n moles of CO2 gas (T1, V1) obey a van der Waals equation of state are contained in an insulated piston-cylinder arrangement. A reversible expansion of the gas is carried out until the volume become 2V1.
[CV.m=28.80 J mol−1K−1,a=3.610 atm.dm6.mol−2,b=4.29 x 10−2 dm3.mol−1]
(a) Find the final temperature of gas as a function of n, 𝐂𝐕.𝐦 , T1, V1 and the van der Waals parameter a and b.
(b) If two moles of CO2 gas involved and T1 = 350K, V1 = 40L, compute final temperature of the gas.
(c) Find work done and internal energy of the gas.
a)Temperature of gas =49.3°C
b)Final Temperature =34.9°C
c)Work Done =267kW
Internal Energy =-471kJ
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Dear macdonald, please post a new question
At T= 100 K, 1.00 mol of CO2 occupies a volume of 1.00 L. Calculate the pressures given by the ideal gas equation and the van der Waals equation. (a= 3.610 atm dm6 mol-2) and (b = 4.29 dm3 mol-1).
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