Last night’s homework:
Problems 4-6 on page 282
Questions 7-11 on page 283
Write chemical equations for
each of the following reactions.
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
4. In water, iron(III) chloride reacts with
sodium hydroxide, producing solid
iron(III) hydroxide and sodium
chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
FeCl3 + NaOH → Fe(OH)3 + NaCl
FeCl3 + NaOH → Fe(OH)3 + NaCl
Fe
Cl
Na
O
H
Fe
Cl
Na
O
H
FeCl3 + NaOH → Fe(OH)3 + NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
1
1
3
3
FeCl3 + NaOH → Fe(OH)3 + NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
1
1
3
3
FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
1
1
3
3
FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
3
3
3
3
FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
3
3
3
3
FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
1
1
1
Fe
Cl
Na
O
H
1
3
3
3
3
FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
3
3
3
Fe
Cl
Na
O
H
1
3
3
3
3
FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe
Cl
Na
O
H
1
3
3
3
3
Fe
Cl
Na
O
H
1
3
3
3
3
5. Liquid carbon disulfide reacts with
oxygen gas, producing carbon
dioxide gas and sulfur dioxide gas.
5. Liquid carbon disulfide reacts with
oxygen gas, producing carbon
dioxide gas and sulfur dioxide gas.
CS2 + O2 → CO2 + SO2
CS2 + O2 → CO2 + SO2
CS2 + O2 → CO2 + SO2
C
O
S
C
O
S
CS2 + O2 → CO2 + SO2
C
O
S
1
2
2
C
O
S
1
4
1
CS2 + O2 → CO2 + 2SO2
C
O
S
1
2
2
C
O
S
1
4
1
CS2 + O2 → CO2 + 2SO2
C
O
S
1
2
2
C
O
S
1
6
2
CS2 + 3O2 → CO2 + 2SO2
C
O
S
1
2
2
C
O
S
1
6
2
CS2 + 3O2 → CO2 + 2SO2
C
O
S
1
6
2
C
O
S
1
6
2
CS2 + 3O2 → CO2 + 2SO2
C
O
S
1
6
2
C
O
S
1
6
2
6. Solid zinc and aqueous hydrogen
sulfate react to produce hydrogen
gas and aqueous zinc sulfate.
6. Solid zinc and aqueous hydrogen
sulfate react to produce hydrogen
gas and aqueous zinc sulfate.
Zn + H2SO4 → H2 + ZnSO4
Zn + H2SO4 → H2 + ZnSO4
Zn
H
S
O
Zn
H
S
O
Zn + H2SO4 → H2 + ZnSO4
Zn
H
S
O
1
2
1
4
Zn
H
S
O
1
2
1
4
7. List three types of evidence that a
chemical reaction has occurred.
7. List three types of evidence that a
chemical reaction has occurred.
Changes in:
• Temperature
• Color
Appearance of:
• Odor
• Gas bubbles
• Solid precipitate
8. Compare and contrast a skeleton
equation and a chemical equation.
8. Compare and contrast a skeleton
equation and a chemical equation.
Both show formulas of reactants
and products.
Chemical equation also shows
relative amounts.
9. Why is it important that a chemical
equation be balanced?
9. Why is it important that a chemical
equation be balanced?
Mass is neither
created nor
destroyed.
10. When balancing a chemical equation,
can you adjust the number that is
subscripted to a substance formula?
10. When balancing a chemical equation,
can you adjust the number that is
subscripted to a substance formula?
No
10. When balancing a chemical equation,
can you adjust the number that is
subscripted to a substance formula?
No
H2O → H2 + O2
10. When balancing a chemical equation,
can you adjust the number that is
subscripted to a substance formula?
No
H2O → H2 + O2
H2O2 → H2 + O2
11. Why is it important that to reduce the
coefficients in a balanced equation to
the lowest possible whole-number
ratio?
11. Why is it important that to reduce the
coefficients in a balanced equation to
the lowest possible whole-number
ratio?
Clearly shows the
relative amounts.
.