss of electrons
Reduction: gain of electrons

15. Examples Identify each of the following as
1) oxidation or 2) reduction.
__A. Sn(s) Sn4+(aq) e−
__B. Fe3+(aq) e− Fe2+(aq)
__C. Cl2(g) e− Cl-(aq)

16. Writing Oxidation and Reduction Reactions
Write the separate oxidation and reduction reactions for the following equation.
2Cs(s) F2(g) CsF(s)
A cesium atom loses an electron to form cesium ion.
Cs(s) Cs+(s) e− oxidation
Fluorine atoms gain electrons to form fluoride ions.
F2(s) + 2e F−(s) reduction

17. Examples
In light-sensitive sunglasses, UV light initiates an oxidation-reduction reaction. uv light Ag+ + Cl− Ag + Cl A. Which reactant is oxidized? B. Which reactant is reduced?

18. Examples
Identify the substances that are oxidized and reduced in each of the following reactions. A. Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) B. 2Al(s) + 3Br2(g) 2AlBr3(s)

19. 5.7 Mole Relationships in Chemical Equations
The law of conservation of mass indicates that in an
ordinary chemical reaction,
matter cannot be created or destroyed.
no change in total mass occurs in a reaction.
mass of products is equal to mass of reactants.
2 moles of Ag mole of S = mole of Ag2S
2 (107.9 g) (32.1 g) = (247.9 g)
247.9 g reactants = g product

20. Reading Equations in Moles
Consider the following equation: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) This equation can be read in “moles” by placing the word “moles of” between each coefficient and formula. 4 moles of Fe + 3 moles of O2 2 moles of Fe2O3

21. Writing Mole-Mole Factors
A mole-mole factor is a ratio of the moles for any two substances in an equation. 4Fe(s) + 3O2(g) 2Fe2O3(s) Fe and O2 4 moles Fe and 3 moles O2 3 moles O2 4 moles Fe Fe and Fe2O3 4 moles Fe and 2 moles Fe2O3 2 moles Fe2O3 4 moles Fe O2 and Fe2O3 3 moles O2 and 2 moles Fe2O3 2 moles Fe2O3 3 moles O2

22. Examples
Consider the following equation: 3H2(g) + N2(g) 2NH3(g) A. A mole-mole factor for H2 and N2 is 1) 3 moles N2 2) 1 mole N2 3) 1 mole N2 1 mole H2 3 moles H2 2 moles H2 B. A mole-mole factor for NH3 and H2 is 1) 1 mole H2 2) 2 moles NH3 3) 3 moles N2 2 moles NH3 3 moles H2 2 moles NH3

23. Calculations with Mole Factors
How many moles of Fe2O3 can form from 6.0 moles of O2? 4Fe(s) + 3O2(g) 2Fe2O3(s) Equality: 3 mole O2 = 2 mole Fe2O3 Use a mole-mole factor to determine the moles of Fe2O mole O2 x 2 mole Fe2O3 = 4.0 moles of Fe2O3 3 mole O2

24. Example
How many moles of Fe are needed for the reaction of 12.0 moles of O2? 4Fe(s) + 3O2(g) 2Fe2O3(s) 1) 3.00 moles of Fe 2) 9.00 moles of Fe 3) 16.0 moles of Fe

25. 5.8 Mass Calculations for Reactions
Suppose we want to determine the mass (g) of NH3 that can form from 2.50 moles of N2. N2(g) + 3H2(g) 2NH3(g) The plan needed would be moles N2 moles NH3 grams NH3 Equalities:

26. Example
How many grams of O2 are needed to produce mole of Fe2O3 in the following reaction? 4Fe(s) + 3O2(g) 2Fe2O3(s) 1) 38.4 g of O2 2) 19.2 g of O2 3) 1.90 g of O2

27. Calculating the Mass of a Reaction
The reaction between H2 and O2 produces 13.1 g of water. How many grams of O2 reacted? 2 H2(g) + O2(g) 2 H2O(g) ? g 13.1 g The plan and factors would be g H2O mole H2O mole O2 g of O2 molar mole-mole molar mass H2O factor mass O2

28. Calculating the Mass of Product
When 18.6 g of ethane gas, C2H6, burns in oxygen, how
many grams of CO2 are produced?
2C2H6(g) O2(g) CO2(g) + 6H2O(g)
18.6 g ? g
The plan and factors would be
g C2H mole C2H mole CO g of CO2
molar mole-mole molar
mass C2H factor mass CO2

29. Learning Check
Acetylene gas, C2H2, burns in the oxyacetylene torch for welding. How many grams of C2H2 are burned if the reaction produces 75.0 g of CO2?
2C2H2(g) O2(g) CO2(g) + 2H2O(g)
1) g of C2H2
2) g of C2H2
3) g of C2H2

30. Example
How many grams of H2O are produced when 35.8 g of C3H8 react by the following equation? C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) 1) 14.6 g of H2O 2) 58.6 g of H2O 3) 117 g of H2O

31. 5.9 Energy in Chemical Reactions
Collision Theory of Reactions
A chemical reaction occurs when
collisions between molecules have sufficient energy to break the bonds in the reactants.
bonds between atoms of the reactants (N2 and O2) are broken and new bonds (NO) can form.

32. Activation Energy
The activation energy is the minimum energy needed for a reaction to take place.
When a collision provides energy equal to or greater than the activation energy, product can form.

33. Exothermic Reactions C(s) + 2H2(g) CH4(g) + 18 kcal
In an exothermic reaction,
heat is released.
the energy of the products is less than the energy of the reactants.
heat is a product.
C(s) + 2H2(g) CH4(g) + 18 kcal

34. Endothermic Reactions
In an endothermic reaction
Heat is absorbed.
The energy of the products is greater than the energy of the reactants.
Heat is a reactant (added).
N2(g) + O2 (g) kcal NO(g)

35. Example Identify each reaction as 1) exothermic or 2) endothermic.
A. N2 + 3H NH kcal
B. CaCO kcal CaO + CO2
C. 2SO2 + O2 2SO3 + heat

36. Rate of Reaction Reaction rate
is the speed at which reactant is used up
is the speed at which product forms.
Factors that affect the rate of reaction
increases when temperature rises because reacting molecules move faster, providing more colliding molecules with energy of activation.
Increasing concentrations of reactants also increases the rate of reaction because there are more collision between reactants

37. Reaction Rate and Catalysts
A catalyst
increases the rate of a reaction.
lowers the energy of activation.
is not used up during the reaction.

38. Summary of Factors That Increase Reaction Rate

39. Examples
State the effect of each on the rate of reaction as: 1) increases 2) decreases 3) no change A. increasing the temperature. B. removing some of the reactants. C. adding a catalyst. D. placing the reaction flask in ice. E. increasing the concentration of one of the reactants.

40. Example Indicate the effect of each factor listed on the rate of the
following reaction as:
1) increases 2) decreases 3) none
2CO(g) + O2(g) CO2 (g)
raising the temperature
adding O2
adding a catalyst
D. lowering the temperature