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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...
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