<p>Name ______Per______Date______</p><p>REVIEW Unit 5 - Stoichiometry</p><p>Balancing Equations 1. Balance the following equations:</p><p> a) ___Cr (s) + ___O2 (g)  ___Cr2O3 (s) 4 + 3  2</p><p> b) ___Cu2S (s) + ___O2 (g)  ___Cu (s) + ___SO2 (g) 1 + 1  2 + 1</p><p> c) ___C6H5CH3 (ℓ) + ___O2 (g)  ___H2O (ℓ) + ___CO2 (g) 1 + 9  4 + 7</p><p>2. Balance the following equations and name the reaction products:</p><p> a) ___Fe2O3 (s) + ___Mg (s)  ___MgO (s) + ___Fe (s) 1 + 3  3 + 2 (Magnesium Oxide; Iron)</p><p> b) ___AlCl3 + (s) + ___H2O (ℓ)  ___Al(OH)3 (s) + ___HCl (aq) 1 + 3  1 + 3 (Aluminum Hydroxide; Hydrochloric Acid)</p><p> c) ___NaNO3 (s) + ___H2SO4 (aq)  ___Na2SO4 (s) + ___HNO3 (g)</p><p>2 + 1  1 + 2 (Sodium Sulfate; Nitric Acid)</p><p> d) ___NiCO3 (s) + ___HNO3 (aq)  ___Ni(NO3)2 (aq) +___CO2 (g) + ___H2O (ℓ) 1 + 2  1 + 1 + 1 (nickel II nitrate; carbon dioxide; water)</p><p>3. Balance the following equations: a) The synthesis of urea , a common fertilizer</p><p>___CO2 (g) + ___NH3 (g)  ___NH2CONH2 (s) + ___H2O (ℓ)</p><p>1 + 2  1 + 1</p><p> b) Reactions used to make uranium (VI) fluoride for the enrichment of natural uranium</p><p>___UO2 (s) + ___HF (aq)  ___UF4 (s) + ___H2O (ℓ) 1 + 4  1 + 2</p><p>___UF4 (s) + ___F2 (g)  ___UF6 (s) 1 + 1  1 c) The reaction to make titanium (IV) chloride, which is then converted to titanium metal</p><p>___TiO2 (s) + ___Cl2 (g) + ___C (s)  ___TiCl4 (ℓ) + ___CO (g) 1 + 2 + 2  1 + 2</p><p>___TiCl4 (ℓ) + ___Mg (s)  ___Ti (s) + ___MgCl2 (s)</p><p>1 + 2  1 + 2</p><p>Types of Rxns</p><p>1 Name ______Per______Date______</p><p>Directions: Write out the chemical equation for each reaction AND identify the type reaction. Remember to write (s), (ℓ), (g), or (aq) next to each substance.</p><p>4. Zinc metal + lead (II) nitrate yield zinc (II)nitrate + lead metal</p><p>5. Aluminum bromide solution + chlorine gas yield aluminum chloride solution + bromine gas</p><p>6. Sodium phosphate + calcium chloride yield calcium phosphate + sodium chloride</p><p>7. Aluminum metal + hydrochloric acid yield aluminum chloride + hydrogen gas</p><p>8. Hydrogen gas + nitrogen monoxide yield water + nitrogen gas</p><p>9. Copper metal heated with oxygen gives solid copper (II) oxide.</p><p>10. Mercury (II) nitrate solution reacts with potassium iodide solution to give mercury (II) iodide precipitate and potassium nitrate solution.</p><p>11. Aluminum metal and sulfuric acid yield aqueous aluminum sulfate and hydrogen gas.</p><p>2 Name ______Per______Date______</p><p>12. Acetic acid and lithium hydroxide solution produce water and aqueous lithium acetate.</p><p>13. Sulfur dioxide gas reacts with oxygen on a platinum catalyst surface to produce sulfur trioxide gas.</p><p>14. Sodium metal reacts with water to give sodium hydroxide solution and hydrogen gas.</p><p>15. Heating solid potassium chlorate in the presence of a manganese dioxide catalyst produces potassium chloride and oxygen gas.</p><p>General Stoichiometry 16. Aluminum reacts with oxygen to give aluminum oxide.</p><p>4 Al (s) + 3O2 (g) 2 Al2O3 (s)</p><p>If you have 6.0 mol of Al, how many moles of O2 are needed for complete reaction? </p><p>What mass of Al2O3, in grams, can be produced?</p><p>4.5 mol O2; 310 g Al2O3</p><p>17. Suppose 16.04 g of methane, CH4, is burned in oxygen. a) What are the products of the reaction?</p><p>CO2 and H2O</p><p> b) What is the balanced equation for the reaction?</p><p>1 CH4 (g) + 2 O2 (g)  1 CO2 (g) + 2 H2O (l)</p><p> c) What mass of O2, in grams, is required for complete combustion of the methane?