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Chapter 9 – Chemical Quantities

Chapter 9 – Chemical Quantities. The Physical Meaning of Chemical Equations Solving Stoichiometry Problems Limiting Reactants Percent Yield. Example 1. Given: 4 Fe (s) + 3 O 2 (g)  2 Fe 2 O 3 (s) a. How many moles of iron (III) oxide can be formed from 8.0 moles of iron metal?

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Chapter 9 – Chemical Quantities

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  1. Chapter 9 – Chemical Quantities • The Physical Meaning of Chemical Equations • Solving Stoichiometry Problems • Limiting Reactants • Percent Yield

  2. Example 1 Given: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) a. How many moles of iron (III) oxide can be formed from 8.0 moles of iron metal? b. How many moles of oxygen gas are needed to react with this iron? c. How many moles of iron are needed to produce 5.0 moles of iron (III) oxide?

  3. Example 2 Given the following unbalanced chemical equation, predict how many moles of carbon dioxide will be formed when 10.0 moles of ethane, C2H6, are burned completely. C2H6(g) + O2(g) CO2(g) + H2O(g)

  4. Example 3 How many grams of water can be formed from the decomposition of 1.00 g of sugar, C12H22O11? How much carbon will be formed? C12H22O11(s)  12 C(s) + 11 H2O(l)

  5. Example 4 Given the following balanced equation, Fe2O3(s) + 3 CO (g) 2 Fe (s) + 3 CO2(g) how many grams of iron can be produced from 2.0 g of Fe2O3 reacting with excess CO?

  6. Example 5 You wish to produce 1.0 kg of sodium metal via the electrolysis of molten sodium chloride. How many kg of sodium chloride will be needed? 2 NaCl(l)  2 Na(s) + Cl2(g)

  7. Example 6 How many moles of oxygen gas are needed to completely burn 1.0 gallon of gasoline? Assume that gasoline is pure octane, C8H18, and that it has a density of 0.703 g/mL. The products of the combustion reaction will be carbon dioxide gas and water vapor.

  8. Example 7 If 5.0 moles NaBr and 5.0 moles Cl2 are combined, how much bromine can be formed? 2 NaBr(s) + Cl2(g)  2 NaCl(s) + Br2(l)

  9. Example 8 If 35.4 g of CO are combined with 10.2 g of H2, how many grams of CH3OH can be formed? CO (g) + 2 H2 (g)  CH3OH(g)

  10. Example 9 If 15.0 g of CS2 are combined with 35.0 g of O2, how many grams of SO2 can be formed? CS2(g) + 3 O2(g) CO2(g) + 2 SO2(g)

  11. Example 10 2 H2(g) + CO(g) CH3OH(l) a. If 68.5 kg of CO reacts with 8.60 kg of H2, calculate the theoretical yield of methanol that can be formed. b. If this reaction mixture actually produces 3.57x104 g of methanol, what is the percent yield of this reaction?

  12. Example 11 CS2(g) + 3 O2(g) CO2(g) + 2 SO2(g) When 15.0 g of CS2 burns in excess oxygen with a 78.6% yield, what mass of SO2 is produced?

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