1.1 A 47.3-mL sample of ethyl alcohol (ethanol) has a mass of 37.32 g. What is its density? 1.2 If 116 g of ethanol is needed for a chemical reaction, what volume of liquid would you use? The density of ethanol is 0.789 g/mL
1.3 Battery acid is 40.0% sulfuric acid, H2SO4, and 60.0% water by mass. Its density is 1.31. Calculate the mass of pure H2SO4 in 100.0 mL of battery acid.
1.4 How many moles of atoms does 136.9 g of iron metal contain? 1.5 A stack of 500 sheets of typing paper is 1.9 inches thick. Calculate the thickness, in inches and in miles, of a stack of typing paper that contains one mole (Avogadro’s number) of sheets (1 inch = 2.54 cm)
1.6 Compounds containing sulfur and oxygen are serious air pollutants; they represent the major cause of acid rain. Analysis of a sample of a pure compound reveals that it contains 50.1% sul- fur and 49.9% oxygen by mass. What is the simplest formula of the compound?
1.7 A 20.882-gram sample of an ionic compound is found to contain 6.072 grams of Na, 8.474 grams of S, and 6.336 grams of O. What is its simplest formula?
1.8 Hydrocarbons are organic compounds composed entirely of hydrogen and carbon. A 0.1647-gram sample of a pure hydrocarbon was burned in a C-H combustion train to produce 0.4931 gram of CO2 and 0.2691 gram of H2O. Determine the masses of C and H in the sample and the percentages of these elements in this hydrocarbon.
1.9 A 0.1014-g sample of purified glucose was burned in a C-H combustion train to produce 0.1486 g of CO and 0.0609 g of H2O. An elemental analysis showed that glucose contains only carbon, hydrogen, and oxygen. Determine the masses of C, H, and O in the sample and the percentages of these elements in glucose.
1.10 Phosphorus, P4, burns with excess oxygen to form tetraphosphorus decoxide, P4O10. In this reaction, what mass of P4 reacts with 1.50 moles of O2?
1.11 What mass of CO2 could be formed by the reaction of...