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CHEM 155 TRIAL QUESTIONS 1. How many states of matter exist? a. 1 b. 2 c. 3 d. 4 d. 5 2.What state of matter are the particles the farthest apart? a. Solid b. Liquid c. Gas d. Plasma 3. a. b. c. d. 4. a. b. c. d. What state of matter are the particles the closest together? Liquid Gas Plasma Solid What state of matter are the particles moving in one direction? solid Liquid Gas Plasma 5. Purity of a substance can be estimated through a. boiling points b. melting points c. None of These d. Both A and B 6. The melting point of ice is the same as the freezing point of water. a. True b. False 7. When water vaporizes at room temperature, it changes into a. Water vapour b. Fog c. Steam d. Ice 8. Liquids have the ability to flow because a. their particles can slide over each other. b. their particles are arranged in a regular pattern. c. their particles are very far apart. d.There are strong forces of attraction between the particles. 9. When two gases mix together, they are said to a. Condense b. Evaporate c. Diffuse d. Melt 10. Which one of the following is not a property of gases? a. They have a definite mass. b. They can diffuse. c. They have no definite shape. d. They have a definite volume. 11. Which one of the following states of matter can easily be compressed? a. Gas or liquid b. Gas c. Liquid d. Solid 12. Dry ice is used in fire extinguishers. The dry ice is stored in the cylinder in a solid form. When sprayed on a fire it quickly changes into the gas known as carbon dioxide (CO2). What is this change of state called? a. Evaporation b. Sublimation c. Condensation d.. Distillation 13. A gas will approach ideal behaviour at a. High temperature,low pressure b. Low temperature,high pressure c. Low temperature, low pressure d. High temperature,high pressure 14. If both temperature and volume of a gas doubled, the pressure? a. Also doubled b. Is reduced to half c. Remain unchanged d. increases four times 15. A mixture of gas expands from 0.03 m3 to 0.06 m3 at a constant pressure of 1 MPa and absorbs 84 kJ of heat during the process. The change in internal energy of the mixture is a. 54 kJ b. 84 kJ c. 114 kJ d. 30 kJ 16. In an irreversible process, there is a a. no loss of heat b. gain of heat c. no gain of heat d. loss of heat 17. The measurement of a thermodynamic property known as temperature is based on a. none of these b. Second law of thermodynamics c. Zeroth law of thermodynamics d. First law of thermodynamics 18. In an isothermal process a. there is no change in internal energy b. there is no change in temperature c. there is no change in enthalpy d. all of these 19. When two bodies are in thermal equilibrium with a third body, they are also in thermal equilibrium with each other. This statement is called a. Zeroth law of thermodynamics b. Second law of thermodynamics c. First law of thermodynamics d. Kelvin Planck's law 20. The area under the temperature-entropy curve (T – s curve) of any thermodynamic process represents a. heat rejected b. none of these c. heat absorbed d. either heat absorbed or heat rejected 21. Which of the following is the correct statement of the second law of thermodynamics? a. It is impossible to transfer heat from a body at a lower temperature to a higher temperature, without the aid of an external source. b. all of the above c. It is impossible to construct an engine working on a cyclic process, whose sole purpose is to convert heat energy into work. d. There is a definite amount of mechanical energy, which can be obtained from a given quantity of heat energy. 22. Workdone in a free expansion process is a. zero b maximum c. minimum d. positive 23. The processes occurring in open system which permit the transfer of mass to and from the system, are known as a. non-flow processes b. adiabatic processes c. none of these d. flow processes 24. The amount of heat required to raise the temperature of the unit mass of gas through one degree at constant volume, is called a. specific heat at constant volume b. specific heat at constant pressure c. none of these d. kilo Joule 25. An adiabatic process is one in which a. no heat enters or leaves the gas b. the change in internal energy is equal to the mechanical work done c. the temperature of the gas changes d. all of the above 26. The sum of internal energy (U) and the product of pressure