ASSORTED STOICHIOMETRY PRACTICE PROBLEMS PART I
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1 ASSORTED STOICHIOMETRY PRACTICE PROBLEMS PART I (1) A gram sample of a mixture of CaCO 3 and Na 2 SO 4 was analyzed by dissolving the sample and completely precipitating the Ca 2+ as CaC 2 O 4. The CaC 2 O 4 was dissolved in sulfuric acid and the resulting H 2 C 2 O 4 was titrated with a standard KMnO 4 solution. a. Write the balanced equation for the titration reaction, shown unbalanced below: MnO 4 + H 2 C 2 O 4 + H + Mn 2+ + CO 2 + H 2 O Also, indicate which substance is the oxidizing agent and which substance is the reducing agent. b. The titration of the H 2 C 2 O 4 obtained required milliliters of M MnO 4 solution. Calculate the number of moles of H 2 C 2 O 4 that reacted with the MnO 4. c. Calculate the number of moles of CaCO 3 in the original sample. d. Calculate the percentage by weight of CaCO 3 in the original sample.
2 (2) Water is added to grams of UF 6. The only products are grams of a solid containing only uranium, oxygen, and fluorine and gram of a gas. The gas is 95.0 percent fluorine, and the remainder is hydrogen. a. From these data, determine the empirical formula of the gas. b. What fraction of the fluorine of the original compound is in the solid and what fraction in the gas after the reaction? c. What is the formula of the solid product? d. Write a balanced equation for the reaction between UF 6 and H 2 O. Assume that the empirical formula of the gas is the true formula.
3 (3) Three volatile compounds X, Y, and Z each contain element Q. The percent by weight of element Q in each compound was determined. Some of the data obtained are given below. Compound Percent by Weight of Element Q Molecular Weight X 64.8%? Y 73.0% 104. Z 59.3% 64.0 a. The vapor density of compound X at 27 C and 750. mm Hg was determined to be 3.53 grams per liter. Calculate the molecular weight of compound X. b. Determine the mass of element Q contained in 1.00 mole of each of the three compounds. c. Calculate the most probable value of the atomic weight of element Q. d. Compound Z contains carbon, hydrogen, and element Q. When 1.00 gram of compound Z is oxidized and all of the carbon and hydrogen are converted to oxides, 1.37 grams of CO 2 and gram of water are produced. Determine the most probable molecular formula of compound Z. (4) A mixture of H 2 (g), O 2 (g), and 2 milliliters of H 2 O (l) is present in liter rigid container at 25 O C. The number of moles of H 2 and the number of moles of O 2 are equal. The total pressure is 1,146 millimeters of mercury. (The equilibrium vapor pressure of pure water is 24 millimeters mercury). The mixture is sparked, and H 2 and O 2 react until one reactant is completely consumed.
4 a. Identify the reactant remaining and calculate the number of moles of the reactant remaining. b. Calculate the total pressure in the container at the conclusion of the reaction if the final temperature is 90 O C. (The equilibrium vapor pressure of water at 90 O C is 526 millimeters mercury). c. Calculate the number of moles of water present as vapor in the container at 90 O C. (5) Propane, C 3 H 8, is a hydrocarbon that is commonly used as fuel for cooking. a. Write a balanced equation for the complete combustion of propane gas, which yields CO 2 (g) and H 2 O (l). b. Calculate the volume of air at 30 O C and 1.00 atmosphere that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O 2 by volume. c. The heat of combustion of propane is 2,220.1 kj/mol. Calculate the heat of formation, H O f, of propane given that H O f of H 2 O (l) = kj/mol and H O f of CO 2 (g) = kj/mol. d. Assuming that all of the heat evolved in burning 30.0 grams of propane is transferred to 8.00 kilograms of water (specific heat = 4.18 J/g K), calculate the increase in temperature of the water.
5 KEY: ASSORTED STOICHIOMETRY PRACTICE PROBLEMS I (1) a. 5 H 2 C 2 O MnO 4 b x 10 3 mol c x 10 3 mol d % + 6 H + 10 CO Mn H 2 O (2) a. HF b. 33 % of the original fluorine is in the solid 67 % of the original fluorine is in the gas c. UO 2 F 2 d. UF H 2 O UO 2 F HF (3) a g/mol b. one mole of X contains 57.1 grams of Q one mole of Y contains 75.9 grams of Q one mole of Z contains 38.0 grams of Q c. 19 g/mol d. C 2 H 2 Q 2 (4) a. O 2 is in excess, 7.54 x 10 3 mol O 2 remains b. 868 mm Hg c x 10 2 mol H 2 O
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Review Exam 2. 2.What is the mass of 4 atom(s) of copper in grams? A) g B) g C) g D) g E) 4.
Review Exam 2 1.Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate