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

∆H = ∆E – d

∆H = ∆E + Pv

∆H = ∆E – PV

∆H = ∆E + d

2. 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

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

57.3 kJ

11.46 kJ

573 J

573 kJ

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

-231.6 kcal mol¯¹

+64.8 kcal mol¯¹

+21.4 kcal mol¯¹

-94.0 kcal mol¯¹

5. For a reaction to occur spontaneously

∆ H must be positive

∆ H must be unity

∆ H must be zero

∆ H must be negative

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

Thermochemistry

Mechanics

Thermodynamics

Chemical kinetics

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

Boyle’s law

Henry’s law

Graham’s law

Hess’s law

8. 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

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

Decomposition

Both a and b

Exothermic

Endothermic

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

Physical process

Endothermic process

Biochemical process

Chemical process

11. 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

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

Erg

Electron vol

Calorie

Joule

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

Have the same energy as the products

Have more energy than the products

Are at a higher temperature than the products

Have less energy than the products

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

Negative

Unity

Zero

Positive

15. 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

-668 kJ mol¯¹

-112 kJ mol¯¹

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

Spontaneous

Exothermic

Endothermic

Non-spontaneous

17. 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

18. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

57.3 kJ

2 x 57.3 kJ

Cannot be predicted

57.3/2 kJ

19. The reaction is spontaneous if the cell potential is

Zero

Positive

Negative

Infinite

20. 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

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

Bomb calorimeter

Copper calorimeter

All above

Glass calorimeter

22. 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

23. When a bond breaks

Temperature increases

Heat is evolved

No change in heat contents takes place

Heat is absorbed

24. A spontaneous change means

A lowering of free energy

No energy change

A lowering of energy

An increase in internal energy

25. 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 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

Page 2 of 5

26. 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

27. Two fundamental ways to transfer energy are

Pressure and temperature

Heat and work

Heat and volume

Pressure and volume

28. Enthalpy of a reaction can be measured by

Glass calorimeter

Thermometer

Manometer

Barometer

29. An endothermic reaction is one in which

Heat is evolved

Heat is converted into mechanical work

Heat is converted into electricity

Heat is absorbed

30. 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

28.5 kJ

45.7 kJ

1.7 kJ

31. Mechanical work is especially important in systems that contain

Gases

Solid-liquid

Solid-solid

Liquid-liquid

32. 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

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

P∆V + nRT

∆H = ∆E + P∆V

∆E = q + w

Q = m x X x ∆ T

34. 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

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

Exothermic

Spontaneous

Non-spontaneous

Endothermic

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

Both a and b

Synthesis

Exothermic

Endothermic

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

Entropy change

Internal energy change

Enthalpy change

Free energy change

38. Which type of reactions cannot occur spontaneously?

Endothermic

Neither

Exothermic

Both a and b

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

State function

Any substance

Surrounding

System

40. If internal energy of a system is increased

Temperature of the system may rise

All

Chemical reaction can take place

Change in state of system can occur

41. 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

70960 calories

-70 calories

71030 calories

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

Thermodynamics

Kinetics

Thermochemistry

Stoichiometry

43. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

Y – 2x

2x – y

2x – y/2

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

Second law

Third law

First law

Zeroth law

45. Which one is not a state function?

Work

Internal energy

Enthalpy

Gibbs free energy

46. 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

47. All of the following are state function except

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

Bomb Calorimeter

Monometer

Thermometer

Glass Calorimeter

49. An adiabatic expansion of an ideal gas always has

Q = 0

W = 0

∆H = 0

Decrease in temperature

50. 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

-125 kJ

+250 kJ

-250 kJ

Page 3 of 5

51. 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)

50 days

20 days

32 days

15 days

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

Volume

Pressure

Temperature

Density

53. Most of the thermodynamic parameters are

State function

System

Surrounding

Phase

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

Photochemical

Exothermic

Endothermic

Explosive

55. Free energy change for a reversible process is:

Equal to zero

Unpredictable

56. 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

57. The law of Lavoisier and Laplace illustrates

Equivalence of mechanical and thermal energy

The principle of conservation of matter

The principle of conservation of energy

Equivalent of mechanical and chemical energy

58. 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

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

None of these

Joules

Calorie

Watt

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

It has a large + ve value for enthalpy change

It has small + ve value for enthalpy 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 the entropy change

