Question

3. Calculate the work that must be done on the system to compress 10 moles of hydrogen from 30 to 10 atmospheres isothermally (assume reversible) using three different methods: a) Hydrogen as an ideal gas, b) hydrogen as a van der Waals gas, and c) using the virial equation model. The van der Waals constants for hydrogen are a = 0.2461 liters • atm mole? and b = 0.02668 mole, and in the range of pressure 0-1500 atm, the virial equation for hydrogen is PV = RT (1 + 6.4 x 10P).

please answer neatly with a typed out solution explaining as you go. thank you!!

Answer 1

Melo d t=0. Crsothermal | = c ch t = 3cay. - W = Lef T=29°C. ...9) 4 oy an ideal gal.. a dext (ORT 1. V -- MRTE [OX 0.0838-700 4:3-dm3 6 xoo33 Хgoo V = nRT _ JOY 0.063 X 500 - 8.3-24.9 8.314 0.063 W=-1 (G- 3-349 = 76605 밸에 의, 유의 a et and a (x - 2) = ART Remaining two method calculate it V by putting value of other const which are given of then use tot w = -Pext dv.