chem notes 10-15

chem notes 10-15 - -individual gas types do not interact...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
October 15, 2007 Dr. Stevens Gen. Chem. 1 Test Wednesday -review Tues. night -given on test: R values -chapter 4, 12, 5 Applications of Gas Equations/Relationships -ex: Calculate density of N2 at 20C and 1atm -d = m/v = g/L => moles/vol = n/v -n/v = P/RT =>1/293(0.08206) x 28/1 = 28/293(0.08206) = 1.2g/L -ex: Calculate MM of an unknown gas for which 2.0g is placed in 1.0L at STP. -MM = g/mol = mass/n -MM = 2.0g/n -n = PV/RT = 1(1)/0.08206(273) = 0.045mol -2.0/0.045 = 45g/mol Stoichiometry and Gas Relations -ex: If 2.0g CaCO3 is reacted with excess HCl according to: CaCO3 + 2HCl CaCl2 + H2O + CO2, calculate p if 50.0mL of a test tube is used at 23C. -V = .05000L -P of CO2 -P = nRT/V -2.0g/100 = .020mol -P = .020(0.08206)(296)/.050 = 9.7atm Dalton’s Law of Partial Pressures: -PV = nRT -Partial Pressure: P of an individual gas component in a mixture -Total P of a mixture = sum of individual PP b/c each gas exerts P as if it is alone in the flask -idealized assumption
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: -individual gas types do not interact with each other = very idealized-in the same flask-P and n are variables in Dalton’s Law-PV = nRT-P/n = RT/V = C- P1/n1 = C, P2/n2 = C-P1/n1 = P2/n2-ex: The total P of 1.0mol NO 1.5mol H2O = 8.0atm. Calc. PP of NO and H2O-P(no)/n(no) = P(h2o)/n(h2o) = P/n-P(no)/1 = P(h2o)/1.5 = 8.0atm-P(h2o)/1.5 = 8.0/2.5 = 4.8atm-Pno = 8.0 – 4.8 = 3.2atm Real Gases:-when P and V are NOT ideal-if P and V are not ideal, we cannot correctly use PV = nRT-most ideal P is low, V is large-no interaction-intermediate situation attractive forces (imf) as molecules approach at intermediate P and V-molecules cluster together (if n decreases, P drops as well)-Pideal = P an^2/v^2-large a for large imf-H2O v. He a(h2o)>a(he)-extreme situation P is high, v is small-NOT ideal-Videal = (V(real)-nb(#mole)) b = measure of size-Ideal: PV = nRT-Real: (P + an^2/v^2)(V-nb) = nRT...
View Full Document

This note was uploaded on 04/23/2008 for the course CH 151 taught by Professor Stevens during the Fall '08 term at Whitworth University.

Page1 / 2

chem notes 10-15 - -individual gas types do not interact...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online