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ECAT Chemistry Thermochemistry Online Test

Maan AliLast Updated: April 19, 2025

Chemistry Thermochemistry MCQS Online Test

ECAT Chemistry Thermochemistry Chapter Online Test

Total Questions:	108
Time Allowed:	60 Minutes
Total Marks:	108
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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ECAT Chemistry Thermochemistry Test

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Page 1 of 5

Chemistry

1. Which one is not state function?

Gibbs free energy

Internal energy

Work

Enthalpy

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

It has a + ve value for the entropy change and a – ve value for the enthalpy change

It has small + ve value for enthalpy change

It has a large + ve value for enthalpy change

It has a large – ve value for the entropy change

3. 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

Ice will melt

Ice will sublime

Water will freeze

Water will vaporize

4. Most of the reactions which give stable products are

Exothermic

Isothermal

None of these

Endothermic

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

The affinity of fluorine to hydrogen is greater than the affinity of chlorine to hydrogen

HF and HCl are endothermic compounds

HCl is more stable than HF

HF is more stable than HCl

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

Henry’s law

Hess’s law

Graham’s law

Charles’s law

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

Respiration

Thermal decomposition

Combustion

Neutralization

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

Physical property

Chemical property

Energy of the system

State function

9. The law of Lavoisier and Laplace illustrates

The principle of conservation of matter

Equivalent of mechanical and chemical energy

Equivalence of mechanical and thermal energy

The principle of conservation of energy

10. 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

386 KJ/mole

190 KJ/mole

-27 KJ/mole

395 KJ/mole

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

-142.5 kJ

+285 kJ

-285 kJ

+142.5 kJ

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

– 68 + 48 – 14

68 + 48 + 14

68 – 48 + 14

– 68 – 48 + 14

13. 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

4.8 K

1.2 K

6.6 K

2.4 K

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

Bond length

Bond energy

None of these

Bond strength

15. Reaction in which heat is evolved

Non-spontaneous

Endothermic

Spontaneous

Exothermic

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

The energy change in a cyclic process is not zero

The lattice energy of the crystalline substances can be calculated easily

Born Haber cycle is different from Hess’s law

Heat of formation of the product and lattice energy of the substance can be calculated simultaneously

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

Pressure and volume

Temperature and volume

Energy and volume

Temperature and pressure

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

Photochemistry

Kinetics

Thermodynamics

Thermochemistry

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

Second law

Zeroth law

First law

Third law

20. Unit of heat in S.I system is

Cal

Kcal

21. 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

+250 kJ

-125 kJ

+125 kJ

-250 kJ

22. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and temperature

Pressure and volume

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

Kinetics

Stoichiometry

Thermodynamics

Thermochemistry

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

Boyle’s law

Hess’s law

Graham’s law

Henry’s law

25. 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)

15 days

50 days

20 days

32 days

Page 2 of 5

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

57.3 kJ

573 kJ

573 J

11.46 kJ

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

Calorie

Joule

Electron – volt

Erg

28. Total energy of a system is

K.E, + heat energy

P.E. + heat energy

P.E, + K.E.

P.E, + mechanical energy

29. Hess’s law deals with

Changes in heat or reaction

Rate of reaction

Influence of pressure on volume of a gas

Equilibrium constant

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

Decrease of free energy

Increase of free energy

Increase of enthalpy

Decrease of entropy

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

It is reversible

It is irreversible

It is not irreversible

None of these

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

0.1 R

2.303 R

100.0 R

10.0 R

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

Exothermic

Both a and b

Endothermic

Synthesis

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

None of these

Water equivalent

Thermal capacity

Specific heat

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

Calorie

Electron – volt

Joule

Erg

36. In endothermic reactions, the heat content of the

Products is more than that of reactants

Reactants is more than that of products

Reactants and products are equal

Both a and b

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

Work done is independent of its path

An equivalent amount of heat energy can neither be created nor destroyed

Continuous production of mechanical work without supplying an equivalent amount of heat energy

One form of energy can be transferred to an equivalent amount of the kind of energy

38. Calorie is equivalent to

418.4 J

41.84 J

0.4184 J

4.184 J

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

Bomb calorimeter

Glass calorimeter

Copper calorimeter

All above

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

Isolated

Isothermal

Closed

Adiabatic

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

Explosive

Exothermic

Photochemical

Endothermic

42. If internal energy of the system is increased

Temperature of the system may rise

Change in state of the system is increased

All

Chemical reaction may take place

43. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

2 x 57.3 kJ

Cannot be predicted

57.3/2 kJ

57.3 kJ

44. 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?

