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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. Two fundamental ways to transfer energy are

Pressure and volume

Heat and work

Heat and volume

Pressure and temperature

2. Pumping of water uphill is

None of these

Irreversible process

Spontaneous process

Non spontaneous

3. 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

4. Total energy of a system is

P.E + K.E

P.E + heat energy

K.E + heat energy

P.E + mechanical energy

5. 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

32 days

20 days

15 days

6. 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

2.33 JK¯¹

9.75 JK¯¹

11.272 JK¯¹

Insufficient data

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

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

Born Haber cycle is different from Hess’s law

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

Physical process

Biochemical process

Endothermic process

Chemical process

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

Synthesis

Both a and b

Exothermic

Endothermic

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

Remains same

Remains constant

Increases

Decreases

11. Evaporation of water is

A process where no heat changes occur

An exothermic change

An endothermic change

A process accompanied by chemical reaction

12. 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

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

Bond energy

Bond strength

None of these

Bond length

14. The law of Lavoisier and Laplace illustrates

The principle of conservation of energy

The principle of conservation of matter

Equivalence of mechanical and thermal energy

Equivalent of mechanical and chemical energy

15. Free energy change for a reversible process is:

Equal to zero

Unpredictable

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

Zero

Negative

Unity

Positive

17. 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

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

Endothermic

Exothermic

Both a and b

Decomposition

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

Be half

Not change

Be double

None of these

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

Joule

Electron – volt

Calorie

Erg

21. All of the following are state function except

22. 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 the entropy change

It has a large + ve value for enthalpy change

23. If internal energy of a system is increased

Change in state of system can occur

All

Chemical reaction can take place

Temperature of the system may rise

24. Unit of heat is SI system is

Cal

KCaL

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

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

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

Page 2 of 5

26. When a bond breaks

Heat is evolved

No change in heat contents takes place

Heat is absorbed

Temperature increases

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

State function

System

Any substance

Surrounding

28. Endothermic changes are indicated through

Burning of carbon

All of these

Breaking of chemical bonds

Making of chemical bond

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

∆H = ∆E – d

∆H = ∆E + d

∆H = ∆E + Pv

∆H = ∆E – PV

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

Exothermic

Explosive

Endothermic

Photochemical

31. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be unity

∆ H must be positive

∆ H must be negative

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

Temperature and volume

Pressure and volume

Energy and volume

Temperature and pressure

33. Hess’s law deals with

Influence of pressure on volume of a gas

Changes in heat or reaction

Rate of reaction

Equilibrium constant

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

Combustion

Neutralization

Respiration

Thermal decomposition

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

Have the same energy as the products

Have more energy than the products

Are at a higher temperature than the products

Have less energy than the products

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

37. Most of the reactions which give stable products are

Endothermic

Isothermal

Exothermic

None of these

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

Surrounding

Phase

System

State

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

Endothermic

Exothermic

Spontaneous

Non-spontaneous

40. 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

Water will vaporize

Ice will melt

Water will freeze

41. Two fundamental ways to transfer energy are

Heat and volume

Pressure and volume

Heat and work

Pressure and temperature

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

Pressure

Volume

Temperature

Density

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

Joule cm¯¹ deg¯¹

Joule deg¯¹ Kg¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ atom¯¹

44. 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 negative, and the products have more 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

