Home/MDCAT/MDCAT Thermo-Chemistry and Energetics of Chemical Reactions Test Online

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.
Test Helpful For:	MDCAT Entry Test Chemistry Online Test Interview Questions about Chemisttry All Universities Entrance Test Recruitments Tests

MDCAT Chemistry Thermochemistry Test

Please wait...

Page 1 of 5

Chemistry

1. Reaction in which heat is evolved

Spontaneous

Exothermic

Endothermic

Non-spontaneous

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

Exothermic

Endothermic

Synthesis

Both a and b

3. 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

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

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

Temperature

Volume

Pressure

Density

6. A spontaneous change means

An increase in internal energy

No energy change

A lowering of free energy

A lowering of energy

7. In endothermic reactions, the heat content of the

Both a and b

Reactants is more than that of products

Products is more than that of reactants

Reactants and products are equal

8. When a bond breaks

Temperature increases

Heat is evolved

No change in heat contents takes place

Heat is absorbed

9. Which one is not state function?

Work

Gibbs free energy

Enthalpy

Internal energy

10. 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 freeze

Water will vaporize

Ice will sublime

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

1 kg H₂O

4 kg H₂O

3 kg H₂O

2 kg H₂O

12. Enthalpy of a reaction can be measured by

Manometer

Glass calorimeter

Thermometer

Barometer

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

Have more energy than the products

Have the same energy as the products

Are at a higher temperature than the products

Have less energy than the products

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

First law

Second law

Zeroth law

Third law

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

State

Phase

Surrounding

System

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

Joule deg¯¹ Kg¯¹

Joule cm¯¹ deg¯¹

Joule deg¯¹ mol¯¹

Joule deg¯¹ atom¯¹

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

Rotational motion

Vibrational motion

Translational motion

The sum of all motions which are possible

18. Unit of heat in S.I system is

Kcal

Cal

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

Thermodynamics

Kinetics

Stoichiometry

Thermochemistry

20. 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

-27 KJ/mole

395 KJ/mole

386 KJ/mole

190 KJ/mole

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

None of these

Bond strength

Bond length

Bond energy

22. 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

+142.5 kJ

-285 kJ

23. Endothermic changes are indicated through

Breaking of chemical bonds

Making of chemical bond

All of these

Burning of carbon

24. The enthalpy of formation of carbon monoxide will be

2x – y/2

Y – 2x/2

Y – 2x

2x – y

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

Kinetics

Thermochemistry

Thermodynamics

Photochemistry

Page 2 of 5

26. 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

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

Hess’s law

Boyle’s law

Henry’s law

Graham’s law

28. Pumping of water uphill is

Spontaneous process

Non spontaneous

None of these

Irreversible process

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

It has a large – ve value for the entropy change

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

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

Glass Calorimeter

Bomb Calorimeter

Thermometer

Monometer

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

Combustion

Neutralization

Thermal decomposition

Respiration

32. Which statement describes characteristics of an endothermic reaction?

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

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

33. 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

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

Isolated

Isothermal

Adiabatic

Closed

35. Total energy depends upon the state of system

Free energy of reaction

Enthalpy

All above

Entropy of reaction

36. Calorie is equivalent to

418.4 J

4.184 J

0.4184 J

41.84 J

37. Hess’s law deals with

Rate of reaction

Changes in heat or reaction

Equilibrium constant

Influence of pressure on volume of a gas

38. 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

39. Total energy of a system is

P.E, + K.E.

P.E. + heat energy

P.E, + mechanical energy

K.E, + heat energy

40. The law of Lavoisier and Laplace illustrates

Equivalence of mechanical and thermal energy

Equivalent of mechanical and chemical energy

The principle of conservation of matter

The principle of conservation of energy

41. In general, for exothermic reactions to be spontaneous

Temperature should be zero

Temperature has no effect

Temperature should be low

Temperature should be high

42. An adiabatic expansion of an ideal gas always has

Q = 0

W = 0

∆H = 0

Decrease in temperature

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

Heat of neutralization

Heat of reaction

Heat of sublimation

Heat of combustion

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

Joules

Calorie

Watt

None of these

45. Most of the reactions which give stable products are

None of these

Endothermic

Isothermal

Exothermic

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

4.8 K

1.2 K

2.4 K

6.6 K

47. Which type of reactions cannot occur spontaneously?

Both a and b

Endothermic

Neither

Exothermic

48. 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

0 J

= - k719

-400J

49. 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)

20 days

50 days

15 days

32 days

50. 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

2.303 R

100.0 R

Page 3 of 5

51. 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

None of these

Coal and air react giving a reversible reaction

Burning of coal is and endothermic process

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

∆H = ∆E + P∆V

P∆V + nRT

∆E = q + w

Q = m x X x ∆ T

53. Unit of heat is SI system is

KCaL

Cal

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

Physical process

Chemical process

Biochemical process

Endothermic process

55. 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?