and volume (p.v) is known as a. workdone b. none of these c. enthalpy d. entropy 27. A series of operations, which takes place in a certain order and restore the initial conditions at the end, is known as a. reversible cycle b. irreversible cycle c. thermodynamic cycle d. none of these 28. An isothermal process is governed by a. Avogadro's law b. Charles' law c. Gay-Lussac law d. Boyle's law 29. The entropy of water at 0°C is assumed to be a. 1 b. -1 c. 0 d. 2 30. A process, in which the temperature of the working substance remains constant during its expansion or compression, is called a. isothermal process b. hyperbolic process c. polytropic process d. adiabatic process 31. The specific heat of water is a. none of these b. 4.187 c. 1.817 d. 2512 32. Which of the following is an intensive property of a thermodynamic system? a. Mass b. Temperature c. Energy d. Volume 33. Which one of the following definitions best describes the concept of work? a. the flow of energy from one object or substance to another due to a difference in temperature b. the flow of energy from one body to another through uniform molecular motion c. d. the force associated with molecular motion the random motion of molecules in a gas at low pressure 34. An isolated system is best described by which one of the following statements? a. Neither matter nor heat can pass into or out of the system b. The system has a boundary which allows heat to be transferred but does not allow material to pass into or out of the system c. The system has a diathermic boundary d. A system which has reached thermal equilibrium with its surroundings 35. Which one of the following statements describes a path function? a. A property of a system that depends only on the current state of the system, not on the path the system took to reach that state b. A property of a system that depends on the path taken between the initial and final states c. The sum of kinetic and potential energy contained in a substance d. The heat energy absorbed by a system at constant pressure 36. Consider the following thermodynamic properties. i) work done on a system ii) heat absorbed iii) entropy iv) enthalpy Which of these properties are state functions? a. b. c. d. i) and ii) only i) and iii) only i) only iii) and iv) only 37. Which of the following statements best describes the Second Law of Thermodynamics? a. The internal energy of the universe is constant. b. Energy can be neither created nor destroyed. c. When an isolated system undergoes a spontaneous change, the entropy of the system will increase. d. At absolute zero, the entropy of a perfect crystal is considered to be zero. 38. A drug used to treat hypertension undergoes a decomposition reaction to give an insoluble product. Calculate the temperature at which this reaction becomes spontaneous if the enthalpy of the reaction at 298 K is 51 kJ mol-1 and the entropy of the reaction at this temperature is 118.74 J K-1 mol-1. a. b. c. d. 430 K 2 300 K 0.5 K 430oC 39. Which one of the following equations defines the enthalpy of reaction, ΔH, for a reaction occurring at constant pressure that does expansion work? All terms have their usual meanings. a. b. c. d. ΔH = ΔU ΔH = ΔU + pΔV ΔH = ΔG - TΔS ΔH = q + w 40. Which of the following statements will always apply when a reversible chemical reaction has attained equilibrium? a. b. c. d. All reactants will convert to products The reaction proceeds alternately in the forward and reverse directions The Gibbs free energy of the system reaches a minimum The forward reaction will dominate over the reverse reaction 41. Which one of the following is an expression of the van't Hoff equation? a. b. c. d. ln K = - ΔHθ / RT + ΔSθ /R ΔH(T2) = ΔH(T1) + ΔCp(T2 - T1) ΔGθ = ΔHθ - TΔSθ ΔU = q + w 42. What law asserts that energy is a thermodynamic property? A. First law of Thermodynamics B. Second law of Thermodynamics C. Third law of Thermodynamics D. Zeroth law of Thermodynamics 43. What law asserts that energy has quality as well as quantity? A. First law of Thermodynamics B. Second law of Thermodynamics C. Third law of Thermodynamics D. Zeroth law of Thermodynamics 44. The macroscopic approach to the study of thermodynamics does not require a knowledge of the behavior of individual particles is called _____. A. Dynamic thermodynamics B. Static thermodynamics C. Statistical thermodynamics D. Classical