Chem_3739Exam1Fall_2009

Chem_3739Exam1Fall_2009 - Youngstown State University...

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Youngstown State University Department of Chemistry Chemistry 3737(42725) October 2, 2009 First Exam - 100 pts. Name _______________________ Chap. 1-5, E&R, PChem. [15 pts/Que] ANSWER ANY 6 QUESTIONS – CIRCLE THEM Constants and Equations: PV = nRT [P + a(n 2 /V 2 )][V – nb] = nRT R = 0.08205 lit.atm.mol -1 K -1 R = 8.314 x 10 -2 bar dm 3 mol -1 K -1 ; dm 3 = lit] R = 8.314 J.mol -1 K -1 C V = (3/2)R (monat/ideal) 1 atm = 1.013 bar dw = -P ext dV (PV work) , dU = dq + dw , dU = C v dT, dH = C p dT dH = dU + d(PV) S vap = H vap /T b H = U + PV S mix = -nR{ x A ln x A + x B ln x B + ….} A = U – TS G = H - TS γ = C P /C V C P = C V + R (mol -1 ) (T 2 /T 1 ) = (V 2 /V 1 ) 1-γ (adiab.rev.0 dS = (dq rev /T) ∆S = dT ∆S = nRln(V 2 /V 1 ) + nC p ln(T 2 /T 1 ) (∂P/∂T) V (∂T/∂V) P (∂V/∂P) T = -1 Show your steps for full credit. *1. Use the ideal gas and van der Waals equations to calculate the pressure of 3.00 moles of H 2 if they are confined to a volume of 1.00 L at 298 K. [a = 0.2452 bar dm
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This note was uploaded on 07/15/2011 for the course CHEM 3321 taught by Professor Aa during the Fall '09 term at Dallas Colleges.

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Chem_3739Exam1Fall_2009 - Youngstown State University...

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