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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. Most of the reactions which give stable products are

Exothermic

Endothermic

Isothermal

None of these

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

Isothermal

Adiabatic

Closed

Isolated

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

Increase of free energy

Decrease of entropy

Increase of enthalpy

Decrease of free energy

4. 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

5. Calorie is equivalent to

418.4 J

41.84 J

0.4184 J

4.184 J

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

Thermodynamics

Stoichiometry

Kinetics

Thermochemistry

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

-285 kJ

-142.5 kJ

+142.5 kJ

+285 kJ

8. A spontaneous change means

No energy change

A lowering of free energy

A lowering of energy

An increase in internal energy

9. If internal energy of a system is increased

Change in state of system can occur

Chemical reaction can take place

All

Temperature of the system may rise

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

Calorie

Electron – volt

Erg

Joule

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

It is reversible

None of these

It is not irreversible

It is irreversible

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

The energy change in a cyclic process is not zero

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

The lattice energy of the crystalline substances can be calculated easily

13. Which one is not state function?

Enthalpy

Work

Internal energy

Gibbs free energy

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

Joule

Electron vol

Erg

Calorie

15. The enthalpy of formation of carbon monoxide will be

2x – y/2

Y – 2x

Y – 2x/2

2x – y

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

573 kJ

57.3 kJ

11.46 kJ

573 J

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

Thermometer

Monometer

Glass Calorimeter

Bomb Calorimeter

18. In general, for exothermic reactions to be spontaneous

Temperature should be high

Temperature should be low

Temperature should be zero

Temperature has no effect

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

It has a large – ve value for the entropy change

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

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

HF and HCl are endothermic compounds

HCl is more stable than HF

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

HF is more stable than HCl

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

Graham’s law

Hess’s law

Charles’s law

Henry’s law

22. Enthalpy of a reaction can be measured by

Manometer

Glass calorimeter

Barometer

Thermometer

23. 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)

45.7 kJ

28.5 kJ

1.7 kJ

17.1kJ

24. 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)

