Fundamentals of thermodynamics system surroundings state functions - Question Bank

1. Which of the following is the most appropriate definition of a thermodynamic system?
A) Any object in the universe.
B) A specific region or quantity of matter chosen for study, separated from its surroundings by a boundary.
C) The boundary itself.
D) Everything outside the chosen region.
2. The term 'surroundings' in thermodynamics is important because:
A) It is always identical to the system.
B) It is the source or sink of energy and matter exchanged with the system.
C) It defines the path of the process.
D) It is irrelevant to the system's state.
3. What is the primary difference between a state function and a path function?
A) State functions are measurable, path functions are not.
B) State functions depend only on the initial and final states, path functions depend on the process.
C) Path functions are always positive, state functions can be negative.
D) State functions are always zero for cyclic processes, path functions are not.
4. Which of the following is a property that describes the 'state' of a gas in a container?
A) The speed at which it was filled.
B) The temperature of the gas.
C) The path taken by the gas molecules.
D) The history of its pressure changes.
5. In thermodynamics, a 'state' refers to:
A) A specific point in time during a process.
B) A condition of the system defined by its measurable properties.
C) The trajectory of a chemical reaction.
D) The energy transferred between system and surroundings.
6. Which of the following is a consequence of the First Law of Thermodynamics?
A) Heat cannot spontaneously flow from a colder body to a hotter body.
B) Energy can be created but not destroyed.
C) Energy can be destroyed but not created.
D) Energy is conserved in all processes.
7. If a system undergoes a process where q = -200 J and w = +50 J, what is ΔU?
A) -150 J
B) -250 J
C) 150 J
D) 250 J
8. 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:
A) Zero
B) Positive
C) Negative
D) Cannot be determined without knowing the pressure.
9. Which statement about path functions is correct?
A) Their values depend only on the initial and final states.
B) Their values depend on the process followed.
C) Their sum is always zero for a cyclic process.
D) They are always zero for an isothermal process.
10. The change in enthalpy (ΔH) is equal to the heat transferred (q) when:
A) The process occurs at constant volume.
B) The process occurs at constant temperature.
C) The process occurs at constant pressure.
D) The process occurs adiabatically.
11. Which of the following is a fundamental state function?
A) Work
B) Heat
C) Internal Energy
D) Entropy
12. The state of a thermodynamic system is defined by:
A) The path it took to reach the current condition.
B) A set of its observable properties.
C) The amount of work done.
D) The amount of heat exchanged.
13. A system is in thermodynamic equilibrium if it is simultaneously in:
A) Thermal and chemical equilibrium.
B) Mechanical and chemical equilibrium.
C) Thermal and mechanical equilibrium.
D) Thermal, mechanical, and chemical equilibrium.
14. If a system is in mechanical equilibrium with its surroundings, it means:
A) There is no heat transfer.
B) There is no mass transfer.
C) The pressure is uniform throughout the system and its surroundings.
D) The temperature is uniform throughout the system and its surroundings.
15. A system that is in thermal equilibrium with its surroundings has:
A) The same temperature as the surroundings.
B) The same pressure as the surroundings.
C) The same volume as the surroundings.
D) No interaction with the surroundings.
16. Which of the following is a property of the surroundings?
A) The total energy content of the system.
B) The temperature of the system.
C) The pressure exerted by the system.
D) The amount of matter outside the defined system.
17. The boundary between the system and surroundings can be:
A) Only rigid
B) Only flexible
C) Rigid, flexible, or imaginary
D) Only imaginary
18. A system consisting of ice and water at equilibrium is an example of:
A) Homogeneous system
B) Heterogeneous system
C) Open system
D) Isolated system
19. Which of the following is a homogeneous system?
A) A mixture of oil and water
B) A solution of salt in water
C) Sand and water
D) Ice and water
20. For a process occurring at constant pressure, the heat absorbed or released is equal to the change in:
A) Internal energy
B) Enthalpy
C) Entropy
D) Gibbs free energy
21. Enthalpy (H) is a state function defined as:
A) H = U - PV
B) H = U + PV
C) H = U
D) H = PV
22. The difference between enthalpy (H) and internal energy (U) is given by:
A) H = U - PV
B) H = U + PV
C) H = U - nRT
D) H = U + nRT
23. What is the unit of energy in the SI system?
A) Watt
B) Joule
C) Pascal
D) Newton
24. The equation of state for an ideal gas, PV = nRT, relates which state variables?
A) Pressure, Volume, Temperature
B) Pressure, Work, Heat
C) Internal Energy, Heat, Work
D) Volume, Enthalpy, Entropy
25. Which of the following is NOT a state variable for a real gas?
A) Pressure
B) Temperature
C) Volume
D) Intermolecular forces
26. In an adiabatic expansion of an ideal gas, what happens to the internal energy?
A) It increases.
