Aniline, a starting material for urethane plastic foams, consists of C, H, and N. Combustion of such compounds yields CO2, H2O, and N2 as products. If the combustion of 9.71 g of aniline yields 6.63 g H20 and 1.46 g N2, what is its empirical formula? If the molar mass of aniline is 93 g/mol, what is its molecular formula?

Aniline, a starting material for urethane plastic foams, consists of C, H, and N. Combustion of such compounds yields CO2, H2O, and N2 as products. If the combustion of 9.71 g of aniline yields 6.63 g H20 and 1.46 g N2, what is its empirical formula? If the molar mass of aniline is 93 g/mol, what is its molecular formula?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Antimony is alloyed with lead to increase the rigidity of components used in the construction of lead storage batteries.1.304 g of a particular metallic alloy, compounded of only Pb and Sb, can be quantitatively converted into a 1.511-g mixture of the oxides PbO2 and Sb2O4.What was the percentage (by mass) of antimony in the alloy?
Disulfur dichloride, which has a revolting smell, can be prepared by directly combining Se and Cl₂, but it can also be made by this reaction: 3 SC1₂ (1) + 4 NaF (s) → SF4 (g) + S₂ Cl₂ (l) + 4 NaCl(s) Calculate the mass of SC12 needed to react with excess NaF to prepare 1.37 g S₂ Cl2 if the expected yield is 46%. Mass of SC12 = g
Consider the following chemical reaction: CaO(s) + H2O(l) ----------> Ca(OH)2 (aq) if 1.00 g calcium oxide is mixed with 2.00 g water, calculate grams of the product. CaO = 56.08 g/mole, H2O = 18.02 g/mole, Ca(OH)2 = 74.10 g/ mole
While working in the lab, you find a bottle of white powder labeled "astringent". Since the original investigator neglected to record the identity of the substance, you decide to perform a combustion analysis to identify the compound. You have a 76.8 g sample that when burned produces 139 g CO2 and 24.4 g H2O. What is the empirical formula of this compound? (The compound consists of only C, H, and O.)
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H,O that can be produced by combining 81.4 g of each reactant? 4 NH, (g) + 50,(g) 4 NO(g) + 6 H, O(g) > g H,O mass:
Hydrogen sulfide is a toxic waste product of some industrial processes. It can be recognized by its distinctive rotten egg smell. One method for eliminating hydrogen sulfide is by reaction with dissolved oxygen, as shown below. If 102.24 grams of H2S (GFM = 34.08 g/mol) are combined with 64.0 grams of O2 (GFM = 32.00 g/mol), what is the theoretical yield (in grams) of elemental sulfur that could be produced by the reaction? Show all work and report your answer to the correct units and significant figures.
An organic compound contains Carbon, Hydrogen, and Oxygen. The percentages of H is 6.73%, 39.99% C and 53.28 g of O by mass. What is the empirical formula of the compound? HTML Editore BIUA A I E E = 3 E X 田, Vx D VD¶ T
Hydrogen sulfide is a toxic waste product of some industrial processes. It can be recognized by its distinctive rotten egg smell. One method for eliminating hydrogen sulfide is by reaction with dissolved oxygen, as shown below. If 102.24 grams of H2S (GFM = 34.08 g/mol) are combined with 64.0 grams of O2 (GFM = 32.00 g/mol), what is the theoretical yield (in grams) of elemental sulfur that could be produced by the reaction? Show all work and report your answer to the correct units and significant figures.
A student performed a similar experiment to the one you performed: They took a crucible and lid, cleaned them, heated them over a flame, and after cooling found their combined mass to be 22.538 g. The student then added a sample of zinc(II) sulfate hydrate (ZnSO4·“n”H2O) to the crucible so the combined mass of the sample, crucible, and lid was 25.896 g. They heated this sample for 10 minutes with the lid ajar, let it cool, and measured the mass of the crucible, sample, and lid to be 25.054 g. a. Based on this experiment, what is the formula for they hydrated zinc(II) sulfate compound? b. The student later looked on the reagent bottle for zinc(II) sulfate hydrate and found the actual formula was ZnSO4·7H2O. If everything had been done correctly, what value should the student have expected for the final mass of their sample, crucible, and lid after heating?
The thermite reaction, once used for welding railroad rails, is often used for an exciting chemistry demonstration because it produces red-hot molten iron. The reaction is: Fe2O3(s) + 2Al(s) → 2Fe(I) + Al2O3(s)If you start with 50.0 g of iron(III) oxide and 25.0 g of aluminum, what is the limiting reagent? What is the maximum mass of aluminum oxide that could be produced? How much aluminum oxide would be produced if the yield is 93%?
Benzoquinone, a chemical used in the dye industry and in photography, is an organic compound containing only C, H, and O. What is the empirical formula of the compound if 0.183 g of the compound gives 0.447 g of CO2 and 0.0610 g of H₂O when burned completely in oxygen? (Enter the elements in the order: C, H, O.) Empirical formula:
Benzopyrene is a hydrocarbon that is known to cause cancer. Combustion analysis (see Problem 4.92) of a 2.44-g sample of this compound shows that combustion produces 8.54 g of CO2 and 1.045 g of H2O. What is the empirical formula of benzopyrene?