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122ch10b_001

# 122ch10b_001 - 37 10.76 u = 3RT = 3RT 1 2 At constant T u...

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37 10.76) At constant T, u = (1/ ) 1/2 a) The larger the molar mass, the slower the avg. speed (at constant T). SF 6 < HBr < Cl 2 < H 2 S < CO (g/mol) 146.06 80.91 70.91 34.08 28.01 Dec , Inc speed ( u ) b) Calculate the rms speeds of CO and Cl 2 at 30 0 K. Use eqn above and make sure R, T and are in SI units (8.314 J/mol C K or kg C m 2 /s 2 C mol C K, Kelvin, kg/mol, respectively) to give SI units for u (m/s) 3 (8.314 kg C m 2 /s 2 C mol C K)(30 0 K) u CO = (-------------------------------------------) 1/2 = 516.85 m/s = 516 m/s 28.01 x 10 -3 kg/mol 3 (8.314 kg C m 2 /s 2 C mol C K)(30 0 K) u Cl 2 = (-------------------------------------------) 1/2 = 324.84 m/s = 325 m/s 70.91 x 10 -3 kg/mol As expected, the lighter CO molecules move as the greater rms speed. 10.79) u RT RT = = 3 3 1 2 /

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38 10.79) (cont.) 10.80)
39 10.80) (cont.) 10.81) a) Gases behave non -ideally at HIGH Pressure and LOW Temp (Real gases behave ideally at low P and high T) b) Real gases behave non-ideally because they have: Finite Volumes: real gas particles occupy some of the volume of the container so the volume of free space for the molecules to move in is less than the container (causes P measured > P ideal ) - Positive deviations from ideality Intermolecular Attractive Forces: Real gases have AF and attract each other - causes the measured pressure to be less than ideal (P m < P i ) - Negative deviations from ideality c) For an ideal gas, PV/RT = n, the number of moles of gas particles, which should be a constant for all pressure, volume and temperature conditions (for 1 mole of gas PV/RT = 1 or PV/nRT = 1 is equivalent).

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