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Chapter 11 Notes Material Type: Notes; Professor: Fawzy; Class: General College Chemistry; Subject: CHE Chemistry; University: Murray State University; Term: Spring 2010;
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(P atm = h) mmHg
A Flask Equipped with a Closed-Tube Manometer P gas = (h) mmHg
P V P V or Animation: Microscopic illustration of Boyle’s law See Figure and Animation: Boyle’s Law) Go to 13
f f i i
( 4. 0 atm ) ( 1. 0 atm) ( 1. 8 L ) P P V V f i i f V 0. 45 L
abs
(See Animation: Charles’s Law) (See Video: Liquid Nitrogen and Balloons) Go to 17
f f f i i i T P V T P V using
f i i i f f
Vf 5. 7 L
V V n m V n
m
For one mole of a gas at STP (P = 1atm, T=273K)
Using the Ideal Gas Law n PV RT mol m n M 15 7 32 5 32 5 . . . (atm) 50.0 (L) 0.082 (atm. L. mol. K ) 294 (K) (mol) 32.0 (g. mol ) m = 1.04 10 g O -1 -
3 2
PV nRT atm L mol 0.082 K = C + 273 Animations for ideal gas law