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C112H S10 T1

# C112H S10 T1 - can sue ‘Ti nremetlglolng l A calorimeter...

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Unformatted text preview: can sue ‘Ti nremetlglolng l. A calorimeter is constructed of 600 grams of glass (c3 = 0.75 J/g C) and it contains 300 grams toluene (cs = 2.24 Jig C). The initial temperature of the calorimeter (both glass and toluene together) is 25.00000 C. If 60 J of heat is added to the calorimeter calculate the ﬁnal temperature of the calorimeter (both glass and toluene together) assuming no heat is losttothesurroundings. 25°C,” - , “(000 0.7. AT Mamba-2“ (00: L190 an Al" 0-1333 - (Boo) (2.2%)(0436'53s Q Q =8q.577b - 2 5. l 333) W m ‘°‘°§%‘Z'S%§\$°c E); e heat capacity of Uranium is 0.12? J/g C and the heat capacity of water is 4.184 Jig "f .s.300gran1Ucontrolrod311000C1stobecooledby:n g H 3’: u _ ofI-IZO tan ‘ ﬁnaltemperature of U and H20 combined. £1151 U 0%ng H20 C: 2 9 c, .y _ '"(faooxoazsﬁ-AVG —» (beacon s>cx-\00®_= 0 (500mm) M = Q a (500)(4.Is®(x - 25) “Q 5 AT= (somehow (04259193303: zoqQM want ”3 3. The enthalpy of formation of PC13 (l) is -319.1l kJ/mol and PC15 (s) is 443.5 kJ/mol. I The atomic mass of P is 31 g/mol and Cl is 35.5 g/mol. If0.2468 gramgClkis reacted ' according to PC13(1) + Clg(g) —) PC15 (s) how much heat will be evolved to the .WKO ROSiM surroundmg' s? PClz, + 02—9 PCP; 4: ””1435” 11k} , . 'BIQOIIJ Eb 031 3‘slmumts "(if hm" " 1-H 3. 5" . 2 1'” l X [061(3- (ism-.313??? astronazozq . - r0.0on 0.2%3 0.001106 /3 Awqgswquleof 7 m. S . 3M, sH-c I'LQ-C ‘ tiff—C 4. Chbane, C3113, has a structure with the eight C atoms at the comers of a cube and one H atom on each C atom. Given the enthalpy of the reaction shown below is -820 . [mol and that the C-H bond is 343 kJ/mol and the co bond is 413 kJ/mol calculate . bondstrength: . it] p __ gr. @5055 —> 1\ c-ac —> a ﬁn: 8 H—C = 3% ”l D2 (m) t 80433] ‘Qfﬂsq‘a? + x] [Hq5b t- 219% - 21%‘4-‘4‘! = ‘820 71H®“+.2"IBH”H‘X =‘ ”820 qu‘flbﬁ-HX‘ 87.0 ——e ”D” X= NHL} . 5. Fuel dragsters bum nitromethane according to the eqn. below: i W‘ I“—‘—"r—’—. ““I 2CH3N02 (1) + 3%» 2 c02(g) +3 H20(g)+M) : ‘Hl‘KEé. O 0 not Ifthe enthalpy of the above reaction is -l418 kJ/mol and the enthalpy of forniation of C02 (g) is 693.5 kJ/mol and H20 (3) is -241.8 kJ/mol calculate the standard enthalpy of formation of CH3N02. M0] ﬂats-gr 2(—3qa5)+ 362413) *5}- .. ":81 + ”125% ' 2x '- “\5\2.H-2«X‘-H‘% -—2:tt=th.‘-i }- .151 x 1-H mm ‘5'77 (0 6. In the space below write a balanced chemical equation which, if you could measure it, would give you directly the enthalpy of formation of sucrose: C12H120n (solid). :26", 6H2 +—;'OZ —). CIZHIZO“ "5-1." W?”‘*‘ .... . . .. .r . . . . .. . . _ ... .. . .__ III-“WM," .‘,_:... _,_, . - .= |-' W 7. Given the enthalpies of the ﬁrst four reactions, calculate the enthalpy the ﬁﬁh: — 4020 kJ/mol -- <3 OI-l O- - 620 kJ/mol " I"), Ll O - 240 kJ/mol h' L‘ (a — 2300 kJ/mol 2. 5 (p 00 ????? kJ/mol H 31 2% L3H CLC' H ‘L 3H7.” 302594;“129!) 8. One form of selenium, Sea, is a closed ring of eight selenium atom-gm eight Se-Se single bonds. Given the bond dissociation enthalpies: O=O 495 kamol and Se—Se 145 kJ/mol and that the Se=__Q_ bond strength' 1;; 320 kJ/mol calculate the enthalpy of the reaction shown below: Sex + 4 O=O -—-—) BSe=O AI-I°= ???? kJ/mol 9. For the following events, indicate whether the reaction should be endothermic (endo), exothermic (exo), or nearly thennoneutral (neut). Think about them carefully and Circle only one answer for each. a. Hg (gas) -—-> Hg (liq) . endo 11th b. I-Ig2(gas) +2 Hg(gas) 3 cm Icndo' neat endo neut d. Cl-Hg-Cl(g) + I-Hg—I(g) —> 2 Cl- -Hg-I(g) . endo ‘ Erdo" pus-9 b'm'tbomls EKG-3 neg-3 mm bond-\$- c. Hg(liq) —> Hg (solid) 3. Which of the following is the correct unit for measuring pressure ? (circle one answer only) ' N—M3 N.M2 - NJQ @ N-M" . N—M's b. Which of the following is the correct unit for measuring work ? N F .5 ‘D (circle one answer on 'u c. First law of thermodynamics. E. hers” re mains constan t “m Jdue, universe ~~ "‘5 - e H8 (1 closed system‘) ‘ property or ﬁmctiton. 6. Silicon and carbon are in the same row and both C02 and SiO; are stable compounds. Why are the properties of these two Compounds so different. Explain brieﬂy and sketch the two ...
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