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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. 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

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

Photochemistry

Kinetics

Thermochemistry

Thermodynamics

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

Glass Calorimeter

Bomb Calorimeter

Thermometer

Monometer

4. The law of Lavoisier and Laplace illustrates

Equivalence of mechanical and thermal energy

The principle of conservation of matter

Equivalent of mechanical and chemical energy

The principle of conservation of energy

5. The enthalpy of formation of carbon monoxide will be

Y – 2x

2x – y

2x – y/2

Y – 2x/2

6. Endothermic changes are indicated through

Burning of carbon

Making of chemical bond

All of these

Breaking of chemical bonds

7. Most of the reactions which give stable products are

Isothermal

None of these

Endothermic

Exothermic

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

Thermochemistry

Thermodynamics

Mechanics

Chemical kinetics

9. Mechanical work is especially important in systems that contain

Solid-liquid

Liquid-liquid

Gases

Solid-solid

10. 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

None of these

Burning of coal in air releases large amount of energy

Burning of coal is and endothermic process

11. Unit of heat is SI system is

KCaL

Cal

12. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

2 x 57.3 kJ

57.3 kJ

57.3/2 kJ

Cannot be predicted

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

It has a large – ve value for the entropy change

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

15. If internal energy of a system is increased

Change in state of system can occur

Chemical reaction can take place

Temperature of the system may rise

All

16. 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

150 kJ

50 kJ

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

System

Any substance

State function

Surrounding

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

Temperature and volume

Pressure and volume

Temperature and pressure

Energy and volume

19. 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

50 days

20 days

32 days

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

Isothermal

Isolated

Adiabatic

Closed

21. 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

-11 kcal

-88 kcal

-22 kcal

-44 kcal

22. Free energy change for a reversible process is:

Equal to zero

Unpredictable

23. An adiabatic expansion of an ideal gas always has

W = 0

∆H = 0

Q = 0

Decrease in temperature

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

Water equivalent

None of these

Specific heat

Thermal capacity

25. An endothermic reaction is one in which

Heat is converted into electricity

Heat is converted into mechanical work

Heat is absorbed

Heat is evolved

Page 2 of 5

26. 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

+70 calories

70960 calories

27. 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

28. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be negative

∆ H must be positive

∆ H must be unity

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

It is not irreversible

It is irreversible

It is reversible

None of these

30. Calorie is equivalent to

4.184 J

41.84 J

0.4184 J

418.4 J

31. 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 vaporize

Ice will melt

Water will freeze

Ice will sublime

32. Most of the thermodynamic parameters are

Surrounding

Phase

State function

System

33. Total energy of a system is

P.E + mechanical energy

P.E + K.E

P.E + heat energy

K.E + heat energy

34. 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

6.6 K

2.4 K

35. The reaction is spontaneous if the cell potential is

Negative

Infinite

Zero

Positive

36. 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

Release of 218 kcal of energy

Unpredictable

Absorption of 218 kcal of energy

37. 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

38. Pumping of water uphill is

Irreversible process

Non spontaneous

None of these

Spontaneous process

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

Heat of reaction

Heat of combustion

Heat of sublimation

Heat of neutralization

40. 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

= - k719

-400J

= + k319

41. A spontaneous change means

A lowering of free energy

A lowering of energy

An increase in internal energy

No energy change

42. When a bond breaks

Temperature increases

Heat is evolved

No change in heat contents takes place

Heat is absorbed

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

Respiration

Thermal decomposition

Combustion

Neutralization

44. Enthalpy of a reaction can be measured by

Barometer

Manometer

Glass calorimeter

Thermometer

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

Pressure

Density

Temperature

Volume

46. Which one is not state function?

Internal energy

Gibbs free energy

Enthalpy

Work

47. In general, for exothermic reactions to be spontaneous

Temperature has no effect

Temperature should be low

Temperature should be high

Temperature should be zero

48. 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

-110.5 kJ

110.5 kJ

676.5 kJ

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

Exothermic

Non-spontaneous

Spontaneous

Endothermic

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

Entropy change

Enthalpy change

Free energy change

Internal energy change

Page 3 of 5

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

Calorie

Joules

Watt

None of these

52. 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)

2.198

20.13

21.98

2.013

53. Total energy of a system is

K.E, + heat energy

P.E, + K.E.

