a) Calculate the composition, in weight percent, of an alloy that contains 218.0 kg titanium, 14.6kg of aluminum, and 9.7 kg of vanadium.b) Aluminum-lithium alloys have been developed by the aircraft industry to reduce the weight andimprove the performance of its aircraft. A commercial aircraft skin material having a density of32.55 g/cm is desired. Compute the concentration of Li (in wt%) that is required.

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Answered: a) Calculate the composition, in weight…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 128SCQ

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A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.
21 ETRY AND REDOX REACTIONS If 20% by weight of nitrogen is present in a compound, the molecular weight of the compound may be (a) 144 (c) 100 (b) 28 d) 140 The mineral haematite is Fe2O3. Haematite ore contains unwanted material called gangue in addition to Fe2O3. If 5.0 kg of ore contains 2.78 kg of Fe, What is percentage purity of Fe;O;? A polystyrene, having formula B33C6H2(C&H3)n was prepared by heating styrene with tribromobenzoyl peroxide in the absence of air. If it was found to contain 10.46% bromine by weight, find the value of n. Hexachlorophene, C13H6C16O2, is a germicide in soaps. Calculate weight percent of each element in compound. Determine the empirical formula of Kelvar, used in making bullet proof vests, if it contains 70.6% C, 4.2% H, 11.8% N and 13,4% O: (a) CHSNO2 (c) CH9NO (b) CHSN20 (d) CHSNO In an organic compound of molar mass 108 gm mol C, H and N atoms are present in 9: 1 :3.5 by weight. Molecular formula can be: CaH&N2 7c) CsH&N 8. (b) CHoN (d) CaHN A…
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 5.600 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 23.23 % % Iron (from ion exchange & titration vs. NaOH) : 8.25 % From Part C: % Oxlate : 56.78 % Calculate the % water of hydration :
Qu The amount of calcium carbonate with MM:100.1 g/mol in the ore dolomite can be determined by gravimetry. The dolomite sample is dissolved in acid and the calcium ions (Ca2*) present are precipitated as calcium oxalate (CaC204) with MM: 128.1 g/mol. The calcium oxalate is filtered, dried and strongly heated to form calcium oxide (Cao) with Formula Mass (FM) = 56.1 g mol". In one analysis the mass of dolomite used was 3.72 %3D g. The mass of calcium oxide formed was found to be 1.24 g. Questions: 1. What is the chemical formula of the analyte in this problem? 2. What is precipitating agent? 3. Give the molecular formula of the precipitate measured in this problem. g. 4. What is the mass(g) of the analyte? Show your answer in correct no. of SF. 5. What is the % w/w of the analyte in the sample? Give the answer in correct answer of SF. 026.9 033.3 056 060.1 02.23
A mixture containing onlyl FeCl3 and AlCl3 weighs 5.95 g. The chlorides are converted to the hydrous oxides and ignited to Fe2O3 and Al2O3. The oxide mixture weighs 6.62 g. Calculate the % w/w Fe and % w/w Al in the original mixture.
The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The precipitate was filtered and ignited at 100° c to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the % Al in the sample. (number of moles Al = 2; Al2O3 = 1)
A 0.6599-g sample of impure magnesite, MgCO3 (MW = 84 g/mole), was decomposed with HCl; the liberated CO2 (MW = 44 g/mole) was collected on absorbent and found to weigh 0.1673-g. Calculate the percentage of magnesium (MW = 24 g/mole) in the sample. MgCO3 (s) + 2 HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O(l) Weight of pure magnesium in the sample is a. 0.1825 g b. 0.0913 g c. 0.3194 g d. 0.0456 g Percentage of magnesium carbonate in the sample is a. 24.20% b. 27.66% c. 48.40% d. 96.80%
A 0.2795-g sample of an organic mixture containing only C6H6Cl6 (290.83 g/mol) and C14H9Cl5 (354.49 g/mol) was burned in a stream of oxygen in a in a quartz tubeb. The products (CO2, H2O and HCl) were passed through a solution of NaHCO3. After acidification, the chloride in the solution yielded 0.7161 g of AgCl (143.32 g/mol). Calculate the percentage of each halogen compound in the sample. A mixture containing only FeCl3 (162.21) and AlCl3 (133.34) weighs 5.95 g. The chlorides areconverted to the hydrous oxides and ignited to Fe2O3 (159.69) and Al2O3 (101.96) The oxidesmixture weighs 2.62 g. Calculate the percent Fe (55.85) and Al (26.98) in the original mixture.
A 0.2795 g sample of an organic mixture containing only C,H,Clg (290.83 g/mol) and C14H9CI5 (354.49 g/mol) was burned in a stream of oxygen in a quartz tube. The products (CO2, H20 and HCI) were passed through a solution of NaHCO3. After acidification, the chloride in this solution yielded 0.7161 g of AGCI Calculate the % of each halogen compound in the sample.
0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)
A solution containing 0.40249 g of CoCl2. xH2O was exhaustively electrolyzed to deposit 0.09937 g of metallic cobalt on a platinum cathode. What is the number of moles of water per mole of cobalt in the reagent? FW CoCl2 = 129.84 g/mol H2O = 18.02 g/molAW Co = 58.93 g/mol
1. A 0.8040 g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated with 47.22 ml of 0.02242 M KMnO4 solution. Calculate the results of this analysis in terms of (a) %Fe (MW = 55.845) and (b) %Fe3O4 (MW = 231.535). Consider the reaction 5 Fe²+ + MnO4 + 8H+ → 5Fe3+ + Mn²+ + 4H₂O

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a) Calculate the composition, in weight percent, of an alloy that contains 218.0 kg titanium, 14.6 kg of aluminum, and 9.7 kg of vanadium.