thermodynamics 45. What is the more elaborate approach to the study of thermodynamics and based on the average behavior of large groups of individual particles? A. Dynamic thermodynamics B. Static thermodynamics C. Statistical thermodynamics D. Classical thermodynamics 46. What is a defined region in space chosen for study? A. Surroundings B. System C. Boundary D. Volume 47. The first law of thermodynamics is based on which of the following principles? A. Conservation of mass B. Conservation of energy C. Action and reaction D. The entropy-temperature relationship 48. What is the mass or region outside the system called? A. Surroundings B. Boundary C. Volume D. Environment 49. What is the real or imaginary surface that separates the system from its surroundings? A. Division B. Wall C. Boundary D. Interface 50. A system which consists of fixed amount of mass and no mass can cross its boundary called _____. A. Equilibrium system B. Thermal equilibrium system C. Open system D. Closed system 51. A system in which even energy is not allowed to cross the boundary is called ____. A. Closed system B. Exclusive system C. Isolated system D. Special system 52. A system in which there is a flow of mass is known as _____. A. Equilibrium system B. Isolated system C. Open system D. Closed system 53. Open system usually encloses which of the following devices? A. Compressor B. Turbine C. Nozzle D. All of the above 54. The boundaries of a control volume, which may either real or imaginary is called _____. A. Control boundary B. Control system C. Interface D. Control surface 55. Any characteristic of a thermodynamics system is called a _____. A. Property B. Process C. Phase D. Cycle 56. How are thermodynamic properties classified? A. Physical and chemical B. Intensive and extensive C. Real and imaginary D. Homogeneous and heterogeneous 57. The thermodynamic properties that are independent on the size of the system is called _____. A. Extensive property B. Intensive property C. Open property D. Closed property 58. The thermodynamic properties that are dependent on the size or extent of the system is called _____. A. Extensive property B. Intensive property C. Open property D. Closed property 59. Which is NOT an intensive property of thermodynamics? A. Temperature B. Mass C. Pressure D. Density 60. Which is NOT an extensive property of thermodynamics? A. Density B. Mass C. Volume D. Energy 61. Extensive properties per unit mass are called _____. A. Specific properties B. Relative properties C. Unit properties D. Phase properties 62. A system is in ______ equilibrium if the temperature is the same throughout the entire system. A. Static B. Thermal C. Mechanical D. Phase 63. A system is in ______ equilibrium if there is no change in pressure at any point of the system with time. A. Pressure B. Thermal C. Mechanical D. Phase 64. If a system involves two phases, it is in ______ equilibrium when the mass of each phase reaches an equilibrium level and stays there. A. Chemical B. Thermal C. Mechanical D. Phase 65. A system is in ______ equilibrium of its chemical composition does not change with time, i.e., no chemical reaction occurs. A. Chemical B. Thermal C. Mechanical D. Phase 66. “The state of a simple compressible system is completely specified by two independent, intensive properties”. This is known as ______. A. Equilibrium postulate B. State postulate C. Environment postulate D. Compressible system postulate 67. What is the unit of the total energy of the system? A. Kj B. Kj/Kg C. Kg D. g 68. Without electrical, mechanical, gravitational, surface tension and motion effects, a system is called _____ system. A. Simple B. Simple compressible C. Compressible D. Independent 69. What refers to any change that a system undergoes from one equilibrium state to another equilibrium state? A. Process B. Path C. Phase D. Cycle 70. What refers to the series of state through which a system passes during a process? A. Path B. Phase C. Cycle D. Direction 71. How many independent properties are required to completely fix the equilibrium state of a pure gaseous compound? A. 4 B. 3 C. 2 D. 1 72. Three moles of an ideal gas (Cv = 5cal K-1 mol-1) at 10 atm and 0 are converted to 2.0atm at 50°. The ∆E for the process is A.150 cal B. 300 cal C. 750 cal D. 1500 cal 73. A closed system may refer to ______. A. Control mass B. Control volume C. Control