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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:

Unpredictable

Equal to zero

2. Reaction in which heat is evolved

Exothermic

Endothermic

Spontaneous

Non-spontaneous

3. Which one is not state function?

Work

Gibbs free energy

Enthalpy

Internal energy

4. Two fundamental ways to transfer energy are

Heat and volume

Heat and work

Pressure and volume

Pressure and temperature

5. Total energy depends upon the state of system

Entropy of reaction

Enthalpy

Free energy of reaction

All above

6. 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

2.33 JK¯¹

Insufficient data

7. Unit of heat in S.I system is

Cal

Kcal

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

Copper calorimeter

Glass calorimeter

All above

Bomb calorimeter

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

Decrease of free energy

Increase of free energy

Decrease of entropy

Increase of enthalpy

10. Most of the thermodynamic parameters are

System

Surrounding

Phase

State function

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

Joule deg¯¹ Kg¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ atom¯¹

Joule cm¯¹ deg¯¹

12. The reaction is spontaneous if the cell potential is

Negative

Positive

Zero

Infinite

13. Calorie is equivalent to

4.184 J

0.4184 J

418.4 J

41.84 J

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

Kinetics

Thermochemistry

Thermodynamics

Photochemistry

15. 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

20 days

15 days

16. Mechanical work is especially important in systems that contain

Solid-solid

Gases

Liquid-liquid

Solid-liquid

17. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

2x – y

Y – 2x

2x – y/2

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

None of these

Water equivalent

Specific heat

Thermal capacity

19. The law of Lavoisier and Laplace illustrates

Equivalence of mechanical and thermal energy

The principle of conservation of energy

Equivalent of mechanical and chemical energy

The principle of conservation of matter

20. 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

21. Pumping of water uphill is

Irreversible process

Spontaneous process

Non spontaneous

None of these

22. 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

23. Most of the reactions which give stable products are

Exothermic

None of these

Isothermal

Endothermic

24. 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

190 KJ/mole

395 KJ/mole

-27 KJ/mole

386 KJ/mole

25. An adiabatic expansion of an ideal gas always has

Q = 0

∆H = 0

W = 0

Decrease in temperature

Page 2 of 5

26. 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 sublime

Water will freeze

Ice will melt

Water will vaporize

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

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

Any substance

System

Surrounding

State function

29. 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

Heat of neutralization

Hat of formation

Enthalpy of reaction

30. 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

2.013

20.13

2.198

31. An endothermic reaction is one in which

Heat is evolved

Heat is converted into electricity

Heat is converted into mechanical work

Heat is absorbed

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

Spontaneous

Non-spontaneous

Exothermic

Endothermic

33. 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

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

Graphite has more energy than diamond

Graphite is more stable than diamond

Both are equally stable

Stability cannot to predicated

35. All of the following are state function except

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

2 kg H₂O

1 kg H₂O

4 kg H₂O

3 kg H₂O

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

None of these

Bond strength

Bond energy

Bond length

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

Unity

Zero

Positive

Negative

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

Exothermic

Synthesis

Both a and b

Endothermic

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

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

Endothermic

Exothermic

Explosive

Photochemical

42. Hess’s law deals with

Changes in heat or reaction

Rate of reaction

Influence of pressure on volume of a gas

Equilibrium constant

43. Which type of reactions cannot occur spontaneously?

Both a and b

Neither

Exothermic

Endothermic

44. 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

573 kJ

57.3 kJ

45. Total energy of a system is

P.E, + mechanical energy

P.E. + heat energy

K.E, + heat energy

P.E, + K.E.

