0.42139 17. G 5 19g. mass of Unknown sulfate. macs Of Empty Crucible & cover 18.33449 mass of Crucible & barium dulfate 0.GB269 mass of Barlyun dulfate. suFate %% w/W
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- Aleks data for AgBrO3 is 5.38 x 10^-5A mixture containing only Al2O3 (FM 101.96) and Fe2O3 (FM 159.69) weighs 2.019 g. When heated under a stream of H2, the Al2O3 is unchanged, but the Fe2O3is converted to metallic Fe plus H2O(g). If the residue weighs 1.774 g, what is the weight percent of Al2O3 in the original mixture?The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)
- Souring of wine occurs when ethanol is converted to acetic acid by oxygen: C2H5OH(l) +O2(g)--->CH3COOH(g)+H2O(l). A 1.00 L bottle of wine labeled as 7.00% (%v/v) ethanol, is found to have a defective seal. Analysis of 1.00 mL showed that there were 0.0274 g acetic acid in that 1.00 mL. The density of ethanol is 0.816 g/mL. (a) What mass of oxygen must leaked into the bottle in pounds(lb) (b) What is the percent yield for the conversion of ethanol to acetic acid, if oxygen is in excessBe sure to answer all parts. Fluorite, a mineral of calcium, is a compound of the metal with fluorine. Analysis shows that a 36.77−g sample of fluorite contains 17.87 g of fluorine. Calculate the following: (a) Mass of calcium in the sample. _________g Ca (b) Mass fractions of calcium and fluorine in fluorite. Calculate to 3 significant figures. mass fraction Ca mass fraction F (c) Mass percents of calcium and fluorine in fluorite. Calculate to 3 significant figures. mass % Ca mass % FIn the synthesis of benzoic acid, 3.5 mL of toluene were used and mixed with potassium permanganate solution. In making the potassium permanganate solution, 7 grams of the powder were dissolved in 150 mL of water. The resulting crystals were purified and the yield 1.53 grams. Identify the limiting reagent and compute for the number of moles that it consumed. What is the theoretical yield? What is the percentage yield? MW toluene = 94.14, density=0.87 g/mL , MW KMnO4 = 158, density = 2.7 g/mL , MW Benzoic acid = 122, density = 1.27 g/mL
- 5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?Suppose you reacted 0.500 g of Mg powder mixed with several acid-inactive substances and obtained 246 ml of hydrogen gas under S.T.P. conditions.What percentage by weight of the model is magnesium?General formula of a polymer is-(CH2CHCHCN)n-, where n is typically greater than 10,000. Then take a sample of this polymer weighs 755.9 g and contains 3.112 x 1020 molecules of -(CH2CHCHCN)n-, so calculate n?
- What is the concentration of a 62.0 % (w/w) concentrated nitric acid (HNO3, Mr = 63.0 g/mol) solution (density: 1.32 g/cm3) in mol/dm3 (molarity) and g/dm3 (mass concentraion) units? How many cm3 do you need to dilute into 200.0 cm3 from that concentrated nitric acid if you would like to have a solution with a concentration of 3.0 mol/dm3 ?A mixture of Al2O3(s) and CuO(s) weighing 18.371 mg was heated under H2(g) at 1 0008C to give 17.462 mg of Al2O3(s) 1 Cu(s). The other product is H2O(g). Find wt% Al2O3 in the original mixture.Would you help me whit this example (6) Thank you.