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

Translational motion

Rotational motion

Vibrational motion

The sum of all motions which are possible

46. If internal energy of the system is increased

Change in state of the system is increased

Chemical reaction may take place

Temperature of the system may rise

All

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

∆H = ∆E + P∆V

∆E = q + w

P∆V + nRT

Q = m x X x ∆ T

48. Calorie is equivalent to

418.4 J

0.4184 J

41.84 J

4.184 J

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

Closed

Adiabatic

Isolated

Isothermal

50. An endothermic reaction is one in which

Heat is evolved

Heat is absorbed

Heat is converted into electricity

Heat is converted into mechanical work

Page 3 of 5

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

11.46 kJ

57.3 kJ

573 kJ

573 J

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

Calorie

Erg

Joule

Electron – volt

53. The enthalpy of formation of carbon monoxide will be

Y – 2x/2

Y – 2x

2x – y/2

2x – y

54. Total energy depends upon the state of system

All above

Entropy of reaction

Enthalpy

Free energy of reaction

55. The reaction is spontaneous if the cell potential is

Positive

Negative

Infinite

Zero

56. In endothermic reactions, the heat content of the

Products is more than that of reactants

Reactants and products are equal

Reactants is more than that of products

Both a and b

57. 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

58. 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

Hess’s law

Henry’s law

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

-439.3 kJ mol¯¹

-339.3 kJ mol¯¹

-221.1 kJ mol¯¹

-523.3 kJ mol¯¹

60. Reaction in which heat is evolved

Endothermic

Exothermic

Non-spontaneous

Spontaneous

61. 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

Zero

40 kJ

62. 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

63. 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

+70 calories

70960 calories

71030 calories

64. Most of the thermodynamic parameters are

State function

System

Phase

Surrounding

65. Total energy of a system is

P.E, + K.E.

P.E, + mechanical energy

K.E, + heat energy

P.E. + heat energy

66. Mechanical work is especially important in systems that contain

Solid-liquid

Gases

Solid-solid

Liquid-liquid

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

None of these

Thermal capacity

Specific heat

Water equivalent

68. Which one is not state function?

Work

Gibbs free energy

Internal energy

Enthalpy

69. 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

70. 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

395 KJ/mole

190 KJ/mole

-27 KJ/mole

71. 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

72. 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

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

Stoichiometry

Kinetics

Thermodynamics

Thermochemistry

74. An adiabatic expansion of an ideal gas always has

∆H = 0

Decrease in temperature

Q = 0

W = 0

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

Watt

Calorie

None of these

Joules

Page 4 of 5

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

Copper calorimeter

Bomb calorimeter

All above

Glass calorimeter

77. 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

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

It is reversible

It is irreversible

It is not irreversible

None of these

79. Enthalpy of a reaction can be measured by

Glass calorimeter

Manometer

Thermometer

Barometer

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

Graphite has more energy than diamond

Graphite is more stable than diamond

Both are equally stable

Stability cannot to predicated

81. In order to decompose 9 g of water 142.5 kJ of heat is required. Hence enthalpy of formation of water is

+285 kJ

+142.5 kJ

-285 kJ

-142.5 kJ

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

Chemical property

State function

Physical property

Energy of the system

83. 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

Non-spontaneous

Irreversible

84. 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

-22 kcal

-44 kcal

-11 kcal

-88 kcal

85. In general, for exothermic reactions to be spontaneous

Temperature should be zero

Temperature has no effect

Temperature should be high

Temperature should be low

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

Free energy change

Entropy change

Enthalpy change

Internal energy change

87. Which one is not a state function?

Enthalpy

Work

Gibbs free energy

Internal energy

88. 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

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

Zeroth law

First law

Second law

Third law

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

Monometer

Bomb Calorimeter

Glass Calorimeter

Thermometer

91. 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

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

Decrease of entropy

Decrease of free energy

Increase of free energy

Increase of enthalpy

93. 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

21.98

2.198

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

-231.6 kcal mol¯¹

+21.4 kcal mol¯¹

+64.8 kcal mol¯¹

-94.0 kcal mol¯¹

95. A spontaneous change means

No energy change

A lowering of energy

A lowering of free energy

An increase in internal energy

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

Photochemistry

Kinetics

Thermodynamics

Thermochemistry

97. 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

-112 kJ mol¯¹

-668 kJ mol¯¹

668 kJ mol¯¹

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

Heat of neutralization

Heat of combustion

Heat of sublimation

Heat of reaction

99. 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

1.7 kJ

28.5 kJ

45.7 kJ

100. Which type of reactions cannot occur spontaneously?

Exothermic

Both a and b

Neither

Endothermic

Page 5 of 5

101. Unit of heat in S.I system is

Cal

Kcal

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

Thermochemistry

Mechanics

Thermodynamics

Chemical kinetics

103. 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

Hat of formation

Heat of neutralization

Heat of combustion

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

Endothermic

Spontaneous

Exothermic

Non-spontaneous

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

Joule

Electron vol

Calorie

Erg

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

10.0 R

0.1 R

100.0 R

2.303 R

107. 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

108. 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

2.4 K

1.2 K

4.8 K

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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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