A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the ideal gas law, and (b) the van der Waals equation. (c)A much more accurate equation is the virial equation, C(T) B(T) = 1+ V pVm RT where B(T) and C(T) are functions of temperature. For neon at 25°C, the values of B(T) and C(T) are 11.42 cm3.mol-1 and 221 cm.mol2, respectively. Assuming the pressure calculated using the virial equation is the "true" value, determine the percent error by using ideal gas law and van der Waals equation.

A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the ideal gas law, and (b) the van der Waals equation. (c)A much more accurate equation is the virial equation, C(T) B(T) = 1+ V pVm RT where B(T) and C(T) are functions of temperature. For neon at 25°C, the values of B(T) and C(T) are 11.42 cm3.mol-1 and 221 cm.mol2, respectively. Assuming the pressure calculated using the virial equation is the "true" value, determine the percent error by using ideal gas law and van der Waals equation.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 45QRT: At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove...

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