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10/16/2014 Work through Challenge Problem Set 5, DUE tonight at 11 pm Midterm Exam 2: Next Tuesday, Oct. 21st: ◦ Bring a NONPROGRAMMABLE Scientific Calculator & an ORANGE Parscore Sheet ◦ Check out Canvas for Study Guide & Practice Exam from last year Practice Problems: C8H18 ______________ Na2C2O4 ______________ C7H12 ______________ CH3COOH ______________ C6H2CH3(NO2)3 ______________ C3H6N3(NO2)3 ______________ Practice Problems: Determine the empirical and molecular formulas for an unknown compound based on the information provided below: • Mass Composition Data from Elemental Analysis: • 51.28 % Carbon • 9.40 % Hydrogen • 27.35 % Oxygen • 11.97 % Nitrogen • Molar Mass from Mass Spectrometry Data: 234 g/mol 1 10/16/2014 Practice Problems: Determine the empirical and molecular formulas based on the information provided below: • 11.800 grams of an unknown sample containing only C, H, & N is found to have 7.200 g of carbon, & 4.198 g of nitrogen. • Molar Mass from Mass Spectrometry Data: 354.3 g/mol Practice Problems: Write the balanced chemical equations for the reactions below: • Combustion of butane, C4H10 • Combustion of sucrose, C12H22O11 • Aluminum metal reacts with manganese (IV) oxide to produce aluminum oxide and manganese metal • Ammonium phosphate reacts with iron (II) nitrate to produce a precipitate • Making potassium nitride from its component elements • Uranium (VI) fluoride reacts with magnesium metal Practice Problems: Write the decomposition for ammonium dichromate to produce nitrogen gas, water vapor and chromium (III) oxide. Hint: Dichromate = Cr2O72How many grams of ammonium dichromate would be needed to generate 400. grams of water from this decomposition? 2 10/16/2014 Practice Problems: 2 Mg + CO2 → 2 MgO + C If 30 g of Mg was mixed with 30 g of carbon dioxide, what is the maximum amount of magnesium oxide that could form? In other words, calculate the theoretical yield of MgO. FIRST: calculate the limiting reagent by finding the maximum amount of product (MgO) that could form IF each reactant was fully consumed. THEN: compare the amount of product that could form in each case. The reactant that produces less product is the limiting reagent & LIMITS the formation of product. Practice Problems: Write the balanced chemical equation describing copper (I) oxide reacting with carbon atoms to form copper metal and carbon dioxide. • How much copper metal could be produced from 100.0 grams of copper (I) oxide & 30. grams of carbon? Practice Problems: Urea (CH4N2O), a common fertilizer, can be synthesized by the reaction of ammonia (NH3) with carbon dioxide. 2 NH3(aq) + CO2(aq) CH4N2O(aq) + H2O(l) An industrial synthesis of urea begins with 35.8 kg of ammonia & 89 kg of carbon dioxide. What mass of urea could theoretically be produced from this starting mixture? 3