Wh yield of a chemical reaction? 8. How is the percent yield of a reaction calculated? reti via the online homework management program, Wiley PLUS www.wileyplu 2. Calculate the number of moles in these quantities: (a) 2.10 kg NaHCO3 (b) 525 mg ZnCl2 (c) 9.8 × 1024 molecules CO2 (d) 250 mL ethyl alcohol, C2H3OH (d = 0.789 g/mL) 4. Calculate the number of grams in these quantities: (a) 0.00844 mol NiSO4 (b) 0.0600 mol HC2H,O2 (c) 0.725 mol Bi2S3 (d) 4.50 x 1021 molecules glucose, CH1206 (e) 75 mL K2CrO4 solution (d-_ 1.175 g/mL, 20.0% K2CrO4 by mass) or 6. Which contains the larger numbers of molecules, 25.0 g HCl 85.0 g C,H1206? Show evidence for your answer. 8. Balance the equation for the combustion of butanol and set up the mole ratio of (a) O2 to C4HOH(d) C4HoOH to CO2 (b) H20 to 02 (c) CO2 to H20 (e) H20 to C4H,OH (f) CO2 to 02 10. Given the unbalanced equation

Wh yield of a chemical reaction? 8. How is the percent yield of a reaction calculated? reti via the online homework management program, Wiley PLUS www.wileyplu 2. Calculate the number of moles in these quantities: (a) 2.10 kg NaHCO3 (b) 525 mg ZnCl2 (c) 9.8 × 1024 molecules CO2 (d) 250 mL ethyl alcohol, C2H3OH (d = 0.789 g/mL) 4. Calculate the number of grams in these quantities: (a) 0.00844 mol NiSO4 (b) 0.0600 mol HC2H,O2 (c) 0.725 mol Bi2S3 (d) 4.50 x 1021 molecules glucose, CH1206 (e) 75 mL K2CrO4 solution (d-_ 1.175 g/mL, 20.0% K2CrO4 by mass) or 6. Which contains the larger numbers of molecules, 25.0 g HCl 85.0 g C,H1206? Show evidence for your answer. 8. Balance the equation for the combustion of butanol and set up the mole ratio of (a) O2 to C4HOH(d) C4HoOH to CO2 (b) H20 to 02 (c) CO2 to H20 (e) H20 to C4H,OH (f) CO2 to 02 10. Given the unbalanced equation

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 178CP: You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen),...

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4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
What is the molarity of each ion present in aqueous solutions of the following compounds prepared by dissolving 28.0 g of each compound in water to make 785 mL of solution? (a) potassium oxide (b) sodium hydrogen carbonate (c) scandium(III) iodite (d) magnesium phosphate
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
4.12 In petroleum refining, hydrocarbons are often manipulated by reacting them with H2(g). If hexene, C6H12, is reacted with hydrogen to form hexane, C6H14, how many moles of hydrogen are needed to react with 453 moles of hexene?
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
4-93 Ammonia is prepared industrially by the reaction of nitrogen and hydrogen according to the following equation: If 29.7 kg of N2 is added to 3.31 kg of H2, (a) Which reactant is the limiting reagent? (b) How many grams of the other reactant are left over? (c) How many grams of NH3 are formed if the reaction goes to completion?
The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO2. Determine its empirical and molecular formulas.
For the following reactions, write the ratios that can be established among molar amounts of the various compounds. 2H2+O22H2O 2H2O22H2O+O2 P4+5O2P4O10 2KClO32KCl+3O2 xs
You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
4.68 The pictures below show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (Green balls represent B atoms and orange balls are A atoms). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.