Use the van der Waals equation of state to calculate the pressure of 3.90 mol of Kr at 467 K in a 3.80 L vessel. Van der Waals constants can be found in the van der Waals constants table.   Use the ideal gas equation to calculate the pressure under the same conditions.   In a 16.80 L vessel, the pressure of 3.90 mol of Kr at 467 K is 8.90atm when calculated using the ideal gas equation and 8.64 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 3.80 L compared to the  16.80 L vessel?

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Q: For a certain hydrocarbon gas, 20.0 mg exerts a pressure of 24.7 torr in a 500-cm3 vessel at 25…

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Q: What is the density, in grams per liter, of a gas with a molar mass of 17.02gmol at 303 K and 1.50…

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A:

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A: Solution -

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Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.