Handout0926 - What volume of air(1.00 atm 27° C 20.0...

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Lecture outline for Wednesday, September 26, 2007 (Chem 100, section 2) Applications of Ideal Gas Law Calculating density of gas Calculating molar mass from gas density Using in stoichiometric calculations Using alternative units for R Example Problem) Calculate the formula of the oxide formed if 10.0 g of chromium metal reacts with 6.98 L of pure O 2 at 20.° C and 99.4 kPa Dalton’s Law of Partial Pressures P total = Σ P X = P 1 + P 2 + . ... + P n P 1 = n 1 RT/V; P 2 = n 2 RT/V; P total = n total RT/V Gas Mixtures (mole fractions (%)_ A stoichiometry problem with partial pressure
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Unformatted text preview: What volume of air (1.00 atm, 27° C, 20.0% oxygen) is required to burn 1.00 L of ethanol (d = 0.789 g/L, M = 46.0 g/mol)? Collecting Gases over Water P gas of interest = P total- P H2O 1. O 2 is collected by bubbling through water. If T = 21° C and 250. mL is collected at P = 0.987 atm, how many moles of O 2 were produced? 2. If decomposed 0.833 g of KClO 3 , what was the percent yield of O 2 ? Online homework will be available by 5 pm; due 9 am. Friday....
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This note was uploaded on 04/07/2008 for the course CHEM 100 taught by Professor Scarrow during the Fall '07 term at Haverford.

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