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Unformatted text preview: Exam 11 Name
Introductory Chemistry 030.101 (Print) Last Name ' First Name Section I — Professor GJ. Meyer
November 3, 2003 SOC. Sec. # (optional) SHOW ALL WORK FOR FULL/PARTIAL CREDIT
GIVE FINAL ANSWERS ON THE LINE WHEN INDICATED Chapter 4: P = pg11(1) PV = C (2) V = Vn(1+ t/273.15) (3) T = 273.15 + t (4) PV =11RT (5) (P Vl)/11IT‘[— ” (P3V3)/112T2 (6) PM: 11“,I(RT/V) (7) PA = XAPmt (8) PV = l/3NmL_tl (9) 1/3Numg3 = RT (10) L_! — 3RT/M (1 1)
f(u) = 41t(m/27t1q,'1")15 113 exp(—mul/2ka) (12) Z = 'A (N/VMA (13) (l‘ateA/rateB) = NA/NB(Mg/MA)I II} (14) Chapter 7: w = PmAV (1) q = McSAT (2) AB = q + w (3) AEm‘i‘. = A13Sys + AEsurr = 0 (4) q. = 11chT (5)
qp =11cpAT (6) H = E + PV (7) c\. = 3/2 R (8) cp = CV + R (9) AE =11cVAT (10) AH = ncpAT (11)
AH = AE + A (PV) 2 AE + A (nRT) = 0 (12) (T.vl)"“ = (TZVZY'I (13) PMY = PlvzY Chapter 8: S = k., 111 Q (1) AS = qm/T (8) AS =11R111(V3/V,) (9) AS: AHmslT, (10) ASmp= 88 + 5 .l mol‘I K'I (11)
AS=11cV 111(T2/T1) (12) AS ~11c, 111(T2/T1) (13) ASSWT= AHS(S WISH” (14) S"=1(cII,/T)dT + ASP.laSL (15) Standaids and Unit Conversions. For H O: elm“; — 75 J mol I‘IK cm— 38 l n1ol'I KI ,AHms— H 6.007 kJ molI AHWP= 170 kJ mol I
R— 0.0821 LatmmolI KI=8.314J11101I KI 101J=Latn1 g=9.81111/s 11=1kgn12 s '
Avagadlo’ s Nun1be1= No: 6.022 x 10“ 1 cal= 4 184 J 1 Pa— — 1 kg mI 52 1. (15) Answer the following assuming ideal gas behavior:
a; The gas inside a balloon at a temperature of 20.0 C is heated until the volume of the balloon is
doubled. The pressure remains constant at 1.00 atm. What is the new temperature of the gas? T;— 26 ,’3 K V1 ’ »
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b. A balloon whosekolume 1s 5.0 L contains 6 1 g of N2 gas. What mass of H2 gas must be added to the
balloon to expand its volume to 1 1 L at the same temperature and p1 essure" (6'1 mfg: _, 21,11,691:
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c. A bulb is ﬁlled with C02(g) at a pressure of 0.86 atm and a temperature of 298 K. A quantity of C210 is \ff introduced into the bulb. After some time, the pressure of COz(g) is found to drop to 0.39 atm because
w it is consumed by the process: CaOm + COM, 9 CaCOW. What is the mass of calcium carbonate formed? You may assume that the solid materials do not significantly change the total volume. maw 0535/; O}(’+J;.. (Lt)L WM;
(Va 111 H" a h 7.. (6. “(7)1.0173'L9/6otlt £43? [M 1‘) (Mr/C)
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Section I  Professor Meyer NM. WW. . . . e .a 0 L— 2. (10) A liquid sample of NC13 was introduced into a container thaLeL/isiaéfs—argor s at a pressure of
1.00 atm. The temperature was maintained at 29 GC. The NC13 was exposed to light and decomposes
completely to fonn N2(g) and C12(g). If the ﬁnal pressure was measured to be 1.88 atm., what was the initial amount of NC13 in the c011tainer? g margin/”7 Hues ”“740 A
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=00W“”——»——n—eee~—~w .3 Among; were We. (is) 0.02? Mew/L My .QS‘I'MWe ed Cesar? r5395 3. a) The volume of an ideal gas coritracts from 8.4 L to 4.2 L as the result 0 an applied pre su
atm. The system evolves 830 J of heat during this contraction. Find A13 for this change in state. W: "iDewﬂAV (35:73,“; __: J
e.— ‘08’Jze3 (Ln 1.44%) UOH’LE) ' ; $50 New ‘2 (Bi{DJ AE "WEJ b) Calculate the heat necessary to raise the temperature of 1.0 kg of water from 298 K to 308 K.
