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Ch_6-3_Other

# Ch_6-3_Other - THE VAN DER WAALS EQUATION THE VAN DER WAALS...

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DALTON’S LAW OF PARTIAL PRESSURES ( A B A B tot A B n n RT n RT n RT P P P V V V + = + = + =

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A mole fraction = A A A A C A B A B C A B C V P n P P P P n n RT V V V RT RT P P P RT n χ = = = + + + + +

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EXAMPLE 6.12 P. 228: A sample of KClO 3 is heated and decomposes to produce O 2 gas. The gas is collected by water displacement at 26°C. The total volume of the collected gas is 229 mL at 754 torr pressure (atmospheric pressure). How many moles of O 2 form? P tot = P H20 + P O2 754 = 25 + P O2 P O2 = 754 - 25 = 729 torr 2 729 1 0.959 1 760 O torr atm P x atm torr = = ( ( ( 29 2 0.959 0.229 0.00895 0.0821 299 O atm L PV n mol L atm RT K mol K = = =
THE VAN DER WAALS EQUATION Nitrogen gas

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( 29 2 2 an P V nb nRT V + - = Excluded volume Attractive forces between molecules
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Unformatted text preview: THE VAN DER WAALS EQUATION THE VAN DER WAALS EQUATION Example. What is the pressure of N 2 gas, if V = 3.50 L, n = 85.0 moles, and T = 293 K? ( 29 ( 29 820. 0.18 2045 P + = 2045/ 0.18 820 10,500 11,000 P atm =-= → Using PV =nRT, P = 7,120 atm (huge error). ( 29 2 2 1.39 85 3.50 85 0.0391 85 0.0821 293 3.5 x P x x x +-= 3.32 Excluded V makes P larger Attractive forces make P smaller Excluded volume more important ( 29 2 2 an P V nb nRT V +-= 2 sig. fig....
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