To prevent tank rupture during deep-space travel, an engineering team is studyin

Question

To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 3.00 mol of gas D measured at 251 C in a 1.75-L container assuming real behavior?

Express your answer with the appropriate units.

Note: this question is asking based on REAL and not IDEAL behavior. Please help.

Real gases, especially under extremes of temperature and pressure, deviate from ideal behavior due to intermolecular forces and the volume occupied by the gas molecules themselves. Correction factors can be applied to the ideal gas equation to arrive at the van der Waals equation,

P=nRTVnbn2aV2

where a and b are van der Waals constants for the particular gas. The term nb corrects the volume to account for the size of the molecules and the term n2a/V2 corrects the pressure for intermolecular attraction.

Explanation / Answer

PV = nRT

van der waals:

v = V/n

(P-a/v^2)(v-b) = RT

Solve for P

P = RT/(v-b) + a/v^2

substitute known data

v = V/n = 1.75/3 = 0.583

P = 0.082*(251+273)/(0.583-b) + a/(0.583^2)

we need a and b from gas...

substitute a and b and you get Pressure in atm

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