1. Consider the following velocity distributions for the SAME gas at two differe
ID: 547102 • Letter: 1
Question
1. Consider the following velocity distributions for the SAME gas at two different temperatures. Which temperature is HIGHER? 1.0 (a) Temperature A (b) Temperature B8 8 08 04 02 0.0 0 500 1000 1500 2000 2500 Molecular velocitymS (b) Briefly explain why? 2. A piece of dry ice (solid CO.) with a mass of 22.1 grams sublimes (changes phase from solid to gas) into a large balloon. Assuming that all of the CO, goes into the balloon, what is the volume of the balloon at 30°C and a pressure of 10.99 psi? 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? (b) What mass of each gas is present in a 1.75 L sample of this mixture at 100°C?Explanation / Answer
1)
a) Tempreture B
b) because
root mean square speed = (3RT/M)1/2
where, R = ideal gas constant = 8.3145 (Kg.m2/sec2) / (K.mol)
T = absolute tempreture
M = mass of mole of gas in kilogram
According to formula tempreute is directly proportional to veocity of molecule therefore at high tempreture velocicity of molecule is high.
2.)
molar mass of CO2 = 44.01 gm/mole therefore 22.1 gm = 22.1/44.01 = 0.5 mole
10.99 psi = 0.7478 atm
300C = 303.15 K
We know that ideal gas equatiion PV = nRT
V = nRT/P
n = 0.5 mole,
T = 300C = 30+273.15 = 303.15K,
P= 0.7478 atm,
R = 0.08205 L atm mol-1 K-1 ( R = gas constant)
V = ?
Substitute these value in above equation.
V = 0.5 X 0.08205 X 303.15 / 0.7478 = 16.63 liter
volume of CO2 = 16.63 L
3)
a)
According to dalton's law total pressure of gas is equal to sum of partial pressure exerted by each individual gas
Ptotal = P1 + P2 + P3
= PH2 + PHe + PAr = 135 + 100 + 368 = 603 torr
total pressure of gas mixture = 603 torr
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