21ETRY AND REDOX REACTIONSIf 20% by weight of nitrogen is present in a compound, themolecular weight of the compound may be(a) 144(c) 100(b) 28d) 140The mineral haematite is Fe2O3. Haematite ore containsunwanted material called gangue in addition to Fe2O3. If5.0 kg of ore contains 2.78 kg of Fe, What is percentagepurity of Fe;O;?A polystyrene, having formula B33C6H2(C&H3)n wasprepared by heating styrene with tribromobenzoyl peroxidein 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 makingbullet proof vests, if it contains 70.6% C, 4.2% H, 11.8% Nand 13,4% O:(a) CHSNO2(c) CH9NO(b) CHSN20(d) CHSNOIn an organic compound of molar mass 108 gm mol C, Hand N atoms are present in 9: 1 :3.5 by weight. Molecularformula can be:CaH&N27c) CsH&N8.(b) CHoN(d) CaHNA poisonous compound cadaverine has 58.77% C, 13.81%H, and 27.42% N. Its molar mass is 102 g/mol. Determineits molecular formula.The chloride of a metal contains 71% chlorine by weightand the vapour density of it is 50. The atomic weight of themetal will be10.

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Answered: If 20% by weight of nitrogen is present…

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 (d140

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter22: Inorganic Materials

Section: Chapter Questions

Problem 38AP

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World production of chromite (FeCr₂O₄), the main ore ofchromium, was 1.5107metric tons in 2003. To isolate chro-mium, a mixture of chromite and sodium carbonate is heated inair to form sodium chromate, iron(III) oxide, and carbon diox-ide. The sodium chromate is dissolved in water, and this solutionis acidified with sulfuric acid to produce the less soluble sodiumdichromate. The sodium dichromate is filtered out and reduced with carbon to produce chromium(III) oxide, sodium carbonate,and carbon monoxide. The chromium(III) oxide is then reduced to chromium with aluminum metal. (a) Write balanced equations for each step. (b) What mass of chromium (in kg) could be pre-pared from the 2003 world production of chromite?
Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32
Impure nickel, refined by smelting sulfide ores in a blast furnace, can be convertedinto metal from 99.90% to 99.99% purity by the Mond process. The primaryreaction involved in the Mond process is:Ni(s) + 4CO(g) ⇌ Ni(CO)4(g)In the second step of the Mond process, the gaseous Ni(CO)4 is isolated andheated to 227°C. The purpose of this step is to deposit as much nickel as possibleas pure solid (the reverse of the preceding reaction). Calculate the equilibriumconstant for the preceding reaction at 227°C.
The key reaction (unbalanced) in the manufacture of syn-thetic cryolite for aluminum electrolysis is HF(g)+ Al(OH)₃(s) +NaOH(aq) →Na₃AlF₆(aq) +H₂O(l) Assuming a 95.6% yield of dried, crystallized product, whatmass (in kg) of cryolite can be obtained from the reaction of 365 kg of Al(OH)₃, 1.20 m3of 50.0% by mass aqueous NaOH (d=1.53 g/mL), and 265 m³ of gaseous HF at 305 kPa and 91.5°C? (Assume that the ideal gas law holds.)
Write a complete and balanced redox equation for the synthesis of the coordinationcompound. Use iron(II) oxalate (the yellow/orange solid) as a reactant. In other words,complete the following reaction: FeC2O4(s) + H2O2(aq) + ??? → product(s) Assume that the net reaction occurs in an acidic solution: this will make balancing theequation easier. Use the formula of the iron (III) oxalate compound that you found in theliterature to balance the equation ([Fe(C2O4)3]). You must write out the individual half-reactions.
1a) Determine the formulae (show all calculations) represented by the following chemicalanalyses. All values are in weight percentages:i. SiO2 = 36.76, Al2O3 = 62.74ii. SiO2 = 38.0, Al2O3 = 21.5, FeO = 26.6, MgO = 6.3, MnO = 7.6iii. Try to name the minerals if possible. 1b) Please give a balanced reaction forThe dissolution ofi. Anorthiteii. Ca-smectiteiii. Kaoliniteiv. Plot all 3 reactions on a log[Ca/H] vs log[H4SiO4(aq)] graph.v. Add a progress line of stability if a small amount of anorthite is added to a largevolume of water and increasingly more solid is added compared to that volume(assume a closed system). Label key points of interest along that line. Give allreactions.
(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000g is treated with 0.6000g of pure H2C2O4•2H2O and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+→ Mn2++ 2CO2 + 2H2O), the excess oxalic acid requires 26.26ml of 0.1000N KMnO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?
Silver(ag) is obtained in much of the same manner as gold using NaCN solution and O2. Describe with appropriate equation the extraction of Ag from argentite Ag2S. The products are SO2 and Ag(CN)2 which are reduced with ZN?
Silver is obtained in much of the same manner as gold using NACN solution and O2. Describe with appropriate equation the extraction of Ag from Argentite Ag2S. The products are SO2 and Af(CN) -2 which are reduced with Zn
A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Write in a padpaper and show the clear and complete solution
A slag sample is known to contain all of its iron in the forms of FeO and Fe2O3. A sample of 1,000 g of the slag was dissolved in hydrochloric acid according to the usual method, then reduced with stannous chloride and finally titrated with a 0.02237 M solution of potassium permanganate, of which 28.59 mL were used. A second aliquot of the slag sample, weighing 1,500, was dissolved in a nitrogen atmosphere to further adjust the oxidation state of the iron, it was immediately titrated with the same potassium permanganate solution. If this second experiment required 15.60 mL of permanganate solution, calculate: a) The percentage of total iron in the slag. b) The percentages of the oxide FeO and Fe2O3
A solution of sodium thiosulfate, Na2S2O3 was standardized by dissolving 0.188 g of KIO3 (MM = 214.00) in water, adding a large excess of KI, and acidifying with HCl. The liberated iodine required 18.25 mL of the thiosulfate solution to decolorize the blue starch/iodine complex. Calculate the molarity of Na2S2O3 solution. Stoichiometry of the reaction is: 1 mol IO3- = 3 mol I2 = 6 mol S2O32-