energy D. Control temperature 74. An open system may refer to ______. A. Control mass B. Control volume C. Control energy D. Control temperature 75. A system is said to be in thermodynamic equilibrium if it maintains ______ equilibrium. A. Mechanical and phase B. Thermal and chemical C. Thermal, mechanical and chemical D. Thermal, phase, mechanical and chemical 76. What is a process with identical end states called? A. Cycle B. Path C. Phase D. Either path or phase 77. What is a process during which the temperature remains constant? A. Isobaric process B. Isothermal process C. Isochoric process D. Isometric process 78. What is a process during which the pressure remains constant? A. Isobaric process B. Isothermal process C. Isochoric process D. Isometric process 79. What is a process during which the specific volume remains constant? A. Isobaric process B. Isothermal process C. Isochoric or isometric process D. Isovolumetric process 80. The prefix “iso” used to designate a process means ______. A. Cannot be interchanged B. Remains constant C. Approximately equal D. Slight difference 81. What does the term “steady” implies? A. No change with volume B. No change with time C. No change with location D. No change with mass 82. What does the tem “uniform” implies? A. No change with volume B. No change with time C. No change with location D. No change with mass 83. What is defined as a process during which a fluid flows through a control volume steadily? A. Transient-flow process B. Steady and uniform process C. Uniform-flow process D. Steady-flow process 84. The sum of all the microscopic form of energy is called _____. A. Total energy B. Internal energy C. System energy D. Phase energy 85. What type of system energy is related to the molecular structure of a system? A. Macroscopic form of energy B. Microscopic form of energy C. Internal energy D. External energy 86. What form of energy refers to those a system possesses as a whole with respect to some outside reference frame, such as potential and kinetic energies? A. Macroscopic form of energy B. Microscopic form of energy C. Internal energy D. External energy 87. Who coined the word “energy” in 1807? A. William Rankine B. Rudolph Clausius C. Lord Kelvin D. Thomas Young 88. The molecules of a gas moving through space with some velocity possesses what kind of energy? A. Translational energy B. Spin energy C. Rotational kinetic energy D. Sensible energy 89. The electrons in an atom which rotate about the nucleus possess what kind of energy? A. Translational energy B. Spin energy C. Rotational kinetic energy D. Sensible energy 90. A gas expands from 10 litres to 20 litres against a constant external pressure of 10atm. The pressure volume work done by the system is i.100 lit atm ii.-100 lit atm iii.10 lit atm iv.-10 lit atm 91. The mathematical relation for the first law of thermodynamics is A. ∆E = q-w B. ∆E = 0 for a cyclic process C. ∆E = q for an isochoric process D. all of these 92 The change in enthalpy of a system is measured by measuring A. B. C. D. Heat of the process at constant volume Heat of the process at constant temperature Heat of the process at constant pressure None of these 93. The enthalpy change, ∆H of a process is given by the relation A. ∆H = ∆E + p ∆v B. ∆H = ∆E + ∆nRT C. ∆H = ∆E + w D. 𝑎𝑙𝑙 𝑜𝑓 𝑡ℎ𝑒𝑠𝑒 94. Which of the following relations is true? A. Cp > Cv B. CV > CP C. Cp = Cv D. Cp = Cv = 0 95. The heat capacity of constant pressure is related to heat capacity at constant volume by the relation A. Cp – R = Cv B. Cv – R = Cp C. Cp – Cv = R D. R - Cp = Cv 96. The enthalpy change of a reaction is independent of A. state of the reactants and products B. nature of the reactants and products C. initial and final enthalpy change of the reaction D. different intermediate reaction 97. One mole of an ideal gas at 300K is expanded isothermally from 1 litre volume to 10 litre volume. ∆E for this process is (R= 2 cal K-1 mol-1) A. 300 cal B. 600 cal C.1200 cal D.0 cal 98. A system absorbs 100kJ heat and performs 50kJ work on the surroundings. The increase in internal energy of the system is A. 50 kJ B. 100kJ C. 150kJ D. 5000Kj 99. For the reaction H2 + I2 A. ∆E + 2RT B. ∆E = 2RT C. ∆E D. ∆E + RT 2HI, ∆𝐻 IS EQUAL TO 100. The work done when 1 mole of a gas expands reversibly and isothermally from 5atm to 1atm at 300K is A. -4015 J B. +4015 J C. zero D. 150 J