JAWAHARLAL NEHRU TECHNOLOGICAL UNIVERSITY HYDERABAD
JAWAHARLAL NEHRU TECHNOLOGICAL UNIVERSITY HYDERABAD B.Tech II MATERIALS THERMODYNAMICS Previous Question Paper (March - 2021 - R18)
Answer any five questions. All questions carry equal marks.
Main
Define intensive property, extensive property and explain the isolated system. Give examples.
Answer
Intensive property: A property whose value is independent of the mass or size of the system. Examples include temperature, pressure, and density.
Extensive property: A property whose value depends on the size or extent of the system. Examples include total mass, total volume, and total internal energy.
Isolated system: A system that exchanges neither energy (heat or work) nor matter with its surroundings. The total mass and energy of an isolated system remain constant. An example is a perfectly insulated, rigid container.
What is meant by process? List out the reasons for irreversibility of the process.
Answer
A process is any change that a system undergoes from one equilibrium state to another. When a process proceeds in such a manner that the system remains infinitesimally close to an equilibrium state at all times, it is called a quasi-equilibrium or quasi-static process.
The reasons for irreversibility include:
- Friction: Mechanical friction between moving parts converts kinetic energy into internal energy (heat), which cannot be fully recovered.
- Unrestrained expansion: Gas expanding into a vacuum cannot perform work, and the process is inherently irreversible.
- Heat transfer across a finite temperature difference: Heat flow from a high-temperature source to a low-temperature sink is irreversible.
- Mixing of substances: The spontaneous mixing of two different gases or fluids is irreversible.
- Chemical reactions: Rapid or uncontrolled chemical reactions are typically irreversible.
- Electrical resistance: The dissipation of electrical energy into heat through a resistor is irreversible.
Prove that
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A mass of 2.5 kg of air is compressed in a quasi-static process from the initial pressure of 0.1 MPa to a final pressure of 0.7 MPa for which
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State and explain the third law of thermodynamics along with two applications.
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Show that the total entropy of the universe increases for an irreversible process.
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Prove that the Gibb’s free energy and Helmholtz free energies are functions of state.
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A container having 3 compartments contains 1 mole of gas A, 2 moles of gas B and 3 moles of gas C at same temperature, pressure (298 K and 1 atm). The partitions are lifted and gases are allowed to mix. Calculate the change in Gibb’s free energy (Assume the gases behave ideally).
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Derive the Maxwells’ relations from the thermodynamic relations and discuss their importance.
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Explain the effect of temperature and pressure on equilibrium constant.
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Compare Raoult’s law and Henry’s law? Give their usefulness.
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Derive Gibbs’ Duhem equation in terms of partial molar quantities.
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Draw the Ellingham diagram of materials and discuss its important characteristics along with their applications.
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Explain about:
Kirchhoff’s equation
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Clausius - Clapeyron equation
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Richardson’s diagrams.
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