Exam 3 - CHM 1220/1225 Exam III B 1. List the...

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Unformatted text preview: CHM 1220/1225 Exam III B 1. List the intermolecular forces in order of decreasing strength. Describe when each occurs .w. . K. . it : n. "’77:": .“J‘lrw .,- H -‘ I" C, r ning of the variable “b” in the van der Waals equation. Relate your explanation to the Kinetic Molecular Theory. 2. Explain the physical mea r e: '5’" manages) must} , a {I to, .— m m 4 (.,{’(_,i s—J ‘7“ ' ,J‘Ah .v“ ‘V u; 7“ ” s ,4“ -w' "' . . s. , ,2" I": sky/xi . 3-. What makes a molecular solute soluble in benzene,C6H6? ' . l, -. , - {egg/a. £3C=="‘G “1’41 5‘9") ,- y 4. Refer to the phase diagrams on the information page. ' 2.. Compare the phase diagram of water to that of carbon dioxide. Why does the line between solid and liquid slant in different directions? C, y i { wttsfi 9.: ‘13, ea." '05 100%; f NP (r A {:72 ' i . AV? - ‘! =5 7 , ,‘v .,. A ->x1/. ' .W‘xii‘x A”, LN’LEFL C»; Fir? ’- C oJlWl—f‘? PFEEfZUi-i “EU-(“*7 22 in: mm!) MTV/e23? *2) I {—0 Bring; ' ’ b. Refer to the phase diagram for sulfur. Explain. the'transitions that will occur yvhen sulfur is C. Q I.‘ . ,. _. r ,_ "' ‘T’TJ—‘i’ "f 1?; V3.3 (f‘fi ‘4‘: l w 2" / - .I‘, if; ’ i‘ “I, :6“ w ‘5 a ((2; Kitty; . V. [Lg-gr); :l CHM 1220/1225 Exam Ill B 3 5. Ethanol burns in air according to the balanced equation below. What volume of oxygen at 350°C and 790.0 mmHg needed to burn 227 g ethanol (CZHSOH, MW 46.07 g/mol). CZHSOHU) + 3 02(3) ——> 2 C02(g) + 3 H200) 6. A 6.62 g sample of a compound is dissolved in 25.0 g water. The boiling point is elevated by 158°C What is the molar mass of the substance? :7, E,“ IN :5 '- " ’ 5 f” x fl ,r r \. -‘ is: » itifiab‘g WMWHQ CHM 1220/1225 Exam III B 4 LCHQOSE EITHER PART a OR b. Circle the part you choose. Put an “X” on the part you omit. ‘ 7. ,r a. l“) Arrange the following molecules, H28, F2, and CH30H, in order of increasing strength of - ‘ xx" intermolecular forces. Which has the highest vapor pressure? ’ . . A sample of Xeszvith a volume of 6.00 L at 700. rman and 35°C is heated until the volume is ‘ 4.12 L and the pressure 1s 1200. mmHg. What-is the final temperature (in °C)? ' LA CHOOSE EITHER PART 3 UK b. Circle the part you choose. Put an “X” on the part you omit. 8. 3&4: Calculate the rms speed of SO2 at 25°C. (Molar mass: _64.06 g/mol) CHM 1220/1225 Exam III B 5 LCHOOSE EITHER PART a 0R b. Circle the part you choose. Put an “X” on the part you omit. 93:; Selenium difluoride, SeFZ, is a colorless liquid. It has a vapor pressure of 757 mmHg at 105°C and 522 niran at 95°C. What is the heat of vaporization of selenium difluoride in kJ/mol? )hj Calculate the number of grams of ice that will melt, if 1000.0 g of iron at 500°C is dropped into ‘ an ice water mixture. The heat of fusion of water is 335 J/g. Specific heat for iron = 0.448 J/g °C . Assume that there is enough ice such that some is left after thermal equilibrium is achieved at 0°C. 1.! \ a7; 1 l“ .4 CHOOSE EITHER PART 3 OR b. Circle the iaart you choose. Put an “X” on the part you omit. 10 a. ’3 The vapor pressure of pure diethyl ether, (C2H5)ZO, is 316 mmHg at 258°C. What is the vapor" pressure lowering if 17.8 g of a nonvolatile solute (molar mass 78.0 g/mol) is added to 250. g of diethyl ether (molar mass 74.12 g/rnol)? .1 \. _.« ,>’%‘ i An aqueous solution is 2.00 M urea, CO(NH2)2. The density of the solution is 1.029 g/mL. What \15 the molal concentration of urea in the solution? (molar mass urea 60.06 g/mol; water 18.02 g/mol) the»: Firs” 1.x “’7 x e la. t J U - < .6;va ~ .. ' {.L,»*'”' 11“ 7\\/'l\j ...
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This note was uploaded on 07/12/2008 for the course CHM 1220 taught by Professor Barber during the Spring '07 term at Wayne State University.

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Exam 3 - CHM 1220/1225 Exam III B 1. List the...

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