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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. Calorie is equivalent to

418.4 J

0.4184 J

41.84 J

4.184 J

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

Closed

Adiabatic

Isothermal

Isolated

3. 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

11.272 JK¯¹

9.75 JK¯¹

2.33 JK¯¹

Insufficient data

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

Boyle’s law

Henry’s law

Hess’s law

Graham’s law

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

Bond length

None of these

Bond strength

Bond energy

6. The enthalpy of formation of carbon monoxide will be

2x – y/2

Y – 2x

Y – 2x/2

2x – y

7. Which type of reactions cannot occur spontaneously?

Neither

Exothermic

Both a and b

Endothermic

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

Exothermic

Endothermic

Spontaneous

Non-spontaneous

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

P∆V + nRT

∆E = q + w

∆H = ∆E + P∆V

Q = m x X x ∆ T

10. Unit of heat is SI system is

Cal

KCaL

11. Two fundamental ways to transfer energy are

Heat and volume

Pressure and volume

Pressure and temperature

Heat and work

12. Hess’s law deals with

Influence of pressure on volume of a gas

Rate of reaction

Changes in heat or reaction

Equilibrium constant

13. 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

14. Most of the reactions which give stable products are

Exothermic

Isothermal

None of these

Endothermic

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

Not change

Be double

None of these

Be half

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

Specific heat

Thermal capacity

None of these

Water equivalent

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

Calorie

Watt

Joules

None of these

18. 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

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

-94.0 kcal mol¯¹

+64.8 kcal mol¯¹

+21.4 kcal mol¯¹

-231.6 kcal mol¯¹

20. 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

21. The reaction is spontaneous if the cell potential is

Zero

Negative

Positive

Infinite

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

23. The law of Lavoisier and Laplace illustrates

Equivalent of mechanical and chemical energy

The principle of conservation of energy

The principle of conservation of matter

Equivalence of mechanical and thermal energy

24. Most of the thermodynamic parameters are

Surrounding

Phase

State function

System

25. Free energy change for a reversible process is:

Equal to zero

Unpredictable

Page 2 of 5

26. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Cannot be predicted

2 x 57.3 kJ

57.3/2 kJ

57.3 kJ

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

Both a and b

Endothermic

Exothermic

Decomposition

28. Which of the following is not correct?

Dissolution on NH₄Cl in excess of water is an endothermic process

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

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

Neutralization is always exothermic

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

573 kJ

573 J

57.3 kJ

11.46 kJ

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

Exothermic

Explosive

Endothermic

Photochemical

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

Thermochemistry

Mechanics

Thermodynamics

Chemical kinetics

32. 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

+250 kJ

-125 kJ

+125 kJ

33. An endothermic reaction is one in which

Heat is absorbed

Heat is converted into mechanical work

Heat is converted into electricity

Heat is evolved

34. In general, for exothermic reactions to be spontaneous

Temperature should be low

Temperature should be zero

Temperature should be high

Temperature has no effect

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

Glass Calorimeter

Thermometer

Monometer

Bomb Calorimeter

36. Total energy depends upon the state of system

All above

Enthalpy

Free energy of reaction

Entropy of reaction

37. 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

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

State function

Surrounding

Any substance

System

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

Temperature and volume

Temperature and pressure

Pressure and volume

Energy and volume

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

Zeroth law

Third law

First law

Second law

41. Which statement describes characteristics of an endothermic reaction?

The sign of H is positive and the products a have more potential energy than the reactant

