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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. Free energy change for a reversible process is:

Equal to zero

Unpredictable

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

Stability cannot to predicated

Graphite is more stable than diamond

Graphite has more energy than diamond

Both are equally stable

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

Decomposition

Exothermic

Both a and b

Endothermic

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

Exothermic

Endothermic

Spontaneous

Non-spontaneous

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

Are at a higher temperature than the products

Have the same energy as the products

Have more energy than the products

Have less energy than the products

6. Reaction in which heat is evolved

Spontaneous

Endothermic

Non-spontaneous

Exothermic

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

State function

Chemical property

Physical property

Energy of the system

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

System

Any substance

State function

Surrounding

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

Glass Calorimeter

Monometer

Thermometer

Bomb Calorimeter

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

Heat of reaction

Heat of neutralization

Heat of sublimation

Heat of combustion

11. 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

676.5 kJ

-676.5 kJ

-110.5 kJ

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

The lattice energy of the crystalline substances can be calculated easily

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

13. Which statement describes characteristics of an endothermic reaction?

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

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

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

Free energy change

Entropy change

Internal energy change

Enthalpy change

15. Two fundamental ways to transfer energy are

Pressure and volume

Pressure and temperature

Heat and volume

Heat and work

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

17. 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

-221.1 kJ mol¯¹

-439.3 kJ mol¯¹

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

1 kg H₂O

3 kg H₂O

4 kg H₂O

2 kg H₂O

19. Which type of reactions cannot occur spontaneously?

Both a and b

Neither

Exothermic

Endothermic

20. Most of the thermodynamic parameters are

System

Surrounding

Phase

State function

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

Calorie

None of these

Joules

Watt

22. Evaporation of water is

A process where no heat changes occur

An exothermic change

A process accompanied by chemical reaction

An endothermic change

23. 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

24. All of the following are state function except

25. 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

21.98

20.13

2.198

Page 2 of 5

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

Bond length

None of these

Bond energy

Bond strength

27. 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

9.75 JK¯¹

11.272 JK¯¹

Insufficient data

2.33 JK¯¹

28. 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

Release of 109 kcal of energy

Release of 218 kcal of energy

Absorption of 218 kcal of energy

Unpredictable

29. 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

30. Enthalpy of a reaction can be measured by

Manometer

Glass calorimeter

Thermometer

Barometer

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

Increase of enthalpy

Increase of free energy

Decrease of free energy

Decrease of entropy

32. 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

-44 kcal

-22 kcal

-11 kcal

-88 kcal

33. 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

1.7 kJ

45.7 kJ

28.5 kJ

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

Remains constant

Decreases

Increases

Remains same

35. The reaction is spontaneous if the cell potential is

Positive

Infinite

Negative

Zero

36. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and volume

Pressure and temperature

37. An endothermic reaction is one in which

Heat is converted into electricity

Heat is converted into mechanical work

Heat is absorbed

Heat is evolved

38. 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

39. 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

32 days

15 days

50 days

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

Biochemical process

Endothermic process

Chemical process

Physical process

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

Temperature

Pressure

Volume

Density

42. Total energy of a system is

P.E + heat energy

P.E + K.E

P.E + mechanical energy

K.E + heat energy

43. Hess’s law deals with

Rate of reaction

Equilibrium constant

Changes in heat or reaction

Influence of pressure on volume of a gas

44. Which of the following is not correct?

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

Neutralization is always exothermic

Dissolution on NH₄Cl in excess of water is an endothermic process

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

45. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

2x – y

2x – y/2

Y – 2x

46. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Cannot be predicted

57.3/2 kJ

2 x 57.3 kJ

57.3 kJ

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

Specific heat

None of these

Water equivalent

Thermal capacity

48. 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

-112 kJ mol¯¹

-668 kJ mol¯¹

668 kJ mol¯¹

49. An adiabatic expansion of an ideal gas always has

∆H = 0

Q = 0

W = 0

Decrease in temperature

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

Isothermal

Isolated

Adiabatic

Closed

Page 3 of 5

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

Mechanics

Thermodynamics

Chemical kinetics

Thermochemistry

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

Erg

Electron – volt

Calorie

Joule

53. 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

71030 calories

-70 calories

70960 calories

54. 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

Reversible

Non-spontaneous

Irreversible

Spontaneous

