?In an industrial process, nitrogen is heated to 500 K at a constant volume of \(1.000
Chapter 1, Problem E1C.4(a)(choose chapter or problem)
In an industrial process, nitrogen is heated to 500 K at a constant volume of \(1.000 \mathrm{m}^{3}\). The mass of the gas is 92.4 kg. Use the van der Waals equation to determine the approximate pressure of the gas at its working temperature of 500 K. For nitrogen, \(a=1.352 \mathrm{dm}^{6} \mathrm{atmmol}^{-2}\),\(b=0.0387 \mathrm{dm}^{3} \mathrm{~mol}^{-1}\).
Text Transcription:
1.000 m^3
a = 1.352 dm^6 atm mol^−2
= 0.0387 dm^3 mol^−1
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