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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. 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

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

Calorie

Joule

Erg

Electron – volt

3. When a bond breaks

Heat is evolved

Heat is absorbed

Temperature increases

No change in heat contents takes place

4. Which of the following is not correct?

Dissolution on NH₄Cl in excess of water is an endothermic process

Neutralization is always exothermic

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

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

5. Reaction in which heat is evolved

Endothermic

Non-spontaneous

Spontaneous

Exothermic

6. 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

-22 kcal

-11 kcal

-44 kcal

7. In general, for exothermic reactions to be spontaneous

Temperature has no effect

Temperature should be high

Temperature should be zero

Temperature should be low

8. 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 218 kcal of energy

Absorption of 218 kcal of energy

Release of 109 kcal of energy

Unpredictable

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

Watt

Calorie

Joules

None of these

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

Increases

Remains constant

Decreases

Remains same

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

Bond energy

Bond strength

Bond length

None of these

12. If internal energy of the system is increased

All

Change in state of the system is increased

Chemical reaction may take place

Temperature of the system may rise

13. 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

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

∆H = ∆E + d

∆H = ∆E – d

∆H = ∆E + Pv

∆H = ∆E – PV

15. 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

2.4 K

6.6 K

1.2 K

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

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

Work done is independent of its path

17. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and volume

Pressure and temperature

18. If internal energy of a system is increased

All

Temperature of the system may rise

Chemical reaction can take place

Change in state of system can occur

19. 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

20. Which one is not a state function?

Enthalpy

Work

Internal energy

Gibbs free energy

21. The law of Lavoisier and Laplace illustrates

Equivalent of mechanical and chemical energy

The principle of conservation of matter

The principle of conservation of energy

Equivalence of mechanical and thermal energy

22. Which type of reactions cannot occur spontaneously?

Exothermic

Endothermic

Neither

Both a and b

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

Rotational motion

Translational motion

Vibrational motion

The sum of all motions which are possible

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

Joule deg¯¹ atom¯¹

Joule deg¯¹ Kg¯¹

Joule deg¯¹ mol¯¹

Joule cm¯¹ deg¯¹

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

State

System

Phase

Surrounding

Page 2 of 5

26. Total energy of a system is

P.E + K.E

P.E + mechanical energy

P.E + heat energy

K.E + heat energy

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

Exothermic

Synthesis

Both a and b

Endothermic

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

Endothermic process

Physical process

Chemical process

Biochemical process

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

30. Unit of heat is SI system is

Cal

KCaL

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

Electron – volt

Erg

Joule

Calorie

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

Stability cannot to predicated

Both are equally stable

Graphite has more energy than diamond

Graphite is more stable than diamond

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

Mechanics

Thermodynamics

Chemical kinetics

Thermochemistry

34. 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

0 J

-400J

= - k719

= + k319

35. 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 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

36. The reaction is spontaneous if the cell potential is

Infinite

Negative

Positive

Zero

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

None of these

Thermal capacity

Specific heat

Water equivalent

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

1 kg H₂O

2 kg H₂O

4 kg H₂O

3 kg H₂O

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

Thermodynamics

Stoichiometry

Thermochemistry

Kinetics

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

Both a and b

Endothermic

Decomposition

Exothermic

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

State function

Energy of the system

Chemical property

Physical property

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

Density

Temperature

Volume

Pressure

43. 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

None of these

Burning of coal is and endothermic process

44. 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 less energy than the products

