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

Thermal capacity

None of these

Specific heat

Water equivalent

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

2 x 57.3 kJ

57.3 kJ

57.3/2 kJ

Cannot be predicted

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

Thermodynamics

Mechanics

Chemical kinetics

Thermochemistry

4. 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

Spontaneous

Irreversible

Non-spontaneous

5. When a bond breaks

Heat is evolved

Temperature increases

No change in heat contents takes place

Heat is absorbed

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

Glass calorimeter

Copper calorimeter

Bomb calorimeter

All above

7. 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

-110.5 kJ

-676.5 kJ

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

Work done is independent of its path

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

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

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

Third law

Second law

Zeroth law

First law

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

Both a and b

Decomposition

Exothermic

Endothermic

11. 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 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 a have more potential energy than the reactant

12. Unit of heat in S.I system is

Cal

Kcal

13. If internal energy of a system is increased

All

Change in state of system can occur

Temperature of the system may rise

Chemical reaction can take place

14. Which one is not a state function?

Internal energy

Work

Enthalpy

Gibbs free energy

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

Have less energy than the products

Are at a higher temperature than the products

Have the same energy as the products

Have more energy than the products

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

Decreases

Remains same

Remains constant

Increases

17. 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

Insufficient data

11.272 JK¯¹

2.33 JK¯¹

9.75 JK¯¹

18. 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 109 kcal of energy

Release of 218 kcal of energy

Absorption of 218 kcal of energy

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

System

Phase

Surrounding

State

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

2.303 R

10.0 R

0.1 R

100.0 R

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

Non-spontaneous

Endothermic

Spontaneous

Exothermic

22. Free energy change for a reversible process is:

Equal to zero

Unpredictable

23. 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

150 kJ

100 kJ

300 kJ

50 kJ

24. Enthalpy of a reaction can be measured by

Thermometer

Barometer

Manometer

Glass calorimeter

25. Total energy depends upon the state of system

Free energy of reaction

Entropy of reaction

Enthalpy

All above

Page 2 of 5

26. 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

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

∆E = q + w

P∆V + nRT

∆H = ∆E + P∆V

Q = m x X x ∆ T

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

Joule

Calorie

Erg

Electron – volt

29. Hess’s law deals with

Equilibrium constant

Influence of pressure on volume of a gas

Rate of reaction

Changes in heat or reaction

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

Endothermic

Exothermic

Synthesis

Both a and b

31. 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

-11 kcal

-44 kcal

-88 kcal

32. Total energy of a system is

K.E + heat energy

P.E + heat energy

P.E + mechanical energy

P.E + K.E

33. Mechanical work is especially important in systems that contain

Solid-liquid

Gases

Solid-solid

Liquid-liquid

34. 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)

28.5 kJ

17.1kJ

45.7 kJ

1.7 kJ

35. All of the following are state function except

36. 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

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

Born Haber cycle is different from Hess’s law

The lattice energy of the crystalline substances can be calculated easily

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

38. 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 large + ve value for enthalpy change

