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MDCAT Thermo-Chemistry and Energetics of Chemical Reactions Test Online

Mustansar KhanLast Updated: May 24, 2025

Chemistry Thermochemistry MCQS Online Test

MDCAT 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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MDCAT Chemistry Thermochemistry Test

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Page 1 of 5

Chemistry

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

2. Calorie is equivalent to

4.184 J

0.4184 J

418.4 J

41.84 J

3. 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

4. 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)

2.013

21.98

20.13

2.198

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

All above

Glass calorimeter

Bomb calorimeter

Copper calorimeter

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

Explosive

Exothermic

Endothermic

Photochemical

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

Surrounding

Any substance

State function

System

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

Specific heat

None of these

Water equivalent

Thermal capacity

9. Pumping of water uphill is

Irreversible process

Spontaneous process

Non spontaneous

None of these

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

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

Isolated

Adiabatic

Closed

Isothermal

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

Henry’s law

Graham’s law

Charles’s law

Hess’s law

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

Energy of the system

Physical property

State function

Chemical property

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

None of these

It is reversible

It is irreversible

It is not irreversible

15. If internal energy of the system is increased

All

Chemical reaction may take place

Temperature of the system may rise

Change in state of the system is increased

16. Evaporation of water is

A process where no heat changes occur

A process accompanied by chemical reaction

An endothermic change

An exothermic change

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

Physical process

Chemical process

Endothermic process

Biochemical process

18. Which one is not state function?

Gibbs free energy

Work

Internal energy

Enthalpy

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

P∆V + nRT

Q = m x X x ∆ T

∆H = ∆E + P∆V

∆E = q + w

20. 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

15 days

20 days

21. Enthalpy of a reaction can be measured by

Thermometer

Glass calorimeter

Manometer

Barometer

22. 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

2.33 JK¯¹

9.75 JK¯¹

11.272 JK¯¹

23. If internal energy of a system is increased

All

Chemical reaction can take place

Change in state of system can occur

Temperature of the system may rise

24. Which type of reactions cannot occur spontaneously?

Endothermic

Both a and b

Exothermic

Neither

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

Volume

Density

Temperature

Pressure

Page 2 of 5

26. When a bond breaks

No change in heat contents takes place

Temperature increases

Heat is evolved

Heat is absorbed

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

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

Continuous production of mechanical work without supplying an equivalent amount of heat energy

Work done is independent of its path

28. Unit of heat is SI system is

Cal

KCaL

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

Electron vol

Calorie

Erg

Joule

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

Erg

Electron – volt

Calorie

Joule

31. 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

32. Two fundamental ways to transfer energy are

Heat and work

Pressure and temperature

Pressure and volume

Heat and volume

33. 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?