P.E. + heat energy

P.E, + mechanical energy

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

Bomb calorimeter

All above

Glass calorimeter

Copper calorimeter

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

Stability cannot to predicated

Graphite has more energy than diamond

Both are equally stable

Graphite is more stable than diamond

56. 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

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

573 J

57.3 kJ

573 kJ

11.46 kJ

58. 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

59. 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

-439.3 kJ mol¯¹

-339.3 kJ mol¯¹

60. 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

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

The sum of all motions which are possible

Translational motion

Rotational motion

Vibrational motion

62. 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

63. Which one is not a state function?

Internal energy

Gibbs free energy

Enthalpy

Work

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

Photochemical

Explosive

Endothermic

Exothermic

65. Evaporation of water is

An endothermic change

An exothermic change

A process where no heat changes occur

A process accompanied by chemical reaction

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

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

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

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

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

The lattice energy of the crystalline substances can be calculated easily

The energy change in a cyclic process is not zero

68. 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 neutralization

Enthalpy of reaction

Heat of combustion

Hat of formation

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

Both a and b

Exothermic

Decomposition

Endothermic

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

4 kg H₂O

2 kg H₂O

3 kg H₂O

1 kg H₂O

71. Unit of heat in S.I system is

Cal

Kcal

72. 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

+142.5 kJ

-285 kJ

73. 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)

1.7 kJ

17.1kJ

28.5 kJ

45.7 kJ

74. If internal energy of the system is increased

Chemical reaction may take place

Change in state of the system is increased

All

Temperature of the system may rise

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

Hess’s law

Henry’s law

Boyle’s law

Graham’s law

Page 4 of 5

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

Stoichiometry

Kinetics

Thermochemistry

Thermodynamics

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

Not change

None of these

Be double

Be half

78. Reaction in which heat is evolved

Spontaneous

Non-spontaneous

Exothermic

Endothermic

79. 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

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

Endothermic process

Chemical process

Biochemical process

Physical process

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

2.303 R

0.1 R

100.0 R

10.0 R

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

Joule

Erg

Electron – volt

Calorie

83. Which of the following is not correct?

Neutralization is always exothermic

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

84. 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 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

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

85. In endothermic reactions, the heat content of the

Reactants is more than that of products

Products is more than that of reactants

Reactants and products are equal

Both a and b

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

Positive

Zero

Negative

Unity

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

Endothermic

Both a and b

Synthesis

Exothermic

88. Two fundamental ways to transfer energy are

Heat and work

Pressure and temperature

Heat and volume

Pressure and volume

89. 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

90. Hess’s law deals with

Influence of pressure on volume of a gas

Rate of reaction

Changes in heat or reaction

Equilibrium constant

91. 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

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

Energy of the system

Chemical property

State function

Physical property

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

Erg

Electron vol

Joule

Calorie

94. All of the following are state function except

95. Total energy depends upon the state of system

Free energy of reaction

Entropy of reaction

All above

Enthalpy

96. 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

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

Graham’s law

Charles’s law

Henry’s law

Hess’s law

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

Bond energy

Bond length

Bond strength

None of these

99. Two fundamental ways to transfer energy are

Pressure and volume

Heat and work

Pressure and temperature

Heat and volume

100. Which type of reactions cannot occur spontaneously?

Both a and b

Endothermic

Exothermic

Neither

Page 5 of 5

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

Calorie

Joule

Electron – volt

Erg

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

Decreases

Increases

Remains constant

Remains same

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

Spontaneous

Non-spontaneous

Endothermic

Exothermic

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

Have less energy than the products

Have more energy than the products

Have the same energy as the products

Are at a higher temperature than the products

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

Surrounding

Phase

State

System

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

-231.6 kcal mol¯¹

-94.0 kcal mol¯¹

+21.4 kcal mol¯¹

+64.8 kcal mol¯¹

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

∆H = ∆E + Pv

∆H = ∆E – d

∆H = ∆E – PV

∆H = ∆E + d

108. 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

11.272 JK¯¹

Insufficient data

2.33 JK¯¹

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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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