Thermo-Chemistry Online Mcqs Test

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Question 1

1. Reaction in which heat is evolved

Answer

Exothermic

Answer

Endothermic

Answer

Spontaneous

Answer

Non-spontaneous

Question 2

2. 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

Question 3

3. 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

Answer

-668 kJ mol¯¹

Answer

112 kJ mol¯¹

Answer

668 kJ mol¯¹

Answer

-112 kJ mol¯¹

Question 4

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

Answer

Absorption of 218 kcal of energy

Answer

Release of 109 kcal of energy

Answer

Unpredictable

Answer

Release of 218 kcal of energy

Question 5

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

Answer

Spontaneous

Answer

Non-spontaneous

Answer

Endothermic

Answer

Exothermic

Question 6

6. If internal energy of the system is increased

Answer

Change in state of the system is increased

Answer

Temperature of the system may rise

Answer

Chemical reaction may take place

Question 7

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

Answer

Both a and b

Answer

Endothermic

Answer

Decomposition

Answer

Exothermic

Question 8

8. In general, for exothermic reactions to be spontaneous

Answer

Temperature should be high

Answer

Temperature has no effect

Answer

Temperature should be zero

Answer

Temperature should be low

Question 9

9. 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)

Question 10

10. An adiabatic expansion of an ideal gas always has

Answer

Decrease in temperature

Question 11

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

Answer

-231.6 kcal mol¯¹

Answer

+64.8 kcal mol¯¹

Answer

-94.0 kcal mol¯¹

Answer

+21.4 kcal mol¯¹

Question 12

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

Answer

Endothermic

Answer

Photochemical

Answer

Exothermic

Question 13

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

Answer

Hess’s law

Answer

Graham’s law

Answer

Henry’s law

Answer

Boyle’s law

Question 14

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

Question 15

15. 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?

Answer

+70 calories

Answer

-70 calories

Answer

70960 calories

Answer

71030 calories

Question 16

16. When a bond breaks

Answer

Temperature increases

Answer

No change in heat contents takes place

Answer

Heat is absorbed

Answer

Heat is evolved

Question 17

17. Evaporation of water is

Answer

An exothermic change

Answer

A process where no heat changes occur

Answer

A process accompanied by chemical reaction

Answer

An endothermic change

Question 18

18. All of the following are state function except

Question 19

19. Which of the following is not correct?

Answer

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

Answer

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer

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

Answer

Neutralization is always exothermic

Question 20

20. 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

Answer

Ice will sublime

Answer

Water will freeze

Answer

Ice will melt

Answer

Water will vaporize

Question 21

21. Total energy of a system is

Answer

K.E + heat energy

Answer

P.E + heat energy

Answer

P.E + mechanical energy

Question 22

22. 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)

Question 23

23. Which one is not state function?

Answer

Internal energy

Answer

Gibbs free energy

Question 24

24. Most of the thermodynamic parameters are

Answer

State function

Answer

Surrounding

Question 25

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

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 26

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

Answer

Temperature and pressure

Answer

Temperature and volume

Answer

Pressure and volume

Answer

Energy and volume

Question 27

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

Answer

Remains same

Answer

Remains constant

Question 28

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

Answer

Thermal capacity

Answer

None of these

Answer

Specific heat

Answer

Water equivalent

Question 29

29. 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?

Question 30

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

Answer

None of these

Question 31

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

Answer

It is not irreversible

Answer

None of these

Answer

It is reversible

Answer

It is irreversible

Question 32

32. An endothermic reaction is one in which

Answer

Heat is converted into mechanical work

Answer

Heat is evolved

Answer

Heat is converted into electricity

Answer

Heat is absorbed

Question 33

33. Mechanical work is especially important in systems that contain

Answer

Liquid-liquid

Answer

Solid-liquid

Answer

Solid-solid

Question 34

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

Question 35

35. 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

Question 36

36. A spontaneous change means

Answer

No energy change

Answer

An increase in internal energy

Answer

A lowering of free energy

Answer

A lowering of energy

Question 37

37. Which statement describes characteristics of an endothermic reaction?

Answer

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

Answer

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

Answer

The sign of H is positive and the products a have more potential energy than the reactant