55. Unit of heat is SI system is

Cal

KCaL

56. A spontaneous change means

An increase in internal energy

No energy change

A lowering of free energy

A lowering of energy

57. Calorie is equivalent to

418.4 J

41.84 J

0.4184 J

4.184 J

58. Pumping of water uphill is

Non spontaneous

None of these

Irreversible process

Spontaneous process

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

None of these

It is irreversible

It is not irreversible

It is reversible

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

All above

Glass calorimeter

Copper calorimeter

Bomb calorimeter

61. If internal energy of a system is increased

Chemical reaction can take place

Change in state of system can occur

Temperature of the system may rise

All

62. 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

395 KJ/mole

-27 KJ/mole

190 KJ/mole

63. 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

Coal and air react giving a reversible reaction

Burning of coal is and endothermic process

None of these

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

Hess’s law

Henry’s law

Graham’s law

Charles’s law

65. 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

Enthalpy of reaction

Heat of neutralization

66. 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

67. Endothermic changes are indicated through

Burning of carbon

All of these

Breaking of chemical bonds

Making of chemical bond

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

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

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

Work done is independent of its path

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

69. 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

70. 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

71. 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

Water will vaporize

Water will freeze

Ice will sublime

72. Which one is not state function?

Work

Internal energy

Enthalpy

Gibbs free energy

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

Spontaneous

Exothermic

Endothermic

Non-spontaneous

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

Zero

Negative

Unity

Positive

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

Electron – volt

Calorie

Erg

Joule

Page 4 of 5

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

0.1 R

100.0 R

10.0 R

2.303 R

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

Endothermic

Both a and b

Synthesis

Exothermic

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

Explosive

Endothermic

Photochemical

Exothermic

79. If internal energy of the system is increased

Change in state of the system is increased

All

Temperature of the system may rise

Chemical reaction may take place

80. When a bond breaks

Heat is evolved

Temperature increases

Heat is absorbed

No change in heat contents takes place

81. The law of Lavoisier and Laplace illustrates

Equivalence of mechanical and thermal energy

The principle of conservation of matter

Equivalent of mechanical and chemical energy

The principle of conservation of energy

82. Most of the reactions which give stable products are

Exothermic

Isothermal

Endothermic

None of these

83. 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

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

11.46 kJ

573 kJ

573 J

57.3 kJ

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

Thermodynamics

Photochemistry

Thermochemistry

Kinetics

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

+64.8 kcal mol¯¹

+21.4 kcal mol¯¹

-231.6 kcal mol¯¹

-94.0 kcal mol¯¹

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

Erg

Calorie

Electron vol

Joule

88. In general, for exothermic reactions to be spontaneous

Temperature should be zero

Temperature should be high

Temperature should be low

Temperature has no effect

89. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be positive

∆ H must be negative

∆ H must be unity

90. 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

150 kJ

50 kJ

300 kJ

91. Total energy depends upon the state of system

Entropy of reaction

Enthalpy

All above

Free energy of reaction

92. Unit of heat in S.I system is

Cal

Kcal

93. Mechanical work is especially important in systems that contain

Gases

Solid-liquid

Solid-solid

Liquid-liquid

94. In endothermic reactions, the heat content of the

Both a and b

Products is more than that of reactants

Reactants is more than that of products

Reactants and products are equal

95. Which one is not a state function?

Work

Gibbs free energy

Internal energy

Enthalpy

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

Translational motion

Vibrational motion

The sum of all motions which are possible

Rotational motion

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

∆H = ∆E + Pv

∆H = ∆E – d

∆H = ∆E + d

∆H = ∆E – PV

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

Thermodynamics

Thermochemistry

Kinetics

Stoichiometry

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

Energy and volume

Temperature and volume

Temperature and pressure

Pressure and volume

100. 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

6.6 K

1.2 K

2.4 K

4.8 K

Page 5 of 5

101. Total energy of a system is

K.E, + heat energy

P.E. + heat energy

P.E, + mechanical energy

P.E, + K.E.

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

Thermal decomposition

Combustion

Neutralization

Respiration

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

Be half

Be double

Not change

None of these

104. 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

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

HF is more stable than HCl

HCl is more stable than HF

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

State

System

Surrounding

Phase

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

Graham’s law

Hess’s law

Henry’s law

Boyle’s law

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

Joule deg¯¹ mol¯¹

Joule cm¯¹ deg¯¹

Joule deg¯¹ atom¯¹

Joule deg¯¹ Kg¯¹

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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

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