B) It decreases.
C) It remains constant.
D) It depends on the volume change.
27. For an isothermal process in an ideal gas, the change in internal energy is:
A) Always positive.
B) Always negative.
C) Zero.
D) Dependent on pressure.
28. In an exothermic process where no work is done, what is the change in internal energy?
A) Positive and equal to the heat released.
B) Negative and equal to the heat released.
C) Zero.
D) Positive and equal to the heat absorbed.
29. If a system absorbs 100 J of heat and does 50 J of work, what is the change in internal energy?
A) 50 J
B) 100 J
C) 150 J
D) -50 J
30. According to the First Law of Thermodynamics, ΔU = q + w, where 'w' represents:
A) Work done by the system.
B) Work done on the system.
C) Heat absorbed by the system.
D) Heat released by the system.
31. The internal energy (U) of a system is defined as:
A) The sum of kinetic and potential energies of all particles in the system.
B) The energy transferred as heat.
C) The energy transferred as work.
D) The total energy of the universe.
32. The First Law of Thermodynamics is a statement of the conservation of:
A) Mass
B) Energy
C) Momentum
D) Charge
33. Which of these is a macroscopic state variable for a gas?
A) The motion of individual gas molecules
B) The pressure of the gas
C) The average kinetic energy of molecules
D) The type of intermolecular forces
34. Which of the following is a property that defines the state of a thermodynamic system?
A) Process
B) Work
C) State variable
D) Surroundings
35. Consider a gas expanding from volume V1 to V2. The work done by the gas is:
A) A state function.
B) A path function.
C) Always zero.
D) Independent of the final volume.
36. For a cyclic process, the change in a state function over the entire cycle is:
A) Maximum
B) Minimum
C) Zero
D) Equal to the heat absorbed
37. Which of the following is a path function?
A) Temperature
B) Volume
C) Heat
D) Enthalpy
38. The change in internal energy (ΔU) of a system is always:
A) Equal to the heat absorbed.
B) Equal to the work done by the system.
C) Independent of the path taken.
D) Dependent on the path taken.
39. If a system undergoes a change from state A to state B, the change in a state function depends on:
A) The specific path followed from A to B.
B) Only state A.
C) Only state B.
D) The initial and final states (A and B).
40. Which of the following is NOT a state function?
A) Pressure
B) Volume
C) Temperature
D) Work
41. Which of the following is a state function?
A) Work done
B) Heat transferred
C) Internal energy
D) Enthalpy change
42. What is a state function in thermodynamics?
A) A property that depends on the path taken to reach a state.
B) A property whose value depends only on the current state of the system, not on the path.
C) A property that measures the rate of change.
D) A property that is always zero.
43. A system where no heat can be transferred across its boundary is called:
A) Open system
B) Closed system
C) Adiabatic system
D) Isolated system
44. Which of the following is an example of an open system?
A) A sealed thermos flask
B) A boiling pot of water without a lid
C) A perfectly insulated container
D) A closed reaction vessel
45. An isolated system is characterized by:
A) Exchange of energy but not matter
B) Exchange of matter but not energy
C) Exchange of both energy and matter
D) No exchange of energy and no exchange of matter
46. In a closed system, what can be exchanged with the surroundings?
A) Only matter
B) Only energy
C) Both matter and energy
D) Neither matter nor energy
47. Which type of system allows both energy and matter to be exchanged with its surroundings?
A) Isolated system
B) Closed system
C) Adiabatic system
D) Open system
48. What is the purpose of the system boundary in thermodynamics?
A) To define the surroundings.
B) To isolate the system from its surroundings and control energy and mass transfer.
C) To represent the state of the system.
D) To measure the temperature of the surroundings.
49. In thermodynamics, what is defined as everything that is not part of the system?
A) System boundary
B) State variables
C) Surroundings
D) Internal energy
50. Which of the following is a characteristic of a thermodynamic system?
A) It is the region outside the boundaries of the system.
B) It is a precisely defined region of space or quantity of matter.
C) It is the interface between the system and its surroundings.
D) It represents the total energy of the universe.
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