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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. 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

50 kJ

300 kJ

100 kJ

150 kJ

2. Unit of heat is SI system is

Cal

KCaL

3. Total energy of a system is

P.E, + mechanical energy

P.E. + heat energy

P.E, + K.E.

K.E, + heat energy

4. 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

Absorption of 218 kcal of energy

Unpredictable

Release of 109 kcal of energy

Release of 218 kcal of energy

5. Mechanical work is especially important in systems that contain

Solid-solid

Gases

Solid-liquid

Liquid-liquid

6. Total energy of a system is

P.E + heat energy

K.E + heat energy

P.E + mechanical energy

P.E + K.E

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

Surrounding

System

State function

Any substance

8. 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

9. 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

Heat of formation of the product and lattice energy of the substance can be calculated simultaneously

Born Haber cycle is different from Hess’s law

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

Thermochemistry

Stoichiometry

Thermodynamics

Kinetics

11. Most of the reactions which give stable products are

None of these

Exothermic

Endothermic

Isothermal

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

Joules

Calorie

Watt

None of these

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

Bond energy

None of these

Bond strength

Bond length

14. 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

-400J

= - k719

= + k319

15. Unit of heat in S.I system is

Kcal

Cal

16. Which one is not state function?

Enthalpy

Work

Gibbs free energy

Internal energy

17. 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

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

Thermal capacity

None of these

Specific heat

Water equivalent

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

Electron – volt

Calorie

Erg

Joule

20. 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

Hess’s law

Graham’s law

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

∆H = ∆E – PV

∆H = ∆E + d

∆H = ∆E + Pv

∆H = ∆E – d

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

Exothermic

Non-spontaneous

Spontaneous

Endothermic

23. 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

-22 kcal

-11 kcal

24. 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

25. 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

Page 2 of 5

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

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

Temperature and pressure

Energy and volume

Pressure and volume

Temperature and volume

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

Joule deg¯¹ mol¯¹

Joule cm¯¹ deg¯¹

Joule deg¯¹ Kg¯¹

Joule deg¯¹ atom¯¹

29. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and temperature

Pressure and volume

30. An endothermic reaction is one in which

Heat is evolved

Heat is converted into electricity

Heat is converted into mechanical work

Heat is absorbed

31. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

57.3/2 kJ

Cannot be predicted

57.3 kJ

2 x 57.3 kJ

32. 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

33. 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

34. Endothermic changes are indicated through

All of these

Burning of carbon

Making of chemical bond

Breaking of chemical bonds

35. Most of the thermodynamic parameters are

State function

Surrounding

Phase

System

36. 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

-221.1 kJ mol¯¹

-339.3 kJ mol¯¹

-523.3 kJ mol¯¹

-439.3 kJ mol¯¹

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

Density

Temperature

Pressure

Volume

38. 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

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

Boyle’s law

Hess’s law

Henry’s law

Graham’s law

40. Evaporation of water is

An exothermic change

An endothermic change

A process where no heat changes occur

A process accompanied by chemical reaction

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

Zeroth law

Second law

First law

Third law

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

Chemical kinetics

Thermodynamics

Mechanics

Thermochemistry

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

Zero

Unity

Negative

Positive

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

190 KJ/mole

386 KJ/mole

-27 KJ/mole

395 KJ/mole

45. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

Y – 2x

2x – y/2

2x – y

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)

20.13

2.013

2.198

21.98

47. Which of the following is not correct?

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

Dissolution on NH₄Cl in excess of water is an endothermic process

Neutralization is always exothermic

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

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

Exothermic

Endothermic

Spontaneous

Non-spontaneous

49. An adiabatic expansion of an ideal gas always has

W = 0

∆H = 0

Decrease in temperature

Q = 0

50. When a bond breaks

No change in heat contents takes place

Heat is absorbed

Heat is evolved

Temperature increases

Page 3 of 5

51. Total energy depends upon the state of system

Free energy of reaction

All above

Enthalpy

Entropy of reaction

52. 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

53. 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)