71030 calories

70960 calories

+70 calories

-70 calories

45. 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

-22 kcal

-44 kcal

-88 kcal

-11 kcal

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

Positive

Zero

Negative

Unity

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

Burning of coal in air releases large amount of energy

None of these

Coal and air react giving a reversible reaction

Burning of coal is and endothermic process

48. 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

676.5 kJ

-676.5 kJ

-110.5 kJ

110.5 kJ

49. All of the following are state function except

50. Total energy depends upon the state of system

Entropy of reaction

Enthalpy

Free energy of reaction

All above

Page 3 of 5

51. An adiabatic expansion of an ideal gas always has

∆H = 0

Q = 0

W = 0

Decrease in temperature

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

Remains constant

Remains same

Decreases

Increases

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

Bomb Calorimeter

Thermometer

Monometer

Glass Calorimeter

54. Two fundamental ways to transfer energy are

Heat and volume

Pressure and temperature

Heat and work

Pressure and volume

55. The reaction is spontaneous if the cell potential is

Infinite

Positive

Zero

Negative

56. Which type of reactions cannot occur spontaneously?

Both a and b

Neither

Endothermic

Exothermic

57. If internal energy of a system is increased

Temperature of the system may rise

All

Change in state of system can occur

Chemical reaction can take place

58. Endothermic changes are indicated through

Breaking of chemical bonds

Making of chemical bond

Burning of carbon

All of these

59. Evaporation of water is

An exothermic change

A process accompanied by chemical reaction

A process where no heat changes occur

An endothermic change

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

Joule cm¯¹ deg¯¹

Joule deg¯¹ Kg¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ atom¯¹

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

The sum of all motions which are possible

Vibrational motion

Rotational motion

Translational motion

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

Surrounding

System

Any substance

State function

63. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

2x – y/2

2x – y

Y – 2x

64. Which of the following is not correct?

Dissolution on NH₄Cl in excess of water is an endothermic process

The heat of reaction at constant volume is denoted by ∆E.

The absolute value of enthalpy (H) can be determined experimentally

Neutralization is always exothermic

65. Which statement describes characteristics of an endothermic reaction?

The sign of H is positive and the products a have more potential energy than the reactant

The sign of H is negative, and the products have less potential energy than the reactants

The sign of H is negative, and the products have more potential energy than the reactants

The sign of H is positive, and the products have less potential energy than the reactants

66. 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

50 kJ

150 kJ

100 kJ

300 kJ

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

∆H = ∆E + Pv

∆H = ∆E – PV

∆H = ∆E + d

∆H = ∆E – d

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

+64.8 kcal mol¯¹

+21.4 kcal mol¯¹

-94.0 kcal mol¯¹

-231.6 kcal mol¯¹

69. Pumping of water uphill is

Non spontaneous

Spontaneous process

Irreversible process

None of these

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

Have the same energy as the products

Are at a higher temperature than the products

Have less energy than the products

Have more energy than the products

71. An endothermic reaction is one in which

Heat is converted into electricity

Heat is converted into mechanical work

Heat is evolved

Heat is absorbed

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

Heat of neutralization

Heat of reaction

Heat of sublimation

Heat of combustion

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

Graphite is more stable than diamond

Stability cannot to predicated

Both are equally stable

Graphite has more energy than diamond

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

Internal energy change

Entropy change

Enthalpy change

Free energy change

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

3 kg H₂O

1 kg H₂O

2 kg H₂O

4 kg H₂O

Page 4 of 5

76. A spontaneous change means

No energy change

An increase in internal energy

A lowering of free energy

A lowering of energy

77. Most of the thermodynamic parameters are

Phase

System

State function

Surrounding

78. 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

= - k719

0 J

= + k319

-400J

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

P∆V + nRT

Q = m x X x ∆ T

∆H = ∆E + P∆V

∆E = q + w

80. 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

Unpredictable

Release of 218 kcal of energy

Release of 109 kcal of energy

Absorption of 218 kcal of energy

81. Mechanical work is especially important in systems that contain

Solid-solid

Solid-liquid

Liquid-liquid

Gases

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

Phase

State

Surrounding

System

83. Enthalpy of a reaction can be measured by

Manometer

Glass calorimeter

Barometer

Thermometer

84. 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)

2.198

21.98

20.13

2.013

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

Endothermic process

Biochemical process

Physical process

Chemical process

86. Total energy of a system is

P.E + K.E

K.E + heat energy

P.E + heat energy

P.E + mechanical energy

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

Joules

Watt

None of these

Calorie

88. When a bond breaks

Heat is absorbed

Temperature increases

Heat is evolved

No change in heat contents takes place

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

Non-spontaneous

Spontaneous

Exothermic

Endothermic

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

Be double

None of these

Be half

Not change

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

Temperature

Pressure

Density

Volume

92. In general, for exothermic reactions to be spontaneous

Temperature has no effect

Temperature should be low

Temperature should be high

Temperature should be zero

93. 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)

17.1kJ

28.5 kJ

45.7 kJ

1.7 kJ

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

Joule

Electron vol

Calorie

Erg

95. For a reaction to occur spontaneously

∆ H must be positive

∆ H must be negative

∆ H must be zero

∆ H must be unity

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

Heat of neutralization

Hat of formation

Enthalpy of reaction

Heat of combustion

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

Endothermic

Both a and b

Decomposition

Exothermic

98. 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

Spontaneous

Irreversible

Non-spontaneous

Reversible

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

100. 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

-523.3 kJ mol¯¹

-439.3 kJ mol¯¹

-339.3 kJ mol¯¹

-221.1 kJ mol¯¹

Page 5 of 5

101. 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?

< 40 kJ

Zero

40 kJ

> 40 kJ

102. 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

11.272 JK¯¹

2.33 JK¯¹

9.75 JK¯¹

Insufficient data

103. Free energy change for a reversible process is:

Unpredictable

Equal to zero

104. Which one is not a state function?

Internal energy

Gibbs free energy

Work

Enthalpy

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

Spontaneous

Exothermic

Endothermic

Non-spontaneous

106. 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

-112 kJ mol¯¹

-668 kJ mol¯¹

112 kJ mol¯¹

668 kJ mol¯¹

107. Unit of heat is SI system is

Cal

KCaL

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

Thermodynamics

Mechanics

Thermochemistry

Chemical kinetics

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Maan AliLast Updated: April 19, 2025

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ECAT Chemistry Thermochemistry Online Test

Chemistry Thermochemistry MCQS Online Test

ECAT Chemistry Thermochemistry Chapter Online Test

ECAT Chemistry Thermochemistry Test

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