MDCAT Thermo-Chemistry and Energetics of Chemical Reactions Test Online

1. Which one is not state function?

2. The energy required to break 1 mole of bonds to form neutral atom is

3. The branch of science which deals with energy transformation is known as

4. Which one is not a state function?

5. Which type of reactions cannot occur spontaneously?

6. The S.I unit of heat and energy is

7. If internal energy of a system is increased

8. Endothermic changes are indicated through

9. What type of reaction releases energy and does not require initial energy to occur?

10. One of the statement about Born Haber cycle is correct. Which is that statement?

11. Change in enthalpy of a system can be calculated by following relationship

12. The reason of kinetic energy of the molecules of a gaseous substance among the following is

13. An adiabatic expansion of an ideal gas always has

14. The enthalpies of combustion of carbon and carbon monoxide are -383.5 and -283 kJ mol¯¹ respectively. The enthalpy of formation of carbon monoxide per mole is

15. The apparatus used to measure the enthalpy of combustion of a substance is

16. The enthalpies of combustion of carbon and carbon monoxide are -390 kJ mol¯¹ and -278 kJ mol¯¹ respectively. The enthalpy of formation of carbon monoxide is

17. Which of the following units represents largest amount of energy?

18. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

19. The law of thermodynamics that provides the basis for the determination of absolute entropy of substance is

20. In order to decompose 9 g of water 142.5 kJ of heat is required. Hence enthalpy of formation of water is

21. A spontaneous change means

22. Most of the thermodynamic parameters are

23. The amount of heat which is involved during the completion of a chemical reaction at 25°C and 1 atmospheric pressure is called

24. The reaction is spontaneous if the cell potential is

25. A chemist heated a balloon by supplying 600 J of heat. The balloon expands doing 200 J of work against the atmospheric pressure. The change in internal energy of

26. Two fundamental ways to transfer energy are

27. For a system in equilibrium, ∆ G = 0, under conditions of constant

28. The law of Lavoisier and Laplace illustrates

29. Which statement describes characteristics of an endothermic reaction?

30. One mole of an ideal gas expands isothermally to ten times its original volume. The change in entropy is

31. Free energy change for a reversible process is:

32. The enthalpies of all elements in their standard states are

33. Heat exchanged in a chemical reaction at constant temperature and pressure is called

34. All the naturally occurring processes proceed spontaneously in a direction which lead to

35. Hess’s law deals with

36. The net change in energy in a chemical reaction is same whether it takes place directly or indirectly is

37. 10.16 g of graphite is burnt in a bomb calorimeter and the temperature rise recorded is 3.78 K. Calculate the enthalpy of combustion of graphite if the heat capacity is 86.02 KJ K¯¹

38. Which of the following unit represent the largest amount of energy?

39. Enthalpy of combustion for food, fuel and other compounds can be measured accurately by

40. A particular reaction has a negative value for the energy change. Then at ordinary temperature

41. Mechanical work is especially important in systems that contain

42. What type of chemical reaction absorbs energy and requires energy for the reaction occur?

43. Evaporation of water is

44. Four containers hold the following quantity at the same temperature. Which one has the highest heat capacity?

45. An exothermic reaction is one in which the reacting substances

46. A material or a collection of materials which is under study is called

47. What is the entropy change (in JK¯¹ mol¯¹) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol¯¹ at 0°C)

48. The best characteristic of spontaneous reactions among the following is that

49. The enthalpy of formation of carbon monoxide will be

50. The heats evolved in combustion of rhombic and monoclinic sulphur are -70960 and -71030 cal mol¯¹ respectively. What will be heat of conversion of rhombic sulphur to monoclinic?

