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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

Page 1 of 5

Chemistry

1. 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

-400J

0 J

= - k719

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

Q = m x X x ∆ T

∆H = ∆E + P∆V

∆E = q + w

P∆V + nRT

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

Stoichiometry

Thermodynamics

Thermochemistry

Kinetics

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

Hess’s law

Boyle’s law

Graham’s law

Henry’s law

5. An endothermic reaction is one in which

Heat is converted into mechanical work

Heat is evolved

Heat is converted into electricity

Heat is absorbed

6. Reaction in which heat is evolved

Spontaneous

Exothermic

Endothermic

Non-spontaneous

7. 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

8. The law of Lavoisier and Laplace illustrates

The principle of conservation of matter

The principle of conservation of energy

Equivalent of mechanical and chemical energy

Equivalence of mechanical and thermal energy

9. An adiabatic expansion of an ideal gas always has

∆H = 0

Decrease in temperature

W = 0

Q = 0

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

Glass Calorimeter

Bomb Calorimeter

Thermometer

Monometer

11. The enthalpy of formation of carbon monoxide will be

2x – y/2

2x – y

Y – 2x/2

Y – 2x

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

Exothermic

Synthesis

Both a and b

Endothermic

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

None of these

Burning of coal in air releases large amount of energy

Coal and air react giving a reversible reaction

Burning of coal is and endothermic process

14. 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

15 days

32 days

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

System

State function

Surrounding

Any substance

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

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

HF is more stable than HCl

HF and HCl are endothermic compounds

HCl is more stable than HF

17. Hess’s law deals with

Influence of pressure on volume of a gas

Rate of reaction

Changes in heat or reaction

Equilibrium constant

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

Endothermic

Non-spontaneous

Exothermic

Spontaneous

19. 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

-339.3 kJ mol¯¹

-221.1 kJ mol¯¹

-523.3 kJ mol¯¹

-439.3 kJ mol¯¹

20. Mechanical work is especially important in systems that contain

Solid-solid

Solid-liquid

Gases

Liquid-liquid

21. A spontaneous change means

An increase in internal energy

A lowering of free energy

A lowering of energy

No energy change

22. 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

23. Which type of reactions cannot occur spontaneously?

Neither

Both a and b

Endothermic

Exothermic

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

∆H = ∆E – d

∆H = ∆E + Pv

∆H = ∆E + d

∆H = ∆E – PV

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

It is irreversible

None of these

It is not irreversible

It is reversible

Page 2 of 5

26. Total energy of a system is

P.E, + mechanical energy

P.E. + heat energy

K.E, + heat energy

P.E, + K.E.

