10.K-M theory key

10.K-M theory key - Chem 105 Nielson Recitation Partial...

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Unformatted text preview: Chem 105 Nielson Recitation 10/23/07 Partial pressure Kinetic-Molecular Theory 1. A 1.00 g sample of air consists of 0.76 g of nitrogen and 0.24 g of oxygen. Calculate the partial pressures and the total pressure when this sample occupies a 1.00 L vessel at 20 °C. Ans. P(Nz) = 0.65 atm, P(Oz) = 0.18 atm, P 1= 0.83 atm , m a 0 ,oo‘? 5 mre O; (\N z 0.70 mol _O,O’2,'valNZ no : madam! L 0 J p y 05 at»; 95,"! PM "'L‘o-Z/m_”‘?_,___.mf_kk—ZBSQ_OCO 'ogwe I - _. (Po 2 (09075MX0‘08wbmu, ml 1 2— 1.001, P: 0.05%... _ ‘ aim @aP «PD 2. A 3.0 L bulb, containing He at 145 mmHg, is connected by a valve to a 2.0 L bulb M” containing, Ar at 355 mmHg. If the valve is opened so that the two bulbs are ?T ‘ O $331k connected, what is the partial pressure of each gas after mixing? What is the total pressure of the gas mixture? Assmne the temperature remains constant. Ans. P(He) = 87 mmHg, P(Ar) = 140 mmHg, Pm] = 230 mmHg mt] V;=5.0L ‘ \1;=6.01, @Vazmn stpa "PL “trawl-.le “p; a 7 E» ESMQS Pf .7 . 3 Q{{{}— _, [45% (3.0 L "P 355% 23‘: :0de (PF LL!) 5°"): 87 MALE) (‘7G 7, P +§C$fiiaa 3. A flask contains CH4(g), C02(g), and H20(l) at 34.0 0C and a total pI‘Xe-ssure 311344 atm. The volume of the flask not occupied by the water is 2.311 L. The mass of C02(g) in the flask is 2.252 g. a. Detemine the mole fraction of C02(g). Ans. 0.4152 , 2.25 wt Cb; = .Oem was . 0.053,]7WV‘Q co “a 4W ‘9 " Xx, L n1“ EM l 3 a3 23“: = (“7,53 3 Ovhg‘awdc? , 3 %1 b. Deter%Tne the pcairtiD zp‘rté’ssur :fcthe C02(g). Ans. 0.5580 atm KW: L c. Detzermine the average kinetic energy of the molecules in the flask. Ans. 6.361 x 10' J 4. In an experiment to generate nitrogen gas, 352 mL of N2 is collected over Water at a temperature of 24.0 °C. The total pressure of the experiment is 742 mm Hg. What mass of N2 is produced? The water vapor pressure at 24.0 °C is 22.4 mm Hg. Ans. 0.383 g N2 5. You have 2 flasks filled with the same mass, one with N2 and one with Ar gas. The flasks have the same volume and temperature. They are each sealed with a rubber stopper. Answer T or F for each of the following questions and briefly explain why. a. There are more molecules of N2 than Ar atoms. Ans. T, N2 has a smaller Mw than Ar (28 g/mol vs. 40 g/mol), so if the two containers have the same mass there must be more moles or molecules of N2. b. PA, > PN2 Ans. F, P is proportional to n and there are more moles of N2 gas. The average velocity of Ar = average velocity of N2. Ans. F, the average KE is the same for Ar and N2. Since KE = V2 mvz, and the mass of a N2 molecule is less than that of an Ar atom, then the v of N2 must be greater than the v of Ar. d. N2 molecules collide more frequently with the flask walls than Ar atoms do. Ans. T, PN2 > PAr and P = F/A where F is force of the collision. .0 6. Explain the properties of the gases below using the Kinetic-Molecular Theory of gases. Assume all other properties remain constant in each situation, except the two properties that are being related to each other. riment E lanation from theo P is the force of gas molecules colliding with the walls of the container. The frequency of the collisions and the average force of the collisions increase with tem erature. If the force of the collisions increases with T, then the area of the collisions must also increase, so as to reduce the number of collisions in order for P to remain constant. P = F orce/Area the number of molecules increases. with smaller area. Macrosco ic behavior from ex - P increases as T increases. V increases as T increases. ...
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10.K-M theory key - Chem 105 Nielson Recitation Partial...

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