15 days

32 days

20 days

50 days

54. 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

55. Calorie is equivalent to

0.4184 J

418.4 J

41.84 J

4.184 J

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

1 kg H₂O

2 kg H₂O

3 kg H₂O

4 kg H₂O

57. Pumping of water uphill is

Spontaneous process

None of these

Irreversible process

Non spontaneous

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

Physical property

State function

Chemical property

Energy of the system

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

Entropy change

Enthalpy change

Internal energy change

Free energy change

60. 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

1.7 kJ

45.7 kJ

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

Kinetics

Thermochemistry

Photochemistry

Thermodynamics

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

Combustion

Neutralization

Respiration

Thermal decomposition

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

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

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

64. 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

1.2 K

4.8 K

6.6 K

65. 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

66. Two fundamental ways to transfer energy are

Pressure and volume

Heat and work

Heat and volume

Pressure and temperature

67. 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

100.0 R

0.1 R

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

Remains constant

Remains same

Decreases

Increases

69. 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

70. Free energy change for a reversible process is:

Equal to zero

Unpredictable

71. 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

57.3 kJ

573 J

72. In endothermic reactions, the heat content of the

Products is more than that of reactants

Reactants is more than that of products

Reactants and products are equal

Both a and b

73. Reaction in which heat is evolved

Non-spontaneous

Spontaneous

Exothermic

Endothermic

74. A spontaneous change means

A lowering of energy

An increase in internal energy

A lowering of free energy

No energy change

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

Endothermic

Both a and b

Synthesis

Exothermic

Page 4 of 5

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

Decrease of free energy

Increase of enthalpy

Increase of free energy

Decrease of entropy

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

Endothermic

Photochemical

Explosive

Exothermic

78. In general, for exothermic reactions to be spontaneous

Temperature has no effect

Temperature should be zero

Temperature should be low

Temperature should be high

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

Rotational motion

Translational motion

The sum of all motions which are possible

Vibrational motion

80. For a reaction to occur spontaneously

∆ H must be negative

∆ H must be positive

∆ H must be zero

∆ H must be unity

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

Biochemical process

Physical process

Chemical process

Endothermic process

82. 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

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

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

None of these

84. Which one is not a state function?

Internal energy

Work

Gibbs free energy

Enthalpy

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

Erg

Calorie

Electron – volt

Joule

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

Isothermal

Isolated

Closed

Adiabatic

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

Both a and b

Decomposition

Exothermic

Endothermic

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

None of these

It is reversible

It is not irreversible

It is irreversible

89. The reaction is spontaneous if the cell potential is

Negative

Infinite

Positive

Zero

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

∆E = q + w

∆H = ∆E + P∆V

Q = m x X x ∆ T

P∆V + nRT

91. Hess’s law deals with

Equilibrium constant

Influence of pressure on volume of a gas

Rate of reaction

Changes in heat or reaction

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

Calorie

Joule

Electron vol

Erg

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

Monometer

Glass Calorimeter

Bomb Calorimeter

Thermometer

94. 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

-112 kJ mol¯¹

-668 kJ mol¯¹

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

All above

Glass calorimeter

Bomb calorimeter

Copper calorimeter

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

Reversible

Irreversible

Spontaneous

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

HCl is more stable than HF

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

HF and HCl are endothermic compounds

HF is more stable than HCl

98. 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

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

None of these

Not change

Be half

Be double

100. Enthalpy of a reaction can be measured by

Glass calorimeter

Barometer

Manometer

Thermometer

Page 5 of 5

101. Which type of reactions cannot occur spontaneously?

Neither

Both a and b

Exothermic

Endothermic

102. 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 a have more potential energy than the reactant

The sign of H is positive, and the products have less potential energy than the reactants

103. 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

104. All of the following are state function except

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

Have less energy than the products

Have the same energy as the products

Are at a higher temperature than the products

Have more energy than the products

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

State

System

Surrounding

Phase

107. 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

108. 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

Enthalpy of reaction

Hat of formation

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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

Chemistry

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Chemistry Thermochemistry MCQS Online Test

MDCAT Chemistry Thermochemistry Chapter Online Test

MDCAT Chemistry Thermochemistry Test

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