! ( ans with explanation) 2. What is the empirical formula for each of the following compounds?a. N2O4b. H2SO4c. C,H63. In the procedure for this lab, you have to add water to the crucible after the Mg reacts.Why?

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Answered: What is the empirical formula for each…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 144QRT

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A student had a sample of CaCl2 • nH2O. He heated the sample until the mass did not change. From this data, calculate (a). the percentage of CaCl2 in the original sample and (b). the formula of the hydrate Mass of crucible + cover = 28.39 gMass of crucible + cover + sample = 30.41 gMass of crucible + cover + residue = 29.75
For each of the compounds below, indicate the oxidation state of each element in the compound. Be sure to show your work or briefly explain your process. MgCl2 (Mg = ? / Cl = ?) P4O10 (P = ? / O = ?) CuNO3 (Cu = ? / N = ? / O = ?)
Reacting water with magnesium nitride produces ammonia (NH3) and magnesium hydroxide. If this process is 70% efficient, what mass of ammonia (in kg) can be prepared from 19.5 kg of magnesium nitride?
How many grams of solid Ca3(PO4)2 can be formed from a reaction of 51.8 mL of 0.754 M CaCl2 and 21.5 mL of 1.04 M Na3PO4? Why can't 4.04 g of solid Ca3(PO4)2 be formed under these conditions? This amount is (greater than, less than, or equal to) the theoretical yield.
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1 .Pure molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron(III) oxide and coke (pure elemental carbon). If 1.58 kg of pure iron(III) oxide is used, how many kilograms of iron metal can be produced?
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A 1.500 g sample of iron ore, labeled A, was processed accordingly to give 0.5215 g of pure Fe2O3 (159.69 g/mol). A second sample of iron ore, labeled B, weighed 1.750 g and gave 0.5097 g of pure Fe2O3. What is the % Fe (55.85 g/mol) in Ore A?
A 1.500 g sample of iron ore, labeled A, was processed accordingly to give 0.5215 g of pure Fe2O3 (159.69 g/mol). A second sample of iron ore, labeled B, weighed 1.750 g and gave 0.5097 g of pure Fe2O3. What is the %Fe3O4 (231.54 g/mol) in Ore A?
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An ore is analyzed for manganese content gt converting the manganese to Mn3O4 and weighing it. If a 1.52 g sample yields Mn3O4 weighing 0.126 g, what would be the Mn2O3% in th sample? Mn% in the sample?

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What is the empirical formula for each of the following compounds? a. N,O4 b. H2SO4 C. C6H6