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, В (Т) + Vm С (Т) pVm 1+ RT where B(T) and C(T) and C(T) are 11.42 cm3 mol1 and 221 cm6 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 are functions of temperature. For neon at 25°C, the values of B(T)
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, В (Т) + Vm С (Т) pVm 1+ RT where B(T) and C(T) and C(T) are 11.42 cm3 mol1 and 221 cm6 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 are functions of temperature. For neon at 25°C, the values of B(T)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter9: Gases
Section: Chapter Questions
Problem 104E: A 0.245-L flask contains 0.467 mol CO2 at 159 C. Calculate the pressure: (a) using the ideal gas law...
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