10.gas laws key

10.gas laws key - Chem 105 Nielson Recitation 10/18/07...

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Unformatted text preview: Chem 105 Nielson Recitation 10/18/07 Boyle’s, Charles, Avogadro’s laws Ideal gas law Stoichiometry, MW, density calculations Gas laws 1. A 512 ml sample of gas, in a cylinder with a movable piston, at 0.000 °C is heated at a constant pressure of 0.800 atm to 41.0 °C. What is its final volume? Ans. 589 ml V; v 1 Vi. : 512M<§fl>2 ESQML ,f‘ / {— 7‘5 Z73r/‘5K ——-——— lL bf Mate: mime . _ - \ . 2,. , in) in Tr» LNW'fie/Q ~4=€NQ I. 1275.15K T. = BILL/5K Kjb‘fi 2. A 1.20 L sample of gas at 27.0 °C and 1.00 atm pressure is heated to 177 °C and 1.50 atm final pressure. What is its final volume? Ans.>1.2’0 L x I ’ 91/137186 v hL' RV. _ “PM V1 1 \/L' 21 (.1 . WLLW 450.1% —:=—- ' ~——— ~ T. mm 5... (c I L Tr P‘C ‘ I > . y z 2 20 L P T; = 500.1514 TL. =4lbOJ‘3K ‘( MMW , 3. A 0.50 mol sample of air is confined anOD’ C in a cylinder with a movable piston. The (Bl/390916 air has an initial pressure of 760.torr. The gas is then compressed by the piston so a‘( that its final volume is half the initial volume. The final pressure is 1.672 x 103 torr. 0W. What temperature is the air now? Ans. 27 °C WDLVL V 2V; ._ H ._. Tr : TL BXW), 273.51 witfigflfilw if) a .7" ’ ‘fivr Z L L T; (1);, Vt" 7W .4” T35005K= Zléi/x ‘ V “ ZV‘ ? - r . . Ideal gas edcuation L Z1 '€ 5 9606‘? )W K 4. Calcium carbonate decomposes upon heating to give the solid C210 and the gas C02. A sample of CaC03 decomposes and the C02 is collected in a 250 m1 flask. The pressure of the gas is 1.3 atm and the temperature is maintained at 31 °C. How many moles of C02 are produced? Ans. 0.013 mol C02 0303360 “:7 6906;) “L C0260) “Pvmm 7" 5‘ +275 0 2 = amen/14002, RT (0.0821L'm (504 k2 lame 5. What volume in liters does a 1.50 mol sample of H2 occupy at 55.0 °C and 1.00 atm ‘7 _. - pressure. Ans. 40.4 L T: Z 7 5‘ (6 + 5510 3 57/9. (.3 K @chRT‘ _ i _ V? MT : (150M) (0.082062%: (328‘ “3'9 ' P {,dbalh— \/= 40.4 L Variations with mass, Mm, and density 6. A 20.00 L vessel contains 0.200 g of 02 at a pressure of 0.0100 atm. What is the temperature of the gas? Ans. 390.K ?vvaT ., 71? (0.00 (025nm s (aoszotom) —»——-—— m: 0.200 02,. W = 0900225 NW 502 32.0:33 e 7. What weight of C02 is requir d to fll? a 10.0 ml flask to a pressure of 1.00 torr at 30 °C? What is the density of the C02? Ans. 2.33 x 10'5 g, 2.33 x 10'3 g/L 790/7 VHQT 17: I‘ww [Elm 11.3Hasélo‘gaflh‘ “Watt? _ 760m “,7 pwbalolA/(SK m ; LE! _; (Lamp x 10‘7’glw.)(o.OloL> 35'28‘3) )HO WCQS awe/“WW 0.055206% ,1} r “I; . 4mm”.li RT ( 7 W‘KXZZ 3,“) _2.33 no . C02 (1:03.111 m;%: (5.283) x .0“ s I « -5 WW6 col dag] 32.53X10 3 t .07) ‘l‘ow/ 8. One of the methods of estimating the temperature of the center of the sun is based 0 (0 low L) (\S OWWA the ideal gas law. If the center is assumed to consist of gases whose average —_ Z. 33 X ,0—3 \ molecular weight is 2.0 g/mol, the density is 1.4 g/cm3, and the pressure is 1.3 x 109 atm, what is the temperature? Ans. 2.3 x 107 K 1.5»:ch- H hm twat/A : Wm, ,, ([35 mo‘1 AMMzo'almer?) wM1. L MW 1 = 2.3 “’10le 9. A large flask is evacuated and found to weigh 134.567 g. It is filled to a pressure of 735 torr at 31.0 °C with a gas of unknown molar mass and then found to weigh 137.456 g. The flask is evacuated a second time and filled to the top with water. Its mass upon reweighing is 1067.9 g. What is the molar mass of the unknown gas? The density of water at 31.0 °C is 0.997 g/ml. Ans. 79.7 g/mol, Hint: First calculate the volume of the flask from the volume of water that filled it. Then solve for molecular . mass. 137.451.; fl : pv (o am;ch flaw.) a 0 03% W m C m ~5- 416 7 #6435 -: l N 0.0302/ml (Ky; lgz‘gzq QT (0.082002%(504J5K) “1077333511 WBSW ‘3'”? .03ch v= MB“ > W439" r W V 7 wow (imam 0.0197 WM “‘L ...
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This note was uploaded on 12/09/2009 for the course CHEM 105 taught by Professor Macedone during the Spring '07 term at BYU.

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10.gas laws key - Chem 105 Nielson Recitation 10/18/07...

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