51. What would be the heat released when an aqueous solution containing 0.5 mole of HNO₃ is mixed with 0.3 mol of OH¯ (enthalpy of neutralization is -57.1 kJ)

52. The molar heat capacity of water at constant pressure, Cᵨ, is 75 JK¯¹ mol¯¹. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is

53. In general, for exothermic reactions to be spontaneous

54. Which of the following value of ∆Hf’ represent that the product is least stale?

55. C (diamond) → C(Graphite), ∆ H = -ve. This show that

56. For a melting of a solid at 25°C, the fusion process requires energy equivalent to 2906 Joules to be added to system considering the process to be reversible at fusion point, the entropy change of the process is

57. All of the following are state function except

58. A cylinder of gas supplied by PSO is assumed to contain 14 kg of butane. If a normal family requires 20,000 kJ of energy per day for cooking, butane gas in the cylinder last for ……. Days (∆Hc of C₄H₁₀ = -2658 kJ per mole)

59. When water is added to quick lime, the reaction is

60. An endothermic reaction is one in which

61. The unit which indicates the largest amount of energy is

62. Form the above data, the standard heat of formation of KOH in kcal mol¯¹ is

63. Calorie is equivalent to

64. The branch of chemistry which deals with thermal energy change in chemical reaction is called

65. In measurement of melting point of solid, the leaker used will be

66. Conversion of copper hydroxide into copper oxide and water is an example of

67. A mixture of ice and water contains 60 g of ice and water. If 60 J of heat energy is removed from this mixture, some of the

68. If at 298 K the bond energies of C-H, C-C, C=C and H-H bonds are respectively 414, 347, 615 and 435 kJ mol¯¹, the value of enthalpy change for the reaction H₂C = CH₂(g) + H₂(g) → H₃C – CH₃(g) at 298 K will be

69. Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are -382.64kJ mol¯¹ and -145.6kJ¯¹ mol¯¹ respectively. Standard Gibbs energy change for the same reaction at 298 K is

70. Pumping of water uphill is

71. In endothermic reactions, the heat content of the

72. If an endothermic reaction is allowed to take place very rapidly in the air, the temperature of the surrounding air

73. Burning of coal in air is initiated by a spark and it is an example of spontaneous reaction because

74. Which of the following statement is contrary to first law of thermodynamics?

75. Which law among the following has same net change whether it takes place directly or indirectly?

76. When enthalpy and entropy change for a chemical reaction are – 2.5 x 10³ cals and 7.4 cals deg¯¹ respectively. Predict that reaction at 298 K is

77. Unit of heat in S.I system is

78. Enthalpy of formation of HF and HCl are – 161 kJ and -92 kJ respectively. Which of the following statements is incorrect?

79. When enthalpy of reactants is higher than products, then reaction will be

80. Which of the following is not correct?

81. Two fundamental ways to transfer energy are

82. The heat required to raise the temperature of a body by 1 K is called

83. Unit of heat is SI system is

84. Total energy depends upon the state of system

85. The bond dissociation energies of H₂, CL₂ and HCl are 104, 58 and 103 kcal respectively. The enthalpy of formation of HCl gas will be

86. The ∆H values for reaction C + ½ O₂ → CO and CO + ½ O₂ → CO₂ are 100 and 200 kJ respectively. The heat of reaction for C + O₂ → CO₂ will be

87. Choose the S.I units for molar heat capacity among the following

88. A macroscopic property of a system which describes the initial and final state of the system is called

89. Quantity of heat evolved or absorbed during reaction measure according to

90. For a given process, the heat changes at constant pressure (q_p) and at constant volume (q_v) are related to each other as:

91. For a reaction to occur spontaneously

92. System in which there is no exchange of matter, work or energy from surroundings is

93. In thermodynamics which one of the following is not an intensive property?

94. Total energy of a system is

95. Most of the reactions which give stable products are

96. When 50 cm³ of 0.2 n H₂SO₄ is mixed with 50 cm³ of 1 N KOH, the heat liberated is

97. Sublimation, vaporization, melting and p photosynthesis all are examples of

98. When enthalpy of reactants is higher than product then reaction will be

99. Enthalpy of a reaction can be measured by

100. If coefficients of a chemical equation are doubled, the enthalpy change will

101. When a bond breaks

102. The value of ∆Hо₋н is 109 kcal mol¯¹. Then formation of one mole of water in gaseous state form H(g) and O(g) is accompanied by

103. Reaction in which heat is evolved

104. The internal energy change when a system goes form state A to B is 40 kJ.mol. If the system goes from A to B by a reversible path and returns to state A by an irreversible path what would be the net change in internal energy?

105. For the reaction NaOH + HCl → NaCl + H₂O the change in enthalpy is called

106. Total energy of a system is

107. If internal energy of the system is increased

108. ______ is the study about energy of a chemical system