20 days

50 days

32 days

15 days

25. 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

Water will vaporize

Ice will melt

Ice will sublime

Water will freeze

Page 2 of 5

26. If internal energy of the system is increased

Change in state of the system is increased

Chemical reaction may take place

Temperature of the system may rise

All

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

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

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

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

Work done is independent of its path

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

Have more energy than the products

Have the same energy as the products

Are at a higher temperature than the products

Have less energy than the products

29. 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

395 KJ/mole

-27 KJ/mole

386 KJ/mole

190 KJ/mole

30. Evaporation of water is

A process where no heat changes occur

An endothermic change

An exothermic change

A process accompanied by chemical reaction

31. 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

110.5 kJ

-110.5 kJ

676.5 kJ

-676.5 kJ

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

Third law

First law

Zeroth law

Second law

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

Rotational motion

The sum of all motions which are possible

Vibrational motion

Translational motion

34. An adiabatic expansion of an ideal gas always has

W = 0

Decrease in temperature

∆H = 0

Q = 0

35. Hess’s law deals with

Rate of reaction

Equilibrium constant

Changes in heat or reaction

Influence of pressure on volume of a gas

36. Endothermic changes are indicated through

Burning of carbon

Breaking of chemical bonds

All of these

Making of chemical bond

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

Endothermic

Both a and b

Exothermic

Decomposition

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

Surrounding

State

Phase

System

39. All of the following are state function except

40. 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

Absorption of 218 kcal of energy

Unpredictable

Release of 218 kcal of energy

Release of 109 kcal of energy

41. 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

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

Endothermic

Exothermic

Non-spontaneous

Spontaneous

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

Copper calorimeter

Glass calorimeter

Bomb calorimeter

All above

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

Water equivalent

None of these

Specific heat

Thermal capacity

45. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

57.3 kJ

2 x 57.3 kJ

57.3/2 kJ

Cannot be predicted

46. 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

Insufficient data

9.75 JK¯¹

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

Hat of formation

Heat of combustion

Heat of neutralization

Enthalpy of reaction

48. Unit of heat in S.I system is

Kcal

Cal

49. Which statement describes characteristics of an endothermic reaction?

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

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

The sign of H is positive, 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

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

Coal and air react giving a reversible reaction

None of these

Burning of coal in air releases large amount of energy

Burning of coal is and endothermic process

Page 3 of 5

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

Physical process

Chemical process

Biochemical process

Endothermic process

52. Free energy change for a reversible process is:

Unpredictable

Equal to zero

53. 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

-125 kJ

+250 kJ

+125 kJ

-250 kJ

54. Two fundamental ways to transfer energy are

Pressure and volume

Heat and work

Heat and volume

Pressure and temperature

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

3 kg H₂O

2 kg H₂O

1 kg H₂O

4 kg H₂O

56. In endothermic reactions, the heat content of the

Products is more than that of reactants

Reactants and products are equal

Reactants is more than that of products

Both a and b

57. 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

Irreversible

Reversible

Spontaneous

Non-spontaneous

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

Both a and b

Exothermic

Synthesis

Endothermic

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

Density

Volume

Temperature

Pressure

60. Pumping of water uphill is

None of these

Non spontaneous

Irreversible process

Spontaneous process

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

Calorie

Electron – volt

Erg

Joule

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

Enthalpy change

Internal energy change

Entropy change

Free energy change

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

∆H = ∆E + d

∆H = ∆E + Pv

∆H = ∆E – PV

∆H = ∆E – d

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

Photochemical

Explosive

Endothermic

Exothermic

65. 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

100 kJ

50 kJ

150 kJ

300 kJ

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

Respiration

Combustion

Thermal decomposition

Neutralization

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

Q = m x X x ∆ T

∆E = q + w

P∆V + nRT

∆H = ∆E + P∆V

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

Photochemistry

Thermodynamics

Kinetics

Thermochemistry

69. Mechanical work is especially important in systems that contain

Gases

Liquid-liquid

Solid-solid

Solid-liquid

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

None of these

Calorie

Watt

Joules

71. Unit of heat is SI system is

KCaL

Cal

72. The law of Lavoisier and Laplace illustrates

The principle of conservation of energy

Equivalent of mechanical and chemical energy

Equivalence of mechanical and thermal energy

The principle of conservation of matter

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

Positive

Zero

Negative

Unity

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

Henry’s law

Boyle’s law

Hess’s law

Graham’s law

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

Spontaneous

Non-spontaneous

Endothermic

Exothermic

Page 4 of 5

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

Not change

None of these

Be double

Be half

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

Heat of combustion

Heat of reaction

Heat of sublimation

Heat of neutralization

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

Physical property

Chemical property

State function

Energy of the system

79. Most of the thermodynamic parameters are

Surrounding

System

Phase

State function

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

10.0 R

100.0 R

0.1 R

2.303 R

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

Thermochemistry

Chemical kinetics

Mechanics

Thermodynamics

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

+21.4 kcal mol¯¹

-94.0 kcal mol¯¹

-231.6 kcal mol¯¹

+64.8 kcal mol¯¹

83. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be positive

∆ H must be negative

∆ H must be unity

84. Total energy of a system is

K.E + heat energy

P.E + K.E

P.E + mechanical energy

P.E + heat energy

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

Joule deg¯¹ atom¯¹

Joule deg¯¹ mol¯¹

Joule cm¯¹ deg¯¹

Joule deg¯¹ Kg¯¹

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

Temperature and volume

Pressure and volume

Energy and volume

Temperature and pressure

87. When a bond breaks

No change in heat contents takes place

Temperature increases

Heat is absorbed

Heat is evolved

88. 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

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

Decreases

Remains constant

Remains same

Increases

90. 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

-339.3 kJ mol¯¹

-523.3 kJ mol¯¹

-439.3 kJ mol¯¹

-221.1 kJ mol¯¹

91. 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?

-70 calories

+70 calories

71030 calories

70960 calories

92. Total energy of a system is

P.E. + heat energy

K.E, + heat energy

P.E, + K.E.

P.E, + mechanical energy

93. Which type of reactions cannot occur spontaneously?

Both a and b

Exothermic

Endothermic

Neither

94. Total energy depends upon the state of system

Free energy of reaction

All above

Enthalpy

Entropy of reaction

95. Reaction in which heat is evolved

Endothermic

Non-spontaneous

Spontaneous

Exothermic

96. 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

-88 kcal

-11 kcal

-44 kcal

-22 kcal

97. 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)

2.013

2.198

20.13

21.98

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

None of these

Bond strength

Bond length

Bond energy

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

Both are equally stable

Graphite is more stable than diamond

Graphite has more energy than diamond

Stability cannot to predicated

100. Two fundamental ways to transfer energy are

Heat and volume

Pressure and temperature

Heat and work

Pressure and volume

Page 5 of 5

101. 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

1.2 K

4.8 K

6.6 K

2.4 K

102. An endothermic reaction is one in which

Heat is absorbed

Heat is converted into mechanical work

Heat is evolved

Heat is converted into electricity

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

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?

40 kJ

> 40 kJ

< 40 kJ

Zero

105. 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

= + k319

-400J

= - k719

0 J

106. Which one is not a state function?

Internal energy

Enthalpy

Work

Gibbs free energy

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

State function

Any substance

System

Surrounding

108. The reaction is spontaneous if the cell potential is

Zero

Infinite

Positive

Negative

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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

Chemistry

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Chemistry Thermochemistry MCQS Online Test

ECAT Chemistry Thermochemistry Chapter Online Test

ECAT Chemistry Thermochemistry Test

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