Fundamentals of thermodynamics system surroundings state functions - One Line Questions

1. If a system undergoes a process where q = -200 J and w = +50 J, what is ΔU? — -150 J
2. If a system absorbs 100 J of heat and does 50 J of work, what is the change in internal energy? — 150 J
3. Which of the following is a homogeneous system? — A solution of salt in water
4. What is a state function in thermodynamics? — A property whose value depends only on the current state of the system, not on the path.
5. Which of the following is an example of an open system? — A boiling pot of water without a lid
6. In thermodynamics, a 'state' refers to: — A condition of the system defined by its measurable properties.
7. Consider a gas expanding from volume V1 to V2. The work done by the gas is: — A path function.
8. For an isothermal process in an ideal gas, the change in internal energy is: — Zero.
9. Which of the following is the most appropriate definition of a thermodynamic system? — A specific region or quantity of matter chosen for study, separated from its surroundings by a boundary.
10. The change in internal energy (ΔU) of a system is always: — Independent of the path taken.
11. An isolated system is characterized by: —
12. The difference between enthalpy (H) and internal energy (U) is given by: — H = U + PV
13. Enthalpy (H) is a state function defined as: — H = U + PV
14. Which of the following is a consequence of the First Law of Thermodynamics? — Energy is conserved in all processes.
15. A system consisting of ice and water at equilibrium is an example of: — Heterogeneous system
16. For a process occurring at constant pressure, the heat absorbed or released is equal to the change in: — Enthalpy
17. Which type of system allows both energy and matter to be exchanged with its surroundings? — Open system
18. In an adiabatic expansion of an ideal gas, what happens to the internal energy? — It decreases.
19. The term 'surroundings' in thermodynamics is important because: — It is the source or sink of energy and matter exchanged with the system.
20. Which of the following is a characteristic of a thermodynamic system? — It is a precisely defined region of space or quantity of matter.
21. The First Law of Thermodynamics is a statement of the conservation of: — Energy
22. For a cyclic process, the change in a state function over the entire cycle is: — Zero
23. In a closed system, what can be exchanged with the surroundings? — Only energy
24. The boundary between the system and surroundings can be: — Rigid, flexible, or imaginary
25. A system where no heat can be transferred across its boundary is called: — Adiabatic system
26. In an exothermic process where no work is done, what is the change in internal energy? — Negative and equal to the heat released.
27. Which of the following is NOT a state function? — Work
28. Which of the following is NOT a state variable for a real gas? — Intermolecular forces
29. The equation of state for an ideal gas, PV = nRT, relates which state variables? — Pressure, Volume, Temperature
30. Which of the following is a property that defines the state of a thermodynamic system? — State variable
31. What is the primary difference between a state function and a path function? — State functions depend only on the initial and final states, path functions depend on the process.
32. In thermodynamics, what is defined as everything that is not part of the system? — Surroundings
33. Which of the following is a path function? — Heat
34. Which of these is a macroscopic state variable for a gas? — The pressure of the gas
35. The state of a thermodynamic system is defined by: — A set of its observable properties.
36. The change in enthalpy (ΔH) is equal to the heat transferred (q) when: — The process occurs at constant pressure.
37. A system that is in thermal equilibrium with its surroundings has: — The same temperature as the surroundings.
38. If a system undergoes a change from state A to state B, the change in a state function depends on: — The initial and final states (A and B).
39. Which of the following is a property that describes the 'state' of a gas in a container? — The temperature of the gas.
40. The internal energy (U) of a system is defined as: — The sum of kinetic and potential energies of all particles in the system.
41. Which of the following is a property of the surroundings? — The amount of matter outside the defined system.
42. Which statement about path functions is correct? — Their values depend on the process followed.
43. If a system is in mechanical equilibrium with its surroundings, it means: — The pressure is uniform throughout the system and its surroundings.
44. A system is in thermodynamic equilibrium if it is simultaneously in: — Thermal, mechanical, and chemical equilibrium.
45. What is the purpose of the system boundary in thermodynamics? — To isolate the system from its surroundings and control energy and mass transfer.
46. What is the unit of energy in the SI system? — Joule
47. Which of the following is a fundamental state function? — Internal Energy
48. Which of the following is a state function? — Internal energy
49. According to the First Law of Thermodynamics, ΔU = q + w, where 'w' represents: — Work done on the system.
50. Consider the process of heating 1 mole of an ideal gas from 300 K to 400 K at constant volume. The change in internal energy will be: — Positive
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