27. Endothermic changes are indicated through

Burning of carbon

Making of chemical bond

All of these

Breaking of chemical bonds

28. Unit of heat in S.I system is

Kcal

Cal

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

Glass calorimeter

Bomb calorimeter

All above

Copper calorimeter

30. Two fundamental ways to transfer energy are

Heat and work

Pressure and volume

Heat and volume

Pressure and temperature

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

Joule

Erg

Electron – volt

Calorie

32. In endothermic reactions, the heat content of the

Both a and b

Reactants and products are equal

Reactants is more than that of products

Products is more than that of reactants

33. 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

2.198

20.13

2.013

34. Total energy of a system is

P.E + heat energy

K.E + heat energy

P.E + mechanical energy

P.E + K.E

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

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

Electron – volt

Erg

Joule

Calorie

37. In general, for exothermic reactions to be spontaneous

Temperature should be low

Temperature should be zero

Temperature has no effect

Temperature should be high

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

Joule deg¯¹ Kg¯¹

Joule deg¯¹ atom¯¹

Joule cm¯¹ deg¯¹

Joule deg¯¹ mol¯¹

39. 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

-668 kJ mol¯¹

112 kJ mol¯¹

-112 kJ mol¯¹

40. Calorie is equivalent to

0.4184 J

418.4 J

4.184 J

41.84 J

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

Calorie

Joules

None of these

Watt

42. Most of the thermodynamic parameters are

State function

Surrounding

Phase

System

43. 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

100 kJ

50 kJ

150 kJ

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

Mechanics

Thermochemistry

Thermodynamics

Chemical kinetics

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

None of these

Not change

Be half

Be double

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

Have the same energy as the products

Have more energy than the products

Have less energy than the products

Are at a higher temperature than the products

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

Phase

State

Surrounding

System

48. Which one is not state function?

Gibbs free energy

Internal energy

Work

Enthalpy

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

Graphite is more stable than diamond

Stability cannot to predicated

Graphite has more energy than diamond

Both are equally stable

50. Evaporation of water is

An endothermic change

A process where no heat changes occur

An exothermic change

A process accompanied by chemical reaction

Page 3 of 5

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

Increases

Remains constant

Remains same

Decreases

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

The lattice energy of the crystalline substances can be calculated easily

The energy change in a cyclic process is not zero

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

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

State function

Chemical property

Energy of the system

Physical property

54. 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

10.0 R

2.303 R

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

2 kg H₂O

1 kg H₂O

3 kg H₂O

4 kg H₂O

56. 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

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

Heat of sublimation

Heat of combustion

Heat of neutralization

Heat of reaction

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

First law

Second law

Third law

Zeroth law

59. 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

60. Which one is not a state function?

Enthalpy

Internal energy

Work

Gibbs free energy

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

Endothermic process

Physical process

Biochemical process

Chemical process

62. 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 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 positive, and the products have less potential energy than the reactants

63. 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

Unpredictable

Absorption of 218 kcal of energy

Release of 109 kcal of energy

64. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Cannot be predicted

57.3 kJ

57.3/2 kJ

2 x 57.3 kJ

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

Bond strength

None of these

Bond length

Bond energy

66. 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 + ve value for the entropy change and a – ve value for the enthalpy change

It has a large – ve value for the entropy change

It has a large + ve value for enthalpy change

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

Thermodynamics

Thermochemistry

Kinetics

Photochemistry

68. 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

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

Temperature and pressure

Pressure and volume

Energy and volume

Temperature and volume

70. Free energy change for a reversible process is:

Unpredictable

Equal to zero

71. The reaction is spontaneous if the cell potential is

Zero

Positive

Negative

Infinite

72. 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

386 KJ/mole

-27 KJ/mole

395 KJ/mole

73. 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

74. All of the following are state function except

75. 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

70960 calories

+70 calories

Page 4 of 5

76. 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

4.8 K

1.2 K

2.4 K

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

Entropy change

Internal energy change

Enthalpy change

Free energy change

78. 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

79. 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

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

Work done is independent of its path

80. 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.

Neutralization is always exothermic

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

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

Increase of enthalpy

Increase of free energy

Decrease of free energy

Decrease of entropy

82. 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

83. 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

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

Temperature

Volume

Pressure

Density

85. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be positive

∆ H must be negative

∆ H must be unity

86. Most of the reactions which give stable products are

None of these

Endothermic

Exothermic

Isothermal

87. If internal energy of a system is increased

Chemical reaction can take place

All

Change in state of system can occur

Temperature of the system may rise

88. Total energy depends upon the state of system

Enthalpy

All above

Entropy of reaction

Free energy of reaction

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

11.46 kJ

573 J

57.3 kJ

573 kJ

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

Isothermal

Isolated

Closed

Adiabatic

91. Unit of heat is SI system is

KCaL

Cal

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

-231.6 kcal mol¯¹

+64.8 kcal mol¯¹

-94.0 kcal mol¯¹

+21.4 kcal mol¯¹

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

Exothermic

Photochemical

Endothermic

Explosive

94. 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

Water will freeze

Water will vaporize

Ice will melt

Ice will sublime

95. When a bond breaks

Heat is absorbed

No change in heat contents takes place

Temperature increases

Heat is evolved

96. 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

2.33 JK¯¹

11.272 JK¯¹

Insufficient data

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

Erg

Calorie

Electron vol

Joule

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

Henry’s law

Hess’s law

Graham’s law

Charles’s law

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

Combustion

Thermal decomposition

Respiration

Neutralization

100. Two fundamental ways to transfer energy are

Heat and volume

Pressure and temperature

Heat and work

Pressure and volume

Page 5 of 5

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

Endothermic

Exothermic

Both a and b

Decomposition

102. Pumping of water uphill is

Spontaneous process

Irreversible process

Non spontaneous

None of these

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

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

Zero

Negative

Positive

Unity

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

Translational motion

Vibrational motion

Rotational motion

The sum of all motions which are possible

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

None of these

Thermal capacity

Water equivalent

Specific heat

107. 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

-88 kcal

-11 kcal

-22 kcal

108. Enthalpy of a reaction can be measured by

Glass calorimeter

Manometer

Barometer

Thermometer

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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

ECAT Chemistry Thermochemistry Test

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