Zero

40 kJ

> 40 kJ

< 40 kJ

34. 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

35. In general, for exothermic reactions to be spontaneous

Temperature should be zero

Temperature should be low

Temperature should be high

Temperature has no effect

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

37. 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

38. Mechanical work is especially important in systems that contain

Liquid-liquid

Solid-solid

Solid-liquid

Gases

39. 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

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

None of these

Be half

Be double

Not change

41. The enthalpy of formation of carbon monoxide will be

2x – y/2

Y – 2x

Y – 2x/2

2x – y

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

Neutralization

Thermal decomposition

Respiration

Combustion

43. Which one is not a state function?

Enthalpy

Work

Internal energy

Gibbs free energy

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

Pressure and volume

Temperature and pressure

Temperature and volume

Energy and volume

45. 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

46. 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

2.4 K

4.8 K

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

Translational motion

The sum of all motions which are possible

Vibrational motion

Rotational motion

48. 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

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

Monometer

Glass Calorimeter

Thermometer

Bomb Calorimeter

50. For a reaction to occur spontaneously

∆ H must be unity

∆ H must be negative

∆ H must be zero

∆ H must be positive

Page 3 of 5

51. The reaction is spontaneous if the cell potential is

Positive

Negative

Zero

Infinite

52. Hess’s law deals with

Rate of reaction

Changes in heat or reaction

Equilibrium constant

Influence of pressure on volume of a gas

53. 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

45.7 kJ

1.7 kJ

17.1kJ

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

Second law

Zeroth law

Third law

First law

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

Thermochemistry

Mechanics

Thermodynamics

Chemical kinetics

56. A spontaneous change means

An increase in internal energy

A lowering of free energy

A lowering of energy

No energy change

57. 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

= + k319

-400J

= - k719

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

Phase

System

State

Surrounding

59. 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

60. Total energy depends upon the state of system

Free energy of reaction

Enthalpy

Entropy of reaction

All above

61. Endothermic changes are indicated through

Making of chemical bond

All of these

Breaking of chemical bonds

Burning of carbon

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

Stoichiometry

Kinetics

Thermochemistry

Thermodynamics

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

Electron – volt

Erg

Joule

Calorie

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

Have more energy than the products

Have less energy than the products

Have the same energy as the products

Are at a higher temperature than the products

65. All of the following are state function except

66. An adiabatic expansion of an ideal gas always has

W = 0

Q = 0

Decrease in temperature

∆H = 0

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

Both are equally stable

Graphite is more stable than diamond

Graphite has more energy than diamond

Stability cannot to predicated

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

Negative

Unity

Zero

Positive

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

Free energy change

Internal energy change

Enthalpy change

Entropy change

70. 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

-439.3 kJ mol¯¹

-523.3 kJ mol¯¹

-339.3 kJ mol¯¹

-221.1 kJ mol¯¹

71. The law of Lavoisier and Laplace illustrates

The principle of conservation of energy

The principle of conservation of matter

Equivalent of mechanical and chemical energy

Equivalence of mechanical and thermal energy

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

None of these

Joules

Calorie

Watt

73. Which statement describes characteristics of an endothermic reaction?

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

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

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

∆H = ∆E – d

∆H = ∆E – PV

∆H = ∆E + d

∆H = ∆E + Pv

75. Most of the reactions which give stable products are

None of these

Endothermic

Isothermal

Exothermic

Page 4 of 5

76. 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

Heat of neutralization

Hat of formation

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

Increase of free energy

Increase of enthalpy

Decrease of entropy

Decrease of free energy

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

2 kg H₂O

3 kg H₂O

4 kg H₂O

1 kg H₂O

79. 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

80. 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

Release of 218 kcal of energy

Absorption of 218 kcal of energy

81. Unit of heat in S.I system is

Kcal

Cal

82. Two fundamental ways to transfer energy are

Pressure and volume

Pressure and temperature

Heat and volume

Heat and work

83. 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

84. 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 melt

Water will vaporize

Water will freeze

Ice will sublime

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

573 J

573 kJ

11.46 kJ

57.3 kJ

86. 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

395 KJ/mole

-27 KJ/mole

87. 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

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

HCl is more stable than HF

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

Heat of reaction

Heat of neutralization

Heat of combustion

Heat of sublimation

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

Synthesis

Exothermic

Both a and b

Endothermic

90. Total energy of a system is

P.E. + heat energy

P.E, + mechanical energy

K.E, + heat energy

P.E, + K.E.

91. Total energy of a system is

P.E + mechanical energy

P.E + K.E

K.E + heat energy

P.E + heat energy

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

Kinetics

Photochemistry

Thermodynamics

Thermochemistry

93. 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

50 kJ

300 kJ

94. Free energy change for a reversible process is:

Equal to zero

Unpredictable

95. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

57.3/2 kJ

57.3 kJ

Cannot be predicted

2 x 57.3 kJ

96. 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

97. 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

-142.5 kJ

-285 kJ

+285 kJ

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

10.0 R

2.303 R

0.1 R

100.0 R

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

Bond energy

None of these

Bond length

Bond strength

100. 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

Page 5 of 5

101. An endothermic reaction is one in which

Heat is evolved

Heat is absorbed

Heat is converted into mechanical work

Heat is converted into electricity

102. Which of the following is not correct?

Neutralization is always exothermic

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

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

Dissolution on NH₄Cl in excess of water is an endothermic process

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

Henry’s law

Graham’s law

Hess’s law

Boyle’s law

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

Decomposition

Endothermic

Exothermic

Both a and b

105. Most of the thermodynamic parameters are

Surrounding

Phase

System

State function

106. 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

None of these

Burning of coal in air releases large amount of energy

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

+64.8 kcal mol¯¹

-94.0 kcal mol¯¹

+21.4 kcal mol¯¹

-231.6 kcal mol¯¹

108. Reaction in which heat is evolved

Endothermic

Spontaneous

Non-spontaneous

Exothermic

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Mustansar KhanLast Updated: May 24, 2025

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MDCAT Thermo-Chemistry and Energetics of Chemical Reactions Test Online

Chemistry Thermochemistry MCQS Online Test

MDCAT Chemistry Thermochemistry Chapter Online Test

MDCAT Chemistry Thermochemistry Test

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Chemistry Thermochemistry MCQS Online Test

MDCAT Chemistry Thermochemistry Chapter Online Test

MDCAT Chemistry Thermochemistry Test

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