20071008 Day Lecture 14

20071008 Day Lecture 14 - Welcome to CHM 1220/1225 Its time...

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Welcome to CHM 1220/1225 It’s time to start……. Thank you! Dr. Zibuck Pre-lecture Assignment 14 will be available at 2:00 p.m. today and is due by noon, Wednesday, October 10, 2007. Chapter 5 Quiz is due by noon, Friday, October 12, 2007. Chapter 5 Homework is due by 12:50 p.m. Friday, October 12, 2007
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? You put varying amounts of gas into a given container at a given temperature. Use the ideal gas law to show that the amount (moles) of gas is proportional to pressure at constant temperature and volume. t tan cons is RT V where RT V P n nRT PV = = ? A 50.0-L cylinder of nitrogen, N 2 , has a pressure of 17.1 atm at 23°C. What is the mass of nitrogen in the cylinder? V = 50.0 L P = 17.1 atm T = 23°C = 296 K RT PV n = ) K ( K mol atm L . ) L . )( atm . ( n 296 08206 0 0 50 1 17 = mass = 986 g (3 significant figures) mol g . mol . mass 01 28 20 35 =
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Gas Density and Molar Mass Using the ideal gas law it is possible to calculate the moles in one liter at a given temperature and pressure. That can then be converted to gram (per liter). To find molar mass, find the moles of gas, then find the ratio of mass to moles. In equation form that is P drT M or RT PM d m m = = ? What is the density of methane gas (natural gas), CH 4 , at 125°C and 3.50 atm? M m = 16.04 g/mol P = 3.50 atm T = 125°C = 398 K RT P M d m = ) K ( K mol atm L . ) atm . )( mol g . ( d 398 08206 0 50 3 04 16 = ) figures t significan ( L g . d 3 72 1 =
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? A 500.0-mL flask containing a sample of octane, a component of gasoline, is placed in a boiling water bath in Denver, where the atmospheric pressure is 634 mmHg and water boils at 95.0°C. The mass of the vapor
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This note was uploaded on 02/02/2010 for the course CHM 1220 taught by Professor Barber during the Spring '07 term at Wayne State University.

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20071008 Day Lecture 14 - Welcome to CHM 1220/1225 Its time...

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