71030 calories

-70 calories

70960 calories

+70 calories

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

Entropy change

Enthalpy change

Internal energy change

Free energy change

57. 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

58. 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

59. 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 energy change in a cyclic process is not zero

The lattice energy of the crystalline substances can be calculated easily

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

Spontaneous

Exothermic

Non-spontaneous

Endothermic

61. 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

HF and HCl are endothermic compounds

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

HF is more stable than HCl

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

Erg

Joule

Calorie

Electron vol

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

Thermodynamics

Chemical kinetics

Thermochemistry

Mechanics

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

57.3/2 kJ

Cannot be predicted

2 x 57.3 kJ

57.3 kJ

65. Total energy of a system is

P.E + K.E

K.E + heat energy

P.E + heat energy

P.E + mechanical energy

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

All above

Glass calorimeter

Copper calorimeter

Bomb calorimeter

67. 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

68. All of the following are state function except

69. 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

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

Work done is independent of its path

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

Remains same

Increases

Decreases

Remains constant

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

Zero

Positive

Negative

Unity

72. 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

Irreversible

Non-spontaneous

Reversible

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

Decrease of entropy

Increase of enthalpy

Decrease of free energy

Increase of free energy

74. The reaction is spontaneous if the cell potential is

Infinite

Zero

Positive

Negative

75. If internal energy of a system is increased

Temperature of the system may rise

Chemical reaction can take place

Change in state of system can occur

All

Page 4 of 5

76. 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 218 kcal of energy

Release of 109 kcal of energy

77. If internal energy of the system is increased

Chemical reaction may take place

All

Change in state of the system is increased

Temperature of the system may rise

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

∆H = ∆E – d

∆H = ∆E + d

∆H = ∆E – PV

∆H = ∆E + Pv

79. The amount of heat which is involved during the completion of a chemical reaction at 25°C and 1 atmospheric pressure is called

Hat of formation

Enthalpy of reaction

Heat of neutralization

Heat of combustion

80. Which of the following is not correct?

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

Neutralization is always exothermic

Dissolution on NH₄Cl in excess of water is an endothermic process

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

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

Non-spontaneous

Endothermic

Exothermic

Spontaneous

82. Evaporation of water is

A process where no heat changes occur

An endothermic change

A process accompanied by chemical reaction

An exothermic change

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

Thermal capacity

Water equivalent

Specific heat

None of these

84. An endothermic reaction is one in which

Heat is converted into mechanical work

Heat is absorbed

Heat is converted into electricity

Heat is evolved

85. Mechanical work is especially important in systems that contain

Gases

Solid-solid

Liquid-liquid

Solid-liquid

86. 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

-676.5 kJ

676.5 kJ

-110.5 kJ

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

Stability cannot to predicated

Graphite is more stable than diamond

Graphite has more energy than diamond

Both are equally stable

88. 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

2.198

21.98

2.013

89. 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

-88 kcal

-22 kcal

-44 kcal

-11 kcal

90. Free energy change for a reversible process is:

Unpredictable

Equal to zero

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

None of these

Be double

Be half

Not change

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

Joule

Calorie

Electron – volt

Erg

93. 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

11.272 JK¯¹

9.75 JK¯¹

94. Two fundamental ways to transfer energy are

Heat and volume

Heat and work

Pressure and volume

Pressure and temperature

95. Two fundamental ways to transfer energy are

Heat and work

Heat and volume

Pressure and volume

Pressure and temperature

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

It is reversible

None of these

It is not irreversible

It is irreversible

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

Both a and b

Decomposition

Exothermic

Endothermic

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

System

Any substance

State function

Surrounding

99. 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

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

Temperature and pressure

Temperature and volume

Pressure and volume

Energy and volume

Page 5 of 5

101. For a reaction to occur spontaneously

∆ H must be zero

∆ H must be negative

∆ H must be positive

∆ H must be unity

102. 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

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

Joule

Electron – volt

Erg

Calorie

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

Exothermic

Explosive

Endothermic

Photochemical

105. Most of the thermodynamic parameters are

Surrounding

State function

Phase

System

106. Which one is not a state function?

Work

Gibbs free energy

Internal energy

Enthalpy

107. 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

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

Graham’s law

Hess’s law

Charles’s law

Henry’s law

You Can Learn and Gain more Knowledge through our Online Quiz and Testing system Just Search your desired Preparation subject at Gotest.

MDCAT Chemistry Gases Test Online
MDCAT Chemistry Industrial Chemistry Test Online
MDCAT Chemistry Aldehydes and Ketones Test Online
MDCAT Physics Alternating Current Test Online
MDCAT Physics Fluid Dynamics Test Online
MDCAT Physics Vactors And Equilibrium Test Online
MDCAT Chemistry Alcohols And Phenols Test Online
MDCAT Chemistry Alkyl Halides Test Online
MDCAT Biology Biotechnology Online Test
MDCAT Biology Homeostasis Online Test

Mustansar KhanLast Updated: May 24, 2025

Facebook Twitter Reddit WhatsApp Share via Email Print

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

You Might Also Like

Mustansar Khan

Leave a Reply Cancel reply

Chemistry Thermochemistry MCQS Online Test

MDCAT Chemistry Thermochemistry Chapter Online Test

MDCAT Chemistry Thermochemistry Test

Chemistry

You Might Also Like

Mustansar Khan

Your Related

Sindh Medical Universities MDCAT Test Result 2025 Answer Keys

MDCAT Biology Life process in Animals & Plants Test Online

Nishtar Medical College NMC Multan Entry Test 2025 Result & Answer Key

MDCAT English Antonyms Online Test 8

Rawalpindi Medical College RMC Entry Test Result 2025

MDCAT English Active & Passive Voice Test 3 Online

Leave a Reply Cancel reply