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CHEM 111 (69)
Lecture

Standard conditions, gas constant (R), gas law and density, gas mixtures, mole fraction (X)

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Department
Chemistry
Course
CHEM 111
Professor
Dana Johnson
Semester
Fall

Description
3 November Announcements Practice exam tonight Here, A103 7 – 9 pm Mid-semester grade check Please check to make sure all your grades are posted Let me know if something is missing Standard conditions Once P, V, T and n were all related, a constant was needed Standard states had to be specified: P = 1 atm T = 273.15 K (or 0° C) n = 1 mole V = 22.4 L STP conditions – standard temperature and pressure 1 mole in 1 liter How is this possible? Same # of particles But different weights → different average speeds Gas constant, R Determination of R: (1 atm x 22.4141 L) / (1 mol x 273.15 K) 0.08205 Note units of (atm x L) / (mol x K) How R is used to relate the equation: PV = nRT ideal gas law R = P V / n T initial 1 1 1 1 R = P V2/2n T 2 2 final P 1 1 n T1=1P V / n2T2 2 2 Example A rigid plastic container holds 35.0 g of ethylene gas at a pressure of 793 torr. What is the pressure if 5.0 g of ethylene is removed at constant temperature? P / n = P / n 1 1 2 2 793 torr / 35 g = P / 32 g P 2 P n1/ 2 1 P 2 793 (30) / 35 P = 680 torr
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