Chapter 14 Notes

# Chapter 14 Notes - = 22.4 L/mol Calculate the molar volume of 1.00 mol of H_2 gas at 273 K and 760 torr V = RT =22.4 L n P Standard temperature and

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(Skip sections 14.6 and 14.7) I. Avogadro's Law A. Avogadro's Hypothesis Equal volumes of gases under the same conditions of T and P contain the same number of molecules. B. Avogadro's Law At a constant temperature and pressure, the volume of a gas varies directly as the number of molecules present. II. The Ideal Gas Equation 3. Molar Volume a. Def- The volume in liters of one mole of a gas. Molar Volume = V = RT n P molar mass = g/mol molar volume = L/mol b. Differences between molar mass and molar volume: Molar Mass: Each substance has a unique value; independent of T & P

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example: Calculate the molar volume of 1.00 mol of CO_2 gas at 273K and 760 torr. V = RT n P = (62.4 Lxtorr ) (273 k) mol x K (760 torr)

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Unformatted text preview: = 22.4 L/mol Calculate the molar volume of 1.00 mol of H_2 gas at 273 K and 760 torr: V = RT =22.4 L n P Standard temperature and pressure (STP) 0 C or 273 K ˚ 760 torr or 1 atm III. Gas Stoichiometry A. Mass- Volume or Volume-Mass Problems Given mass------> Want Volume 1) Standard Stoichiometry to solve for moles of gas 2) Use the moles of gas and PV= nRT B. Volume-Mass Problems Given volume of a gas---------> Want g of ? 1) Use volume and PV=nRT to solve for moles of gas 2) Standard stoichiometry using moles of gas. C. Volume-Volume Problems Given Volume----> Want Volume (All reactants and products are gases) (All gases are at the same Temperature and Pressure) 1) The coefficients in the equation are in the same ratio as the volumes of the gases....
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## This note was uploaded on 04/08/2009 for the course CHM 109 taught by Professor Staff during the Fall '08 term at Grand Valley State University.

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Chapter 14 Notes - = 22.4 L/mol Calculate the molar volume of 1.00 mol of H_2 gas at 273 K and 760 torr V = RT =22.4 L n P Standard temperature and

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