Ok, so maybe I should have worded my question better.Anyway, I have 4 chemistry questions that I can't solve at allIf you can, please explain how it is solved along with the answer.1The aluminum foil on a certain roll has a total area of 18.5m2 and a mass of 1275gUsing a density of 2.7g per cubic centimeter for aluminum, determine the thickness in millimeters of the aluminum foil.2If a liquid has a density of 1.12g/cm3, how many liters of the liquid have a mass of 3.75kg?3A stack of 500 sheets of paper measuring 28cm by 21cm is 44.5mm high and has a mass of 2090gWhat is the density of the apter in grams per cubic centimeter?4When the ionic compound in NH4Cl dissolves in water, it breaks into one ammonium ion, NH4, and one chloride ion, ClIf you dissolve 10.7g of NH4Cl in water, how many moles of each ion would be in the solution?Thanks so much for your help!
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1Density 2.7 1,275 grams/ x cubic cmThus, 2.7x 1,275 x 472.22222 cubic centimeters The surface area of 18.5 square meters can be given by a rectangle that is 18.5 meters by 1 meterIn centimeters, this translates to an area of 1,850 cm x 100 cm 185,000 square centimetersThus, in order to get the volume, we must multiply the area of this rectangle by it's thicknessWe know both the volume necessary, 472.22222, and the area of 185,000 square cmSo 472.2222 cubic cm 185,000 square cm thickness cm Thickness cm 0.00255255 cm, or 0.0255 mm, a very thin piece of aluminum foil2Once again, we do a density equationBut we must convert kilograms into grams first by multiplying by a thousand1.12 grams per cubic cm 3,750 grams/x cubic cm 1.12x3,750 x 3,348.214286 cubic cmWe should know that 1 cubic centimeter is the same as 1 mL, so we need 3,348.214286 mL, or 3.348 L of this liquid3Converting the last dimension to centimeters, we get a volume of 28 cm 21 cm 4.45 cm 2616.6 cubic centimetersDensity is mass over volume, so the mass of 2090 grams/2616 cubic centimeters 0.799 gram per cubic centimeterHowever, if we wish to find the density of a piece of paper, we would have to divide both the volume and the mass by 500But, since we divide both parts of the density equation by the same value, the density does not change4Ammonium Chloride has the molar mass of 14.01+4(1.01)+35.5 53.55Thus, 10.7 grams amounts to 0.2 moleTherefore, since one formula unit of ammonium chloride dissociates into one unit of ammonium ions and one unit of chloride ions, we expect 0.2 mole of ammonium chloride to yield 0.2 mole ammonium ions and 0.2 moles of chloride ions, for a total of 0.4 moles of ions.
