Mixture of ideal gases, Thermodynamics

## FAQs on Mixture of ideal gases, Thermodynamics - Mechanical Engineering

 1. What is a mixture of ideal gases?
Ans. A mixture of ideal gases refers to a combination of two or more gases that behave according to the principles of ideal gas behavior. In an ideal gas mixture, each gas component behaves independently and the total pressure of the mixture is the sum of the partial pressures of each gas component.
 2. How can the composition of a mixture of ideal gases be determined?
Ans. The composition of a mixture of ideal gases can be determined using various techniques. One common method is the use of gas chromatography, where the mixture is separated into its individual components based on their different affinities for a stationary phase. Another method is the application of Dalton's Law of partial pressures, where the partial pressure of each gas component is measured and used to calculate its mole fraction in the mixture.
 3. What is the significance of thermodynamics in studying a mixture of ideal gases?
Ans. Thermodynamics plays a crucial role in studying a mixture of ideal gases as it provides the fundamental principles and laws governing the behavior of these gases. Thermodynamic concepts such as the ideal gas law, Dalton's law, and the concept of entropy help in understanding and predicting the properties and behavior of gas mixtures under different conditions.
 4. Can the ideal gas law be applied to a mixture of non-ideal gases?
Ans. The ideal gas law is based on certain assumptions, including the absence of intermolecular forces and the negligible volume of gas particles. Therefore, it is not directly applicable to a mixture of non-ideal gases where these assumptions may not hold true. However, certain modifications and corrections can be made to the ideal gas law to account for deviations from ideality, such as using the Van der Waals equation or activity coefficients.
 5. How does the behavior of a mixture of ideal gases differ from that of a pure gas?
Ans. The behavior of a mixture of ideal gases differs from that of a pure gas in several ways. In a mixture, each gas component behaves independently, exerting its own partial pressure and following the ideal gas law. The total pressure of the mixture is the sum of the partial pressures. In contrast, a pure gas behaves as a single component, where the pressure is solely determined by the gas itself. Additionally, the properties of a mixture, such as the boiling point and density, can be different from those of the individual gases in the mixture due to interactions between gas particles.
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