The Joule-Thomson coefficient for a van der Waals gas is given by μ = [(2a/RT) - b]/Cp. Calculate the value of AH in calories for the isothermal, 300 K, compression of 1 mole of nitrogen from 1 to 500 atm: a = 4.17 L² atm mol-2, b = 0.039 L/mol.

The Joule-Thomson coefficient for a van der Waals gas is given by μ = [(2a/RT) - b]/Cp. Calculate the value of AH in calories for the isothermal, 300 K, compression of 1 mole of nitrogen from 1 to 500 atm: a = 4.17 L² atm mol-2, b = 0.039 L/mol.

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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.

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The Joule-Thomson coefficient for a van der Waals gas is given by μ = [(2a/RT) - b]/Cp.
Calculate the value of AH in calories for the isothermal, 300 K, compression of 1 mole of
nitrogen from 1 to 500 atm: a = 4.17 L² atm mol-2, b = 0.039 L/mol.

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