0.2 0.0 500 1000 1500 2000 2500 Molecular velocity (m/s) v b) Briefly explain wh

Question

0.2 0.0 500 1000 1500 2000 2500 Molecular velocity (m/s) v b) Briefly explain why? Tho ucfage op moteculor)s highera lo S0oX 2. A piece of dry ice (solid CO2) with a mass of 22.1 grams sublimes (changes phase from solid to gas) into a large balloon. Assuming that all of the CO2 goes into the balloon, what is the volume of the balloon at 30 °C and a pressure of 10.99 psi? 16,L 3. A gas mixture contains each of the following gases at the indicated partial pressures: H2, 135 torr, He, 100 torr and Ar at 368 torr. (a) What is the total pressure of the mixture? 603 form (b) What mass of each gas is present in a 1.75 L sample of this mixture at 100 c? h-2 4, Calculate the ratio of effusion rates for He and Ar .llg Ar 030 o20u9 5. Which assumption of kinetic molecular theory breaks down under conditions of low

Explanation / Answer

Q3

Ptotal = P1+P2+P3

Ptotal = 135 + 100 +368

Ptotla = 603 torr

b)

mass of each gas, given

Apply Ideal Gas Law,

PV = nRT

where

P = absolute pressure

V = total volume of gas

n = moles of gas

T = absolute Temperature

R = ideal gas constant

n = PV/(RT) = (P)(1.75)/(62.4*373)

n = 0.0000751*P

for mass

n gas = 0.0000751*Pgas*MWgas

choose H2

n gas = 0.0000751*135*2 = 0.0203 g of H2

choose He

n gas = 0.0000751*100*4 = 0.03 g of He

choose Ar

n gas = 0.0000751*368*368 = 10.170 g of Ar

Q4.

rate of effusion

Rate He / Rate Ar = sqrt(MW Ar/ MW of He)

Ratio = sqrt(40/4) = 3.16

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