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

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

Hess’s law

Graham’s law

Boyle’s law

Henry’s law

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

Erg

Electron vol

Calorie

Joule

41. 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

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

It is not irreversible

It is irreversible

None of these

It is reversible

43. 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

44. 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

45. 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

46. Which of the following is not correct?

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

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

Dissolution on NH₄Cl in excess of water is an endothermic process

Neutralization is always exothermic

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

Physical process

Chemical process

Endothermic process

Biochemical process

48. In endothermic reactions, the heat content of the

Reactants is more than that of products

Reactants and products are equal

Products is more than that of reactants

Both a and b

49. Two fundamental ways to transfer energy are

Heat and work

Pressure and temperature

Heat and volume

Pressure and volume

50. Most of the thermodynamic parameters are

System

State function

Surrounding

Phase

Page 3 of 5

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

None of these

Bond length

Bond strength

Bond energy

52. An adiabatic expansion of an ideal gas always has

∆H = 0

Q = 0

W = 0

Decrease in temperature

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

Endothermic

Non-spontaneous

Exothermic

Spontaneous

54. 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

55. If internal energy of the system is increased

Temperature of the system may rise

All

Chemical reaction may take place

Change in state of the system is increased

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

Both are equally stable

Stability cannot to predicated

Graphite is more stable than diamond

Graphite has more energy than diamond

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

Respiration

Neutralization

Combustion

Thermal decomposition

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

Joules

Watt

None of these

Calorie

59. Most of the reactions which give stable products are

Exothermic

Endothermic

Isothermal

None of these

60. 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

Burning of coal is and endothermic process

Burning of coal in air releases large amount of energy

None of these

61. 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

Water will vaporize

Ice will melt

62. 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

63. Two fundamental ways to transfer energy are

Pressure and volume

Pressure and temperature

Heat and work

Heat and volume

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

+64.8 kcal mol¯¹

-231.6 kcal mol¯¹

-94.0 kcal mol¯¹

+21.4 kcal mol¯¹

65. The reaction is spontaneous if the cell potential is

Infinite

Negative

Positive

Zero

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

Endothermic

Exothermic

Photochemical

Explosive

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

573 kJ

11.46 kJ

573 J

57.3 kJ

68. 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

2.4 K

4.8 K

1.2 K

6.6 K

69. Evaporation of water is

A process where no heat changes occur

An endothermic change

An exothermic change

A process accompanied by chemical reaction

70. 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

-668 kJ mol¯¹

112 kJ mol¯¹

668 kJ mol¯¹

-112 kJ mol¯¹

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

Hess’s law

Graham’s law

Charles’s law

Henry’s law

72. Which type of reactions cannot occur spontaneously?

Exothermic

Both a and b

Neither

Endothermic

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

∆H = ∆E – d

∆H = ∆E – PV

∆H = ∆E + Pv

∆H = ∆E + d

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

Isothermal

Adiabatic

Isolated

Closed

75. For a reaction to occur spontaneously

∆ H must be negative

∆ H must be unity

∆ H must be zero

∆ H must be positive

Page 4 of 5

76. 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

-339.3 kJ mol¯¹

-439.3 kJ mol¯¹

-221.1 kJ mol¯¹

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

Be half

Not change

Be double

None of these

78. In general, for exothermic reactions to be spontaneous

Temperature should be low

Temperature has no effect

Temperature should be high

Temperature should be zero

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

Increase of enthalpy

Decrease of entropy

Decrease of free energy

Increase of free energy

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

Surrounding

State function

System

Any substance

81. 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

Heat of combustion

Enthalpy of reaction

Hat of formation

82. 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

83. Reaction in which heat is evolved

Non-spontaneous

Exothermic

Endothermic

Spontaneous

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

Pressure and volume

Energy and volume

Temperature and pressure

Temperature and volume

85. 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

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

87. Endothermic changes are indicated through

Making of chemical bond

All of these

Breaking of chemical bonds

Burning of carbon

88. Unit of heat is SI system is

KCaL

Cal

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

Erg

Calorie

Electron – volt

Joule

90. 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

HF is more stable than HCl

HCl is more stable than HF

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

91. Calorie is equivalent to

418.4 J

0.4184 J

41.84 J

4.184 J

92. An endothermic reaction is one in which

Heat is absorbed

Heat is converted into electricity

Heat is converted into mechanical work

Heat is evolved

93. Total energy of a system is

P.E, + mechanical energy

K.E, + heat energy

P.E, + K.E.

P.E. + heat energy

94. A spontaneous change means

A lowering of free energy

No energy change

A lowering of energy

An increase in internal energy

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

Positive

Unity

Negative

Zero

96. Which one is not state function?

Work

Internal energy

Gibbs free energy

Enthalpy

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

Thermodynamics

Kinetics

Photochemistry

Thermochemistry

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

Thermochemistry

Stoichiometry

Thermodynamics

Kinetics

99. 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

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

Free energy change

Enthalpy change

Internal energy change

Entropy change

Page 5 of 5

101. 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?

70960 calories

-70 calories

+70 calories

71030 calories

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

Heat of sublimation

Heat of combustion

Heat of reaction

Heat of neutralization

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

State function

Physical property

Chemical property

Energy of the system

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

Volume

Temperature

Pressure

Density

105. Pumping of water uphill is

Irreversible process

None of these

Non spontaneous

Spontaneous process

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

Glass Calorimeter

Bomb Calorimeter

Thermometer

Monometer

107. The enthalpy of formation of carbon monoxide will be

2x – y/2

Y – 2x/2

Y – 2x

2x – y

108. 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

-250 kJ

+125 kJ

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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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Chemistry Thermochemistry MCQS Online Test

ECAT Chemistry Thermochemistry Chapter Online Test

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