Question

Consider a mixture of 2.00 g of helium and 10.0 g of xenon atoms in a container with a volume of 1 L. Assume that helium and xenon are ideal gases. (a) If the root mean square speed (v_rms or u_rms in Chapter 9) of helium is 1500 m/s, what is the temperature of the gas? (b) Assuming that the helium and xenon are at the same temperature, what is the root mean squared speed of the xenon gas? (c) How many moles of helium and xenon are in the container? (d) Compute the partial pressures of helium and xenon in the container? (e) What is the total pressure of the gas on the walls of the container?

Answer 1

SOL": Helium Gillen mixture of Helium = 2.00g of 10g of Xenon atoms yolume = 12 molar mass of Xenon = 131 g/mol molar mass of Helium = 491 mol moles of Helium = mass - 22:0.5 mole. Molar mass . 4 moles of Xenon = mass. . = 10 mole molar murs 131 la I root mean square speed of helium = 1500ml Vrums = /BRT MO where Moin kg. 1500 = 3X 8.314XT X1000 V 4 1500 X 1500 = 348.314 XTxim - 4 T= 360.84 K T T-341K | Temperature of the gas = 361k 1b Assuming and Argon have same that the helium Temp.

Vaims He = MAS Vrons Ar Mue PAGE NO: DATE: a las 150 = 110 (Vrms) Ar a Vams) Ar= 1500 10 10 = 150510 = 474 mis pressure of the gas - Plotal - + Protai x V = nRT Protai X 1 = 10.5 +10 ) X0-0821 X 361 a total = 0.576X0.08217361 = 17.07 atm partial pressure of Helium = moles of Helium & Protal Total moel 0.5 g 17.07 atm 0.576 - 14.81 atm partial pressure of Argon = (17.07- 14.51) atm the z 2.26 47m
Please like this answer. THANK YOU

Please comment if you have any doubts about this answer.

All the best for your future.