Gas Laws 1. Chemical analysis of a gaseous compound showed that it contained 33.0% Si and 67.0% F by mass. At 35.00 C, 0.210 L of the compound exerted a pressure of 1.70 atm. If the mass of 0.210 L of the compound was 2.38 g, calculate the molecular formula of the compound. Si 2 F 6 BLB text: p. 96 for empirical formula then calculate empirical weight PV = nRT solve for moles MW = mass/moles look at multiple 2. A chemist synthesized a greenish-yellow gaseous compound of chlorine and oxygen and finds that its density is 7.71 g/L at 36.00 C and 2.88 atm. Calculate the molar mass of the compounds and determine its molecular formula. ClO 2 PV = nRT = mol RT/MW solve for MW and substitute in 3. A mixture of gases contains 4.46 moles of neon, 0.74 argon and 2.15 moles of xenon. Calculate the partial pressure of the gases if the total pressure is 2.00 at a constant temperature. P(Ar) = 0.20 atm P(Xe) = 0.586 atm Χ(each component) = mol(component) / mol(total) P(each component) = Χ(each component) (Total pressure)
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This note was uploaded on 04/29/2008 for the course CHEM 122 taught by Professor Zellmer during the Winter '07 term at Ohio State.