Have more energy than the products

45. Free energy change for a reversible process is:

Unpredictable

Equal to zero

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

Negative

Unity

Zero

Positive

47. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

Y – 2x

2x – y

2x – y/2

48. 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

49. A spontaneous change means

No energy change

A lowering of free energy

An increase in internal energy

A lowering of energy

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

Heat of sublimation

Heat of reaction

Heat of combustion

Heat of neutralization

Page 3 of 5

51. In endothermic reactions, the heat content of the

Reactants and products are equal

Products is more than that of reactants

Reactants is more than that of products

Both a and b

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

53. 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

54. An endothermic reaction is one in which

Heat is evolved

Heat is absorbed

Heat is converted into electricity

Heat is converted into mechanical work

55. 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

56. Endothermic changes are indicated through

Burning of carbon

Breaking of chemical bonds

All of these

Making of chemical bond

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

100.0 R

0.1 R

2.303 R

10.0 R

58. 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

59. Mechanical work is especially important in systems that contain

Solid-solid

Gases

Solid-liquid

Liquid-liquid

60. Enthalpy of a reaction can be measured by

Thermometer

Glass calorimeter

Barometer

Manometer

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

Henry’s law

Graham’s law

Hess’s law

Charles’s law

62. Pumping of water uphill is

Spontaneous process

Non spontaneous

Irreversible process

None of these

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

Kinetics

Thermochemistry

Thermodynamics

Photochemistry

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

Enthalpy change

Internal energy change

Free energy change

Entropy change

65. Total energy depends upon the state of system

Free energy of reaction

Entropy of reaction

All above

Enthalpy

66. 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

67. Unit of heat in S.I system is

Cal

Kcal

68. 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

2.33 JK¯¹

Insufficient data

11.272 JK¯¹

9.75 JK¯¹

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

It has small + ve value for enthalpy change

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 a large + ve value for enthalpy change

70. 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 vaporize

Water will freeze

71. 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

-221.1 kJ mol¯¹

-339.3 kJ mol¯¹

-439.3 kJ mol¯¹

72. Evaporation of water is

An endothermic change

A process where no heat changes occur

A process accompanied by chemical reaction

An exothermic change

73. Total energy of a system is

P.E, + mechanical energy

P.E, + K.E.

K.E, + heat energy

P.E. + heat energy

74. 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

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

Non-spontaneous

Endothermic

Spontaneous

Exothermic

Page 4 of 5

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

Monometer

Thermometer

Bomb Calorimeter

Glass Calorimeter

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

Temperature and volume

Temperature and pressure

Pressure and volume

Energy and volume

78. 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

-110.5 kJ

-676.5 kJ

110.5 kJ

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

Electron vol

Joule

Erg

Calorie

80. Calorie is equivalent to

41.84 J

4.184 J

418.4 J

0.4184 J

81. Two fundamental ways to transfer energy are

Pressure and volume

Pressure and temperature

Heat and volume

Heat and work

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

Exothermic

Explosive

Endothermic

Photochemical

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

Thermal decomposition

Respiration

Neutralization

Combustion

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

Not change

Be double

None of these

Be half

85. Most of the thermodynamic parameters are

Surrounding

State function

System

Phase

86. An adiabatic expansion of an ideal gas always has

∆H = 0

Decrease in temperature

Q = 0

W = 0

87. Which one is not state function?

Enthalpy

Gibbs free energy

Internal energy

Work

88. All of the following are state function except

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

573 J

11.46 kJ

57.3 kJ

573 kJ

90. Hess’s law deals with

Equilibrium constant

Changes in heat or reaction

Influence of pressure on volume of a gas

Rate of reaction

91. For a reaction to occur spontaneously

∆ H must be positive

∆ H must be negative

∆ H must be zero

∆ H must be unity

92. 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)

32 days

50 days

15 days

20 days

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

Zeroth law

First law

Second law

Third law

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

Glass calorimeter

Bomb calorimeter

Copper calorimeter

All above

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

Adiabatic

Closed

Isolated

Isothermal

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 combustion

Enthalpy of reaction

Heat of neutralization

Hat of formation

97. 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

1.7 kJ

17.1kJ

28.5 kJ

98. 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

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

It is reversible

It is not irreversible

It is irreversible

None of these

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

Any substance

System

Surrounding

State function

Page 5 of 5

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

Born Haber cycle is different from Hess’s law

The energy change in a cyclic process is not zero

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

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

HF is more stable than HCl

HCl is more stable than HF

HF and HCl are endothermic compounds

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

103. 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

Zero

> 40 kJ

104. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

57.3/2 kJ

57.3 kJ

2 x 57.3 kJ

Cannot be predicted

105. 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

386 KJ/mole

-27 KJ/mole

190 KJ/mole

106. Most of the reactions which give stable products are

Endothermic

None of these

Exothermic

Isothermal

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

P∆V + nRT

Q = m x X x ∆ T

∆E = q + w

∆H = ∆E + P∆V

108. 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)

21.98

20.13

2.198

2.013

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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

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