For a van der Waal's gas, the critical pressure and temperature are 73.89 atm and 27°C, respectively. What is the volume (in ml) occupied only by the molecules in a sample of gas containing its 2

Question

For a van der Waal's gas, the critical pressure and temperature are 73.89 atm and 27°C, respectively. What is the volume (in ml) occupied only by the molecules in a sample of gas containing its 24 moles?

TestHub · Accepted Answer

For a van der Waals gas, b = RT c /(8P c ). With T c = 300 K and P c = 73.89 atm, using R = 0.0821 L-atm/K-mol: b = (0.0821 × 300)/(8 × 73.89) = 24.63/591.12 = 0.04167 L/mol. The excluded volume b equals 4 times the actual volume of the molecules themselves, so the molecular (own) volume per mole is b/4 = 0.01042 L/mol. For 24 moles: V = 24 × 0.01042 = 0.250 L = 250 ml. Hence the answer is 0250.

Chemistry - Real Gas Question with Solution | TestHub

Doubts & Discussion