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Problems-Empirical formula

Problems-Empirical formula - to form water and another...

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1.Calculate the molar mass of a metal that forms an oxide having the empirical formula M 2 O 3 and contains 68.04% of the metal by mass. Identify the metal. 2) Hemoglobin is the oxygen carrying compound found in human blood. It is found to contain 0.3335% iron by mass. It is already known that one molecule of hemoglobin contains four atoms of iron. What is the molecular mass of hemoglobin? 3) For the reaction represented by the equation: CX 4 + 2 O 2 ---> CO 2 + 2 X 2 O 9.0 g of CX 4 completely reacts with 1.74 g of oxygen. What is the approximate molar mass of X? 4) A mixture of NaCl and NaBr weighing 1.234 g is heated with chlorine gas, which converts the mixture completely to NaCl. The total mass of NaCl is now 1.129 g. What are the mass percentages of NaCl and NaBr in the original sample? 5) A sample of an oxide of vanadium weighing 4.589 g was heated with hydrogen gas
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Unformatted text preview: to form water and another oxide of vanadium weighing 3.782 g. The second oxide was treated further with hydrogen until only 2.573 g of vanadium metal remained. (a) What are the simplest formulas of the two oxides? (b) What is the total mass of water formed in the successive reactions? 6) The term "alum" refers to a class of compounds of general formula MM*(SO 4 ) 2 . 12H 2 O, where M and M* are different metals. A 20.000-g sample of a certain alum is heated to drive off the water; the anhydrous residue weighs 11.123 g. Treatment of the residue with excess NaOH precipitates all the M* as M*(OH) 3 , which weighs 4.388 g. Calculate the molar mass of the alum and identity the two metals, M and M*. 7) 0.158 g of a barium halide is completely precipitated with H 2 SO 4 and 0.124 g of BaSO 4 is collected. What is the formula of the barium halide?...
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