46. In general, for exothermic reactions to be spontaneous

Temperature should be high

Temperature has no effect

Temperature should be low

Temperature should be zero

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

Energy and volume

Temperature and volume

Temperature and pressure

Pressure and volume

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

Have the same energy as the products

Have less energy than the products

Have more energy than the products

Are at a higher temperature than the products

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

∆H = ∆E + P∆V

P∆V + nRT

∆E = q + w

Q = m x X x ∆ T

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

System

State

Surrounding

Phase

Page 3 of 5

51. Evaporation of water is

A process accompanied by chemical reaction

An exothermic change

An endothermic change

A process where no heat changes occur

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

None of these

It is reversible

It is irreversible

It is not irreversible

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

Density

Volume

Pressure

Temperature

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

+285 kJ

-285 kJ

-142.5 kJ

+142.5 kJ

55. Which one is not a state function?

Work

Enthalpy

Gibbs free energy

Internal energy

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

Thermodynamics

Chemical kinetics

Thermochemistry

Mechanics

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

Graham’s law

Boyle’s law

Henry’s law

Hess’s law

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

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

HF is more stable than HCl

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

Burning of coal is and endothermic process

Coal and air react giving a reversible reaction

Burning of coal in air releases large amount of energy

None of these

60. 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

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

Enthalpy change

Internal energy change

Free energy change

Entropy change

62. 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

63. 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

4.8 K

2.4 K

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

Not change

None of these

Be double

Be half

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

∆H = ∆E – d

∆H = ∆E + Pv

∆H = ∆E – PV

∆H = ∆E + d

66. 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

Work done is independent of its path

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

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

Charles’s law

Henry’s law

Graham’s law

Hess’s law

68. 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

+70 calories

-70 calories

70960 calories

69. In endothermic reactions, the heat content of the

Reactants is more than that of products

Products is more than that of reactants

Both a and b

Reactants and products are equal

70. 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

2.303 R

0.1 R

71. 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

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

Vibrational motion

Rotational motion

Translational motion

The sum of all motions which are possible

73. 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

Release of 218 kcal of energy

Unpredictable

Release of 109 kcal of energy

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

None of these

Watt

Joules

Calorie

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

Physical property

State function

Chemical property

Energy of the system

Page 4 of 5

76. Which of the following is not correct?

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

Neutralization is always exothermic

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

Dissolution on NH₄Cl in excess of water is an endothermic process

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

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

Born Haber cycle is different from Hess’s law

The energy change in a cyclic process is not zero

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

Exothermic

Decomposition

Both a and b

Endothermic

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

Thermochemistry

Stoichiometry

Thermodynamics

Kinetics

80. 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

= - k719

-400J

= + k319

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

Electron – volt

Calorie

Erg

Joule

82. Two fundamental ways to transfer energy are

Heat and volume

Heat and work

Pressure and volume

Pressure and temperature

83. If internal energy of the system is increased

Chemical reaction may take place

Temperature of the system may rise

Change in state of the system is increased

All

84. Total energy of a system is

P.E + K.E

K.E + heat energy

P.E + heat energy

P.E + mechanical energy

85. 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

86. When a bond breaks

Temperature increases

Heat is evolved

Heat is absorbed

No change in heat contents takes place

87. 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 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

88. A spontaneous change means

A lowering of free energy

No energy change

A lowering of energy

An increase in internal energy

89. 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 more potential energy than the reactants

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

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

Calorie

Joule

Erg

Electron vol

91. Unit of heat is SI system is

Cal

KCaL

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

Joule

Electron – volt

Erg

Calorie

93. 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

Non-spontaneous

Irreversible

Reversible

94. 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)

1.7 kJ

28.5 kJ

45.7 kJ

17.1kJ

95. 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

-88 kcal

-11 kcal

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

Thermal decomposition

Combustion

Respiration

Neutralization

97. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be negative

∆ H must be unity

∆ H must be positive

98. Endothermic changes are indicated through

All of these

Burning of carbon

Making of chemical bond

Breaking of chemical bonds

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

Closed

Adiabatic

Isolated

Isothermal

100. Enthalpy of a reaction can be measured by

Barometer

Manometer

Glass calorimeter

Thermometer

Page 5 of 5

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

Thermometer

Bomb Calorimeter

Glass Calorimeter

Monometer

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

Physical process

Chemical process

Endothermic process

Biochemical process

103. 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

300 kJ

100 kJ

150 kJ

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

Zeroth law

Second law

Third law

First law

105. If internal energy of a system is increased

All

Temperature of the system may rise

Change in state of system can occur

Chemical reaction can take place

106. 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

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

Heat of sublimation

Heat of reaction

Heat of neutralization

Heat of combustion

108. 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

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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

Chemistry

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