Calculate the heat required to bring about the same temperature change in the same mass of mercury
given that em = 0.14 .1 K“ g“ , ' 1mm VJ 03/17?)
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.3 K XL ) R i Y K: Q(H20)_l7l‘gﬂ—__ , q<Hg> .ﬁﬁL 4. (20) For each section of the following problem, mark the indicated quantities as + (increase). —
(decrease; or 0 (no change) for the system underlined in each part. a. A warm piece of pizza is placed in a refrigerator and comes to equilibrium. q "' AB "' b. write and OZ react to form CO; inside a rigid, sealed, insulated container. wﬁ AE__1:_ c. A bowl ofc_re_a_m is whipped with an egg beater. _ w; AT_"i:_ d. An ideal gas expands isothermally into a vacuum. w___(_2~ q _0_
"56' Sodium chloride melts. AT_D_ AS "1‘ Introductory Chemistry 030.101 Name
Section I ~ Professor Meyer 5. (10) Suppose an ice cube weighing 36 0 g at a tempelatuie of 10 C is placed in 359 g ofwatei at a
tempeiattue of 20 C. Calculate the final temperature assuming no heat loss to the surroundings. in H") 9" “do” Q ”*0 [0”) 12.31443 + 2.00% (W931 1“)”le ”KQODM)
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91; . n Mme«Mi (reel/Maw , (R19 51’ is. ’i 1’ ”w 6. (10) The measured enthalpy change for burning ketene (CHgCO) is AH; = 981.1 k] at 25 C.
CH20<g1+ 2 02<g19 H201g1+ 2 €020.21 (1)
The enthalpy change for burning methane (CH4) is AH; = —802.3 kJ at 25 C. CH4<g1+ 7 02m 9 2 1420th COzrg) (2) Compute the enthalpy change for the following reaction at 25 C: 2 CH4(g) + 2 om, > 3 1120“.) + CHgO(g) (3) ' A113 ”G52 3.. 5’ K T All; a (514,)" AH.2 [505’019‘*(" Will] KT 7. (25) Suppose 1.000 mol ofthe ideal gas argon is conﬁned in a strong rigid container of volume 22.41
L at 273.15 K. The system is heated until 3000 .1 of heat is added. The molar heat capacity of the gas
is 12.47 Jmol"1K". (a) Calculate the initial pressu1e inside the container [00 #7:»
P wr MW ‘— " v "' ZZHI Z. . (b) Determine q for the system during the heating process. 3 000 I
t3, c + 3000 5 (c) Determine w for the system during the heating process. 0 [ii/:57 11> W: 0 .
((1) Compute the temperature of the gas after heating. ' T; : 5—] 3; 71 K ... O ’ J _. .
T513351: .1: 4.20am... ~9906K
1: t r1 1:V (1.00M) U?” 1‘ ME) ’ .
(e) Compute AE of the gas during the heating process. . . ”1' 330003
A t: "= 27%)
(1) Compute AH of the gas during the heating process. £2 000 1
ﬁztﬁSMM AH Ag ‘2 ACN) , A5 + VAP+ EXZ/
RT 0/ J
: i‘_a~'5(>1)o.1 + [623$]le (1.3?! landmﬂl ] V
= 510001 ...
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 Fall '08
 Draper
 Chemistry

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