For a van der Waal's gas, the critical pressure and temperature are 62.8 atm and 33°C, respectively. What is the volume (in ml) occupied only by the molecules in a sample of the gas containing 32

Question

For a van der Waal's gas, the critical pressure and temperature are 62.8 atm and 33°C, respectively. What is the volume (in ml) occupied only by the molecules in a sample of the gas containing 32 moles of it? (R = 0.0821 L-atm/K-mol)

TestHub · Accepted Answer

For a van der Waals gas, b = RT c /(8P c ) = (0.0821 × 306)/(8 × 62.8) = 25.12/502.4 = 0.05 L/mol. The excluded volume b is 4 times the actual volume of the molecules, so the molecular (own) volume per mole is b/4 = 0.0125 L/mol. For 32 moles: V = 32 × 0.0125 = 0.400 L = 400 ml. Hence the answer is 0400.

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