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

Remains same

Remains constant

Increases

Decreases

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

Energy and volume

Temperature and pressure

Temperature and volume

Pressure and volume

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

Phase

System

Surrounding

State

64. Most of the reactions which give stable products are

Isothermal

Exothermic

Endothermic

None of these

65. 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

Insufficient data

2.33 JK¯¹

11.272 JK¯¹

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

It is reversible

It is irreversible

None of these

It is not irreversible

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

Electron – volt

Calorie

Erg

Joule

68. Calorie is equivalent to

41.84 J

0.4184 J

418.4 J

4.184 J

69. Which one is not state function?

Enthalpy

Work

Gibbs free energy

Internal energy

70. Reaction in which heat is evolved

Non-spontaneous

Endothermic

Exothermic

Spontaneous

71. 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

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

73. 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

74. 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

676.5 kJ

-110.5 kJ

110.5 kJ

75. Total energy of a system is

P.E, + K.E.

K.E, + heat energy

P.E. + heat energy

P.E, + mechanical energy

Page 4 of 5

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

3 kg H₂O

2 kg H₂O

4 kg H₂O

1 kg H₂O

77. 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

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

Both are equally stable

Graphite is more stable than diamond

Stability cannot to predicated

Graphite has more energy than diamond

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

Electron – volt

Joule

Calorie

Erg

80. Evaporation of water is

A process accompanied by chemical reaction

An endothermic change

An exothermic change

A process where no heat changes occur

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

Increase of enthalpy

Decrease of entropy

Increase of free energy

Decrease of free energy

82. Hess’s law deals with

Changes in heat or reaction

Influence of pressure on volume of a gas

Equilibrium constant

Rate of reaction

83. Unit of heat in S.I system is

Cal

Kcal

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

Joule cm¯¹ deg¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ Kg¯¹

Joule deg¯¹ atom¯¹

85. 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

Unpredictable

Absorption of 218 kcal of energy

Release of 218 kcal of energy

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

Neutralization

Respiration

Combustion

Thermal decomposition

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

Enthalpy of reaction

Heat of combustion

Hat of formation

Heat of neutralization

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

Thermochemistry

Thermodynamics

Kinetics

Photochemistry

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

Physical property

State function

Energy of the system

Chemical property

90. Total energy of a system is

P.E + K.E

P.E + heat energy

K.E + heat energy

P.E + mechanical energy

91. 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

0 J

= - k719

-400J

92. Two fundamental ways to transfer energy are

Heat and volume

Pressure and volume

Heat and work

Pressure and temperature

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

None of these

Water equivalent

Thermal capacity

Specific heat

94. Total energy depends upon the state of system

Enthalpy

Entropy of reaction

Free energy of reaction

All above

95. Pumping of water uphill is

Spontaneous process

Irreversible process

None of these

Non spontaneous

96. 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

Non-spontaneous

Spontaneous

Reversible

Irreversible

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

Isothermal

Closed

Isolated

Adiabatic

98. 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

1.2 K

2.4 K

6.6 K

99. 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

100. In general, for exothermic reactions to be spontaneous

Temperature should be zero

Temperature should be high

Temperature should be low

Temperature has no effect

Page 5 of 5

101. Endothermic changes are indicated through

Burning of carbon

All of these

Breaking of chemical bonds

Making of chemical bond

102. 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

Zero

< 40 kJ

40 kJ

103. 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

-44 kcal

-22 kcal

-11 kcal

104. Unit of heat is SI system is

Cal

KCaL

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

Bond strength

None of these

Bond energy

Bond length

106. If internal energy of the system is increased

Chemical reaction may take place

Change in state of the system is increased

Temperature of the system may rise

All

107. 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

-27 KJ/mole

395 KJ/mole

190 KJ/mole

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

Be half

Be double

None of these

Not change

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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

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