Calculate the pressure exerted at 1000 K by 2 moles of C2H6 in a volume of 0.5 dm3 behaving as: (a) a perfect gas and (b) a van der Waals gas. [The van der Waals parameters for C2H6 are a = 5.562 dm6 atm mol-2 and b = 0.0638 dm3 /mol]. By what percentage does pressure obtained for the perfect gas deviate from the van der Waals prediction?

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Jarrod RobelLv2

29 Sep 2019

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For carbon dioxide gas the constants in the van der Waals equationare a = 0.364 J m3/mol2 and b = 4.27 x 10-5 m3/mol.
a. If 1.00 mol of CO2 gas at 350 K is confined to a volume of 400cm3, find the pressure of the gas using the ideal gas equation, andagain using the van der Waals equation.
b. Which equation gives a lower pressure? Why? What is thepercentage difference of the van der Waals equation result from theideal-gas equation result?
c. On page 691 of your book the difference for CO2 between theideal gas and van der Waalâs equation is worked out to be 0.5%.Explain why your calculation is different than that in the book?

redrhinoceros371

Physical Chem

1) A 10.60 mol sample of argon gas is maintained in a 0.8466 L container at 298.6 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L²atm/mol² and b = 3.219Ã10^-2 L/mol.

A: ______ atm

2) According to the ideal gas law, a 1.007 mol sample of argon gas in a 1.337 L container at 272.3 K should exert a pressure of 16.83 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Ar gas, a = 1.345 L²atm/mol² and b = 3.219Ã10^-2L/mol.

Hint: % difference = 100Ã(P _ideal - P_{van der Waals}) / P _ideal

A: ________% â

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