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- You are told by your instructor to go to the stock room and find a bottle of the chemical K3Cl. Does such a compund exist?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) Br 4. Name the compounds below or give it's structure (the missing one!) (a) Barium phosphate (d) Fe(NO;)3 (b) iodine heptafluoride (e) (c) ethyl 2-ethoxyethan-1-oate 5. An organic compound is made up of 67.7% carbon, 11.1% hydrogen and 22.2% oxygen. Circle the compounds that will give this elemental analysis. (D)
- Ores with as little as 0.25% by mass of copper are used assources of the metal. (a) How many kilograms of such an ore would be needed for another Statue of Liberty, which contains 2.0X10⁵ lb of copper? (b) If the mineral in the ore is chalcopy-rite (FeCuS₂), what is the mass % of chalcopyrite in the ore?The price of (a) CoCl2•6H2O is $25.00 per 100 g and (b) NH,CI was $11.35 per 500 g. Calculate the costs of each of these reagents used in this preparation. If cost were a determining factor which of these would be used as a limiting reagent? (a)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%
- b To make NaTcO4, the metal is dissolved in nitric acid 7 HNO3 (aq) + Tc(s) → HTCO4(aq) + 7 NO2 (g) + 3 H20(2) and the product, HTCO4, is treated with NaOH to make NaTcO4. Write a balanced equation for the reaction of HTCO4 with NaOH. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.)In the mineral beryl, six silicate tetrahedra are connectedto form a ring as shown here. The negative charge of thispolyanion is balanced by Be2 + and Al3 + cations. If elemental analysis gives a Be:Si ratio of 1:2 and an Al:Si ratio of 1:3 whatis the empirical formula of beryl: (a) Be2Al3Si6O19,(b) Be3Al2 (SiO4)6, (c) Be3Al2Si6O18, (d) BeAl2Si6O15?A 8.12 kg mixed-mineral sample contains chromite (FeCr2O4) as the only chromium-bearing ore. The sample is subjected to an industrial process, using a ferrosilicon alloy as a reducing agent, which quantitatively converts all of the chromium into 12.9 kg of a ferrochrome alloy (stainless steel) which is 19.3% Cr by mass. What is the percentage of chromite (FeCr2O4) in the original sample?
- Consider the series of reactions to synthesize the alum (KAl(SO4 )2 · xH2O(s)) from the introduction. (a) Assuming an excess of the other reagents, from one mole of aluminum Al (s), how many moles of alum will be produced? (b) Assuming an excess of the other reagents, from one mole of potassium hydroxide KOH, how many moles of alum will be produced? (c) Assuming an excess of the other reagents, from one mole of sulfuric acid H2SO4 , how many moles of alum will be produced? (d) If you start the synthesis with 1.00 g of Al, 40.0 mL of 1.50 M KOH, and 20.0 mL of 9.00 M H2SO4 , which of the three will be the limiting reagent? (e) Assuming that the product is anhydrous (that there are no waters of hydration), calculate the theoretical yield of alum, in grams, based on the amounts of reagents in part (d). 3. Consider the nickel salt: (NH4 )2Ni(SO4 )2 ·y H2O (Ammonium Nickel Sulfate Hydrate), where y is the number of coordinated waters. (a) Assuming that the product is anhydrous (y = 0),…Kaolinite clays are produced from the weathering of igneous rocks of which feldspar is a good example: K2O. Al2O3.6SiO2 + CO2 + H2O = K2CO3 + Al2O3.2SiO2.2H2O + SiO2 How many tonnes of kaolinite clay are derived from a tonne of feldspar?Use the following atomic masses (in g/mol): Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 1.) Calculate the MgO content of 12.35g Magnesia Magma, which has been dissolved in 50mL of 1.0340N H2SO4 and required 24.6mL of 1.1255N NaOH in the back titration.