ch440_2009_ex1a

ch440_2009_ex1a - 1 bar Chemistry 440 Hour exam .........

Info iconThis preview shows pages 1–6. Sign up to view the full content.

View Full Document Right Arrow Icon
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
Background image of page 3

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

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

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

View Full DocumentRight Arrow Icon
Background image of page 6
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 1 bar Chemistry 440 Hour exam ...... ......... .. Department of Chemistry, Oregon State University 21 October 2009 2 8 J/(K - mol) 2 0.08 L ~ atm/(K - mol) 105 Pa 2 1 atm I2 (be + we n = qby — / Peacth U+PV (2% (3—91)]: (gist l i Q V 3T 132%,); 1+5v+ pRT __3_V vaPT )P CPI-‘71 —1 = TZf/gy—l $2 + $3 + . . . 1+sz+133p2+~~ for an adiabatic process; 7 = p: 2 V 0p Cu 1. Provide the equation(s) and define terms. (a) (4 pts) State the First Law of Thermodynamics as it applies to the universe and to a system (twoequations). AUUNV 1‘- AUW: +AUSvrr‘ :- 0 WW enmm O’F-H‘VL vmmse ts (ions-eNtol A074; :: 3.5g 4—Wm TKLC/‘angl In inferML emy ' Of- +M ws—km as Mam of~ M Walesde 4— wovka MW ms. (b) (2 pts) Define an adiabatic process in terms of the thermodynamic variables of the system (one equation). 9&4; = O (c) (4 pts) Define the conditions for the critical point of a single component fluid (two equations). (gar-zggrzo N @T;<%9T:O 2. (10 pts) The internal energy per mole U of a model fluid is given by WAT) = CRT - cm (1) Derive (5—)U if 0., and a are constants. dU:®O\T—O\O\P=O CST) : 0L Wu 5"; 3. (10 pts) The van der Waals equation, without allowance for attractive forces, is given by ‘ nRT . V — nb For C52, by: 0.040 L / mole, and its molecular weight is roughly 80 g/ mole. P: (2) a) If the mass density of liquid carbon disulfide is 1.2 g/mL, what is its molar density in moles / L? mg “000111: x mow: I200 =\5‘mdu/L m. L- 80g 759’ b) What is the lowest molar density (moles / L) at which Eq(2) fails? Vnnbzo, L: I :1S‘nmUL b 034on2: .— .— (L v 4. (10 pts) A Joule—Thomson coefficient has a value, an 2 —1.25 mK/bar. Does the temperature increase or decrease and by how much when the pressure drop is 1 kbar? Mn :— 61?)” =(~l.2§&§)€103bax) bar ’— .— AT‘ +1.26 K T In creases 5. Consider a. fluid whose equation of state obeys P ='pRT(1+ bp) - £192; p = n/V where a and b are constant. Derive: (a) (12 pts) BAT), Bg(T), the second and third virial coefficients, respectively; n a. 2'; P/PRT: 1+b9—0LP/RTr—1432P'r83? 1‘" 8320 (b) (6 pts) and the dependence of dU(T, V) on V, note av: _ 8P _ (Wt—487%” (3—1,? = PRch?) so V‘ - @973 PRT(1+bP)"‘{PRTU+Lp-) 4192} r;qu 9. ,_ 2. ' om: OLP dv —or(g_)-ow 6. (12 pts) One mole of argon (assumed to be an ideal gas) is compressed reversibly from 6 L to 1 L at 300 K. Calculate AU,won and qby. First, consider an ISOTHERMAL process and second, an ADIABATIC process. — (m)... (a) isothermal O ’2... H' .- 9. .4 CV AT CV AT . 1 (L) dU'r—O nag—{Pow '=— at“ -—- RT dV/v .3 e ~Ww= RTlh(VZ/v.)—_ RTflh"'ihe] '= "KT Wan :1 RT: 8L-3’OOKza'4-hy (b) adiabatic $4 E. _ yr D’ékCJL—l': 5J2;— T» ’ V2 CV C" 2’3 943 T2 __ e __ T‘ " 'r) TZ’IR C 7. (10 pts) Prove that 8P CUP: KT V 0( :— l V — 8V cychc W12. 8. (10 pts) Determine if dqby is an exact (differential for an ideal gas which undergoes a reversible process. _dU=-CV fiT =4er ~P0W ' iw: CvdT +Pdv I “W gs“):— @a=%(%1>= % 0 ,~ draw is m+ exact 9. (10 pts) dU(S, V) is an exact differential, where S is the entropy and T is the absolute temperature. If ' dU(S, V) = TdS — PdV (6) then by the condition of exactness . . . 0V 5 ‘65 V ...
View Full Document

Page1 / 6

ch440_2009_ex1a - 1 bar Chemistry 440 Hour exam .........

This preview shows document pages 1 - 6. Sign up to view the full document.

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