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

42. 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

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

System

Phase

State

Surrounding

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

395 KJ/mole

386 KJ/mole

190 KJ/mole

-27 KJ/mole

45. Evaporation of water is

A process where no heat changes occur

A process accompanied by chemical reaction

An endothermic change

An exothermic change

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

Increases

Decreases

Remains same

Remains constant

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

Joule

Calorie

Electron – volt

Erg

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

Both are equally stable

Stability cannot to predicated

Graphite has more energy than diamond

Graphite is more stable than diamond

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

4 kg H₂O

1 kg H₂O

3 kg H₂O

2 kg H₂O

50. 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

Burning of coal in air releases large amount of energy

None of these

Coal and air react giving a reversible reaction

Page 3 of 5

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

Kinetics

Thermodynamics

Thermochemistry

Stoichiometry

52. Unit of heat in S.I system is

Kcal

Cal

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

Thermochemistry

Thermodynamics

Kinetics

Photochemistry

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

Synthesis

Endothermic

Both a and b

Exothermic

55. 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

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

Electron vol

Joule

Calorie

Erg

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

Endothermic

Spontaneous

Exothermic

Non-spontaneous

58. 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

Non-spontaneous

Spontaneous

Reversible

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

Heat of neutralization

Heat of sublimation

Heat of combustion

Heat of reaction

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

Energy of the system

Chemical property

Physical property

State function

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

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

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

62. Total energy of a system is

P.E, + mechanical energy

P.E. + heat energy

K.E, + heat energy

P.E, + K.E.

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

2.4 K

6.6 K

1.2 K

4.8 K

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

Pressure

Density

Temperature

Volume

65. If internal energy of the system is increased

Chemical reaction may take place

Temperature of the system may rise

All

Change in state of the system is increased

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

2.303 R

100.0 R

0.1 R

10.0 R

67. Which one is not state function?

Enthalpy

Work

Internal energy

Gibbs free energy

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

Unity

Zero

Negative

Positive

69. 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

45.7 kJ

28.5 kJ

1.7 kJ

70. Mechanical work is especially important in systems that contain

Solid-liquid

Solid-solid

Liquid-liquid

Gases

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

Glass calorimeter

Copper calorimeter

All above

Bomb calorimeter

72. 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

73. All of the following are state function except

74. 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

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

Free energy change

Entropy change

Internal energy change

Enthalpy change

Page 4 of 5

76. If internal energy of a system is increased

Change in state of system can occur

Temperature of the system may rise

All

Chemical reaction can take place

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

None of these

It is not irreversible

It is irreversible

It is reversible

78. 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

79. 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

Ice will melt

Water will freeze

Water will vaporize

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

Joule cm¯¹ deg¯¹

Joule deg¯¹ atom¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ Kg¯¹

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

Graham’s law

Hess’s law

Henry’s law

Charles’s law

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

Physical process

Endothermic process

Biochemical process

Chemical process

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

∆H = ∆E + d

∆H = ∆E + Pv

∆H = ∆E – d

∆H = ∆E – PV

84. 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

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

The energy change in a cyclic process is not zero

The lattice energy of the crystalline substances can be calculated easily

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

86. Reaction in which heat is evolved

Spontaneous

Non-spontaneous

Exothermic

Endothermic

87. 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

88. 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)

20.13

21.98

2.013

2.198

89. When a bond breaks

No change in heat contents takes place

Heat is evolved

Heat is absorbed

Temperature increases

90. 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

Hat of formation

Heat of neutralization

Enthalpy of reaction

91. 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

HCl is more stable than HF

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

HF is more stable than HCl

92. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and volume

Pressure and temperature

93. Endothermic changes are indicated through

Making of chemical bond

All of these

Breaking of chemical bonds

Burning of carbon

94. 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

50 days

15 days

95. An adiabatic expansion of an ideal gas always has

∆H = 0

Decrease in temperature

Q = 0

W = 0

96. Enthalpy of a reaction can be measured by

Glass calorimeter

Barometer

Thermometer

Manometer

97. Total energy of a system is

P.E + heat energy

P.E + mechanical energy

P.E + K.E

K.E + heat energy

98. For a reaction to occur spontaneously

∆ H must be positive

∆ H must be unity

∆ H must be negative

∆ H must be zero

99. 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

100. A spontaneous change means

A lowering of free energy

No energy change

A lowering of energy

An increase in internal energy

Page 5 of 5

101. 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

102. 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

71030 calories

-70 calories

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

Thermal decomposition

Combustion

Respiration

Neutralization

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

Electron – volt

Erg

Calorie

Joule

105. Pumping of water uphill is

Non spontaneous

Spontaneous process

Irreversible process

None of these

106. Which one is not a state function?

Internal energy

Enthalpy

Gibbs free energy

Work

107. 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

300 kJ

150 kJ

50 kJ

100 kJ

108. 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

-400J

= - k719

0 J

= + k319

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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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