ࡱ> proy bjbj b8{{\ZZ$P(,TTn4LQnSnSnSnSnSnSn$przwnwnnQnQnem@_^HFmhJ=nn0nh2s<2sm2smtZ)@i4wnwnn2sZ z: Problem Session 3 Chapters: 4, 8, 9, 10, and 14 Directions: Answer each of the following questions in complete sentences where appropriate. Be sure to show all of your work and report your answers to the correct number of significant figures. Question 1. Write a balanced net ionic equation for the reaction, if any that occurs in each of the following cases. Assume that all soluble reactants are added in the form of aqueous solutions. Indicate gases and precipitates that are formed, as well as insoluble solid reactants. If no reaction occurs, then write NO RXN, and do not write a balanced equation. Be sure to balance your equations and include your phase labels. potassium hydroxide + sodium hydroxide ( sodium acetate + hydrochloride acid ( zinc bromide + potassium phosphate ( hydrochloric acid + calcium ( nitric acid + barium hydroxide ( ammonium nitrate + sodium hydroxide ( Question 2. When a hydrocarbon burns, water and carbon dioxide are produced. The density of gasoline is 0.79 g/mL. Assume that gasoline is completely made up of octane, C8H18. Write the equation for the combustion of octane: Calculate the mass of water produced from the combustion of 2.0 L of gasoline. Question 3. If 11.0 pounds of iron(III) oxide is reacted with excess carbon monoxide gas to yield solid iron ore and carbon dioxide gas, how many grams of iron ore is produced? Question 4. What mass of aluminum in kg is needed to react with 10.0 kg of chromium(III) oxide to produce chromium metal and aluminum oxide? Question 5. Suppose that 24.3 grams of calcium carbonate are decomposed with heat a. Write the decomposition reaction b. How many grams of product(s) is formed? Question 6. Complete the following conversions: 55.8 psi to kPa 780.567 mm Hg to atm Question 7. What is the molar volume of a gas at 45 C and 776 torr? Remember that the universal gas constant is 0.0821 L atm/mol K. Question 8. A 5.0 L sample of chlorine gas at 2.2 atm is compressed isothermally to a volume of 0.100L. What is the pressure of the gas at this volume? Question 9. A flexible container has a pressure of 150 lb/in2 and a volume of 350 mL at 25C. What is the pressure in atmospheres if 200 mL of carbon dioxide gas is released from the container? Question 10. What is the density in g/L of oxygen gas at STP? Question 11. If 8.00 g of oxygen are injected into a 10.0 L cylinder full of hydrogen of unknown amount, at a pressure of 635 torr at 29C, and the mixture is ignited and water is formed, how many moles of water are formed? ___H2 (g) + ___O2 (g) ( ___H2O (l) Question 12. How many molecules of CO2 are in 35.0 L CO2 gas at 1.2 atm and 5 C? Question 13. A sample of a carbon-hydrogen compound is found to contain 9.60 g carbon and 2.42 g hydrogen. At STP, 762 mL of gas has a mass of 1.02 g. What is the molecular formula for the compound? Question 14. In the formation of smog, nitrogen and oxygen gas react to form nitrogen dioxide. How many grams of NO2 will be produced when 2.0 L nitrogen at 840 mm Hg and 24 C are completely reacted? ___N2 (g) + ___O2 (g) ( ___NO2 (g) Question 15. A reaction mixture contains 70.0 g of Fe3O4 and 12.0 g of O2 and the reaction below is allowed to occur. Use an ICE table. 4 Fe3O4 (s) + O2 (g) ( 6 Fe2O3 (s) How many grams of Fe2O3 will be generated? How much of each reagent will remain after the reaction has gone to completion? If 59.6 grams of Fe2O3 are produced, what is the percent yield of the reaction? Question 16. A mixture of 60.0% ZnS and 40.0% CuS is heated in air until the sulfides are completely converted to oxides as shown by the following equations. 2 ZnS (s) + 3 O2 (g) ( 2 ZnO (s) + 2 SO2 (g) 2 CuS (s) + 3 O2 (g) ( 2 CuO (s) + 2 SO2 (g) How many grams of SO2 are produced from the reaction of 82.5 g of the sulfide mixture?     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