</p><p>63.99 g O2</p><p>3 Name ______Per______Date______</p><p> d) What is the total mass of products expected from 16.04 g of methane?</p><p>80.03 g products</p><p>18. Like many metals, aluminum reacts with a halogen to give a metal halide</p><p>2 Al (s) + 3 Br2 (ℓ)  Al2Br6 (s) </p><p>What quantity of Br2, in grams, is requried for complete reaction with 2.56 g of Al? </p><p>What mass of solid Al2Br6 is expected?</p><p>22.7 g Br2; 25.3 g Al2Br6</p><p>19. Iron reacts with oxygen to give iron (III) oxide, Fe2O3. a) Write a balanced equation for the reaction.</p><p>4 Fe (s) + 3 O2 (g)  2 Fe2O3 (s)</p><p> b) If an ordinary iron nail (assumed to be pure iron) has a mass of 2.68 g, what mass </p><p>(in grams) of Fe2O3 does it produce if the nail is converted completely to this oxide?</p><p>3.83 g Fe2O3</p><p> c) What mass of O2 (in grams) is required for the reaction?</p><p>1.15 g O2</p><p>20. The metabolic disorder diabetes causes a buildup of acetone (CH3COCH3) in the blood of untreated victims. Acetone, a volatile compound, is exhaled, giving the breath of untreated diabetics a distinctive odor. The acetone is produced by a breakdown of fats in a series of reactions. The equation for the last step is </p><p>CH3COCH2CO2H CH3COCH3 + CO2 What quantity of acetone can be produced from 125 mg of acetoacetic acid </p><p>(CH3COCH2CO2H)?</p><p>71.2 mg acetone</p><p>4 Name ______Per______Date______</p><p>Limiting Reactant and Percent Yield</p><p>21. Aluminum chloride, AlCl3, is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the following balanced equation:</p><p>2 Al (s) + 3 Cl2 (g)  2 AlCl3 (s) </p><p> a) Which reactant is limiting if 2.70 g of Al and 4.05 g of Cl2 are mixed?</p><p>Cl2 is the LR</p><p> b) What mass of AlCl3 can be produced from 2.70 g of Al and 4.05 g of Cl2?</p><p>5.08 g AlCl3</p><p> c) What mass of the excess reactant remains when the reaction is completed?</p><p>1.67 g Al</p><p>22. Methanol, CH3OH, is a clean-burning, easily handled fuel. It can be made by the direct </p><p> reaction of CO and H2 (obtained from heating coal with steam):</p><p>CO (g) + 2 H2 (g) CH3OH (ℓ)</p><p> a) Starting with a mixture of 12.0 g of H2 and 74.5 g of CO, which is the limiting reactant? </p><p>CO is the LR</p><p> b) What mass of the excess reactant (in grams) remains after reaction is complete? </p><p>1.3 g H2 </p><p> c) What is the theoretical yield of the methanol?</p><p>85.2 g CH3OH</p><p>23. Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride.</p><p>CaO (s) + 2 NH4Cl (s)  2 NH3 (g) + H2O (g) + CaCl2 (s)</p><p>5 Name ______Per______Date______</p><p> a) If 112 g of CaO and 224 g of NH4Cl are mixed, what is the maximum possible </p><p> yield of NH3? </p><p>68.0 g NH3</p><p> b) What mass of the excess reactant remains after the maximum amount of ammonia has been formed?</p><p>10.0 g NH4Cl remains</p><p>24. Ammonia gas can be prepared by the following reaction:</p><p>CaO (s) + 2 NH4Cl (s) 2 NH3 (g) + H2O (g) + CaCl2 (s) If 103 g of ammonia is obtained, but the theoretical yield is 136 g, what is the percent yield of this gas?</p><p>75.7 % yield</p><p>25. The reaction of zinc and chlorine has been used as the basis of a car battery.</p><p>Zn (s) + Cl2 (g)  ZnCl2 (s) </p><p> a) What is the theoretical yield of ZnCl2 if 35.5 g of zinc is allowed to react with excess chlorine? </p><p>74.0 g ZnCl2</p><p> b) If only 65.2 g of zinc chloride is obtained, what is the percent yield of the compound?</p><p>88.1% yield</p><p>6</p>