Question

Exercise 6.4 • How many moles of gas will occupy a 750 ml volume at 25°C and 0.42 atm pressure? . 2 If the argon gas in a light bulb exerts a pressure of 0.54 atm at 20°C. what pressure will it exert at 160°C? 3 What is the molar mass of a gas if 0.21 g occupies a 0.13 liter volume at 80°C and 0.92 atm pressure? - How many grams of ammonia gas, NH,, are there in a 600 ml volume at 1260 torr and -13°C? 5. What is the density of methane gas. CH. at 120°C and a pressure of 0.93 atm?

Answer 1

6 By using Ideal gas equation pv=nRT 750 p= Pressure = 0.42 atm: v=volume = 750mL = 1 Tood = 0.750L n= moles, R = Gees constant = 0.0820 L atmkt mol T = Temperatur = 2500 = 25+ 293 = 298k 0.42 atm x 0.750 L = nx0.0820 L-atmf. moi x 2984 0.315 L.atm = nx 24.436 L.atm. mot! 0.315 Katon in = - 0.0128 more 24.436. yatch moll moles y gas = 0.0128 mole) Accesdiry Gay-Lussaes on, Pi - 2 P= Initial pressure = 0.5 atm P2 = final pressure = To be calculate Is Initial temperature = 20°C 220 +273 = 293k 2 = final temp = 1600 = 1604 273= 433k

0.54 am P2 433K 293K atm 0.001843 atm 0.00184 3 – P2 = 433K 433K !!P2 = 0.001843 atm x 43316 P2 = 0. 798 atm lipussure = 0.798 atm) 3 volume = 0.13 L. Temp = 80+273 = 353k mass pressure = 0.92 atm n= mw m MW . pv= nRT 0.21 g r0.0820 l-atm x 353k 0.92 atm x 0113L =- MW mollc 0.1196L. atm = 6.078 mw MW 6.078 - = 50.82 Hm 0:1196 m Molar man = 50.8

6 v = 600 mL = 600/1000 = 0.600 L p - 1260 tors = 1260x0.001315 atm = 1.658th T= -13°C = -13 + 273 = 2001 na w - 17 am pv = nRT 1.65 atm x 0.600L = m 2 179 xo.0820 Leatm. x 260k more 0.99 L.atm = mx 21.32 L.atm/mot 175m = mx1.284 Liam.pl m= 0.99 L atm 1125h 4 asm.gr = 0.789 g (.man of ammonis a 0.789 g )