last night’s homework: problems 4-6 on page 282 questions 7-11 on page 283
TRANSCRIPT
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Last night’s homework:
Problems 4-6 on page 282
Questions 7-11 on page 283
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Write chemical equations for each of the following reactions.
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.
FeCl3 + NaOH → Fe(OH)3 + NaCl
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FeCl3 + NaOH → Fe(OH)3 + NaCl
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FeCl3 + NaOH → Fe(OH)3 + NaCl
FeClNaOH
FeClNaOH
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FeCl3 + NaOH → Fe(OH)3 + NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 1Na 1O 3H 3
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FeCl3 + NaOH → Fe(OH)3 + NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 1Na 1O 3H 3
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FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 1Na 1O 3H 3
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FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 3Na 3O 3H 3
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FeCl3 + NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 3Na 3O 3H 3
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FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 1O 1H 1
Fe 1Cl 3Na 3O 3H 3
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FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 3O 3H 3
Fe 1Cl 3Na 3O 3H 3
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FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Fe 1Cl 3Na 3O 3H 3
Fe 1Cl 3Na 3O 3H 3
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5. Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas.
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5. Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas.
CS2 + O2 → CO2 + SO2
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CS2 + O2 → CO2 + SO2
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CS2 + O2 → CO2 + SO2
COS
COS
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CS2 + O2 → CO2 + SO2
C 1O 4S 1
C 1O 2S 2
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CS2 + O2 → CO2 + 2SO2
C 1O 4S 1
C 1O 2S 2
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CS2 + O2 → CO2 + 2SO2
C 1O 6S 2
C 1O 2S 2
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CS2 + 3O2 → CO2 + 2SO2
C 1O 6S 2
C 1O 2S 2
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CS2 + 3O2 → CO2 + 2SO2
C 1O 6S 2
C 1O 6S 2
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CS2 + 3O2 → CO2 + 2SO2
C 1O 6S 2
C 1O 6S 2
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6. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas and aqueous zinc sulfate.
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6. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas and aqueous zinc sulfate.
Zn + H2SO4 → H2 + ZnSO4
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Zn + H2SO4 → H2 + ZnSO4
ZnHSO
ZnHSO
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Zn + H2SO4 → H2 + ZnSO4
Zn 1H 2S 1O 4
Zn 1H 2S 1O 4
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7. List three types of evidence that a chemical reaction has occurred.
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7. List three types of evidence that a chemical reaction has occurred.
Changes in:
• Temperature
• Color
Appearance of:
• Odor
• Gas bubbles
• Solid precipitate
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8. Compare and contrast a skeleton equation and a chemical equation.
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8. Compare and contrast a skeleton equation and a chemical equation.
Both show formulas of reactants and products.
Chemical equation also shows relative amounts.
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9. Why is it important that a chemical equation be balanced?
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9. Why is it important that a chemical equation be balanced?
Mass is neither created nor destroyed.
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10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula?
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10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula?
No
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10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula?
NoH2O → H2 + O2
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10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula?
NoH2O → H2 + O2
H2O2 → H2 + O2
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11. Why is it important that to reduce the coefficients in a balanced equation to the lowest possible whole-number ratio?
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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.
.