25 Questions MCQ Test Mechanical Engineering SSC JE (Technical) - Test: Thermodynamics Level - 1
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During free expansion, no work is done by the gas. The gas goes through states of no thermodynamic equilibrium before reaching its final state, which implies that one cannot define thermodynamic parameters as values of the gas as a whole. So work done in a free expansion process is Zero.
Perfect gas, also called ideal gas, a gas that conforms, in physical behaviour, to a particular, idealized relation between pressure, volume, and temperature called the general gas law. This law is a generalization containing both Boyle’s law and Charles’s law as special cases and states that for a specified quantity of gas, the product of the volume v and pressure p is proportional to the absolute temperature t; i.e., in equation form, pv = kt, in which k is a constant. Such a relation for a substance is called its equation of state and is sufficient to describe its gross behaviour.
Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
In nonrelativistic classical mechanics, a closed system is a physical system that doesn't exchange any matter with its surroundings, and isn't subject to any net force whose source is external to the system. A closed system in classical mechanics would be considered an isolated system in thermodynamics.
Explanation: Superheated vapor refers to a state where a substance is heated beyond its boiling point while maintaining its gaseous form. In this state, the vapor does not contain any liquid droplets and is considered to be in a supercritical state. Here is a detailed explanation of why superheated vapor behaves approximately as a gas: 1. Definition of a gas: - A gas is a state of matter where particles are widely spread apart and move freely in all directions. - It does not have a definite shape or volume. 2. Characteristics of superheated vapor: - Superheated vapor is a gaseous phase of a substance that has been heated above its boiling point. - It does not contain any liquid droplets. - The particles in superheated vapor have high kinetic energy and move rapidly. - The vapor molecules are widely spread apart, similar to a gas. 3. Comparison between superheated vapor and gas: - Superheated vapor behaves similarly to a gas because both have particles that are widely spread apart and move freely. - Both superheated vapor and gas do not have a definite shape or volume. - The behavior of superheated vapor is often approximated to that of a gas due to its similarities in particle movement and distribution. 4. Differences between superheated vapor and steam: - Steam refers to the gaseous phase of water at or below its boiling point. - Steam can contain liquid droplets due to condensation or partial vaporization. - Superheated vapor, on the other hand, does not contain any liquid droplets and is in a more energetic state compared to steam. In conclusion, superheated vapor behaves approximately as a gas because its particles are widely spread apart, move freely, and do not have a definite shape or volume. However, it is important to note that superheated vapor is a distinct state of matter and should not be confused with steam, which can contain liquid droplets.
A piston cylinder contains 0.5 kg of air at 500 kPa and 500 K. The air expands in a process so pressure is linearly decreasing with volume to a final state of 100 kPa and 300 K. Find the work in the process.
Avogadro's law states that, "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules." For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.
The absolute zero pressure will be when the molecular momentum of the system becomes zero. ... Thus, Pressure P = F/A = Rate of change of momentum/Area. Now when the ''rate of change of momentum' is zero, the above equation becomes: P = 0 / area = 0 which is the absolute zero pressure.
Liquids are volatile. If taken to zero pressure which effectively means vacuum, in that case, it will boil and vapourise. While different liquids have different viscosity but eventually it will vapourise as there is no pressure to help it maintain the viscosity and surface tension. Water will vapourise much faster than say mercury.
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