WS6_Stoichiometry_Solution

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Worksheet 3: Stoichiometry, Mass Percent, and Theoretical Yield 1. Balance the following chemical reactions: a. 2 CaO(s) + 5 C(s) ® 2 CaC2(s) + 1 CO2(g) b. 4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g)... c. 1 C8H8(l) + 10 O2(g) ® 8 CO2(g) + 4 H2O(g) d. 1 NaHCO3(s) + 1 C2H4O2(aq) ® 1 NaC2H3O2(aq) + 1 CO2(g) + 1 H2O(l) 2. Write balanced chemical equations, including states-of-matter, for the following reactions: a. Dinitrogen pentoxide gas reacts with sodium metal to produce solid sodium nitrate and gaseous nitrogen dioxide. N2O5(g) + Na(s) ® NaNO3(s) + NO2(g) b. A mixture of nitric acid and nitrous acid is formed when water reacts with dinitrogen tetroxide gas. N2O4(g) + H2O(l) ® HNO3(aq) + HNO2(aq) c. Potassium reacts with water to give hydrogen and aqueous potassium hydroxide. 2 K(s) + 2 H2O(l) ® H2(g) + 2 KOH(aq) d. Carbon dioxide reacts with carbon to form carbon monoxide. CO2(g) + C(s) ® 2 CO(g) 3. Iron(III) oxide reacts with carbon monoxide to form iron metal and carbon dioxide gas: 1 Fe2O3(s) + 3 CO(g) ® 2 Fe(s) + 3 CO2(g) In a certain experiment, 5.0 g of iron(III) oxide is reacted with 5.0 g of carbon monoxide gas. a. What mass of iron will be produced, assuming a complete reaction? What is the limiting reactant? Assume excess CO: 5.0 g Fe ( 2O3 ) 1 mol Fe2O3 159.7 g Fe2O3 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 2 mol Fe 1 mol Fe2O3 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 55.85 g Fe 1 mol Fe ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = 3.50 g Fe Assume excess Fe2O3: (5.0 g CO) 1 mol CO 28.01 g CO ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 2 mol Fe 3 mol CO ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 55.85 g Fe 1 mol Fe ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = 6.65 g Fe Theoretical Yield: 3.5 g Fe Limiting Reactant: Fe2O3 b. What mass of carbon dioxide will be produced (the theoretical yield), assuming a complete reaction? We know that Fe2O3 is the limiting reactant, so it will determine the amount of CO formed: 5.0 g Fe ( 2O3 ) 1 mol Fe2O3 159.7 g Fe2O3 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 3 mol CO2 1 mol Fe2O3 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ 44.01 g CO2 1 mol CO2 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = 4.13 g CO2 Theoretical Yield of CO2: 4.1 g [Show More]

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