Answer

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

Question 38

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

Answer

Electron vol

Question 39

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

Answer

Hat of formation

Answer

Heat of combustion

Answer

Enthalpy of reaction

Answer

Heat of neutralization

Question 40

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

Answer

Exothermic

Answer

Endothermic

Answer

Spontaneous

Answer

Non-spontaneous

Question 41

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

Answer

Second law

Answer

Zeroth law

Question 42

42. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 43

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

Answer

Joule deg¯¹ mol¯¹

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ atom¯¹

Answer

Joule deg¯¹ Kg¯¹

Question 44

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

Answer

Heat of sublimation

Answer

Heat of neutralization

Answer

Heat of reaction

Answer

Heat of combustion

Question 45

45. Most of the reactions which give stable products are

Answer

Isothermal

Answer

Endothermic

Answer

None of these

Answer

Exothermic

Question 46

46. Endothermic changes are indicated through

Answer

Burning of carbon

Answer

Making of chemical bond

Answer

Breaking of chemical bonds

Answer

All of these

Question 47

47. 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

Question 48

48. Form the above data, the standard heat of formation of KOH in kcal mol¯¹ is

Answer

68 + 48 + 14

Answer

– 68 + 48 – 14

Answer

– 68 – 48 + 14

Answer

68 – 48 + 14

Question 49

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

Answer

Decrease of entropy

Answer

Increase of free energy

Answer

Increase of enthalpy

Answer

Decrease of free energy

Question 50

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

Answer

Have the same energy as the products

Answer

Have less energy than the products

Answer

Have more energy than the products

Answer

Are at a higher temperature than the products

Question 51

51. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Answer

Cannot be predicted

Answer

2 x 57.3 kJ

Question 52

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

Answer

Glass calorimeter

Answer

Bomb calorimeter

Answer

Copper calorimeter

Question 53

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

Answer

4 kg H₂O

Answer

3 kg H₂O

Answer

1 kg H₂O

Answer

2 kg H₂O

Question 54

54. Free energy change for a reversible process is:

Answer

Unpredictable

Answer

Equal to zero

Question 55

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

Question 56

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

Answer

Electron – volt

Question 57

57. The law of Lavoisier and Laplace illustrates

Answer

Equivalent of mechanical and chemical energy

Answer

Equivalence of mechanical and thermal energy

Answer

The principle of conservation of matter

Answer

The principle of conservation of energy

Question 58

58. 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

Answer

395 KJ/mole

Answer

-27 KJ/mole

Answer

386 KJ/mole

Answer

190 KJ/mole

Question 59

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

Answer

Rotational motion

Answer

The sum of all motions which are possible

Answer

Vibrational motion

Answer

Translational motion

Question 60

60. 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

Answer

-439.3 kJ mol¯¹

Answer

-221.1 kJ mol¯¹

Answer

-523.3 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Question 61

61. Two fundamental ways to transfer energy are

Answer

Pressure and temperature

Answer

Heat and volume

Answer

Heat and work

Answer

Pressure and volume

Question 62

62. Enthalpy of a reaction can be measured by

Answer

Thermometer

Answer

Glass calorimeter

Question 63

63. In endothermic reactions, the heat content of the

Answer

Reactants is more than that of products

Answer

Products is more than that of reactants

Answer

Both a and b

Answer

Reactants and products are equal

Question 64

64. If internal energy of a system is increased

Answer

Chemical reaction can take place

Answer

Temperature of the system may rise

Answer

Change in state of system can occur

Answer 182

Thermochemistry

Answer 183

Thermodynamics

Answer 184

Photochemistry

Answer 185

Henry’s law

Answer 186

Hess’s law

Answer 187

Charles’s law

Answer 188

Graham’s law

Answer 189

P.E. + heat energy

Answer 190

K.E, + heat energy

Answer 191

P.E, + K.E.

Answer 192

P.E, + mechanical energy

Answer 193

Exothermic

Answer 194

Both a and b

Answer 195

Endothermic

Answer 196

Isothermal

Answer 197

Thermodynamics

Answer 198

Stoichiometry

Answer 199

Thermochemistry

Answer 200

∆H = ∆E + P∆V

Answer 201

Q = m x X x ∆ T

Answer 202

∆E = q + w

Answer 203

P∆V + nRT

Answer 204

Temperature

Answer 205

Burning of coal in air releases large amount of energy

Answer 206

Burning of coal is and endothermic process

Answer 207

Coal and air react giving a reversible reaction

Answer 208

None of these

Answer 209

None of these

Answer 210

Not change

Answer 211

Respiration

Answer 212

Thermal decomposition

Answer 213

Combustion

Answer 214

Neutralization

Answer 215

Influence of pressure on volume of a gas

Answer 216

Changes in heat or reaction

Answer 217

Equilibrium constant

Answer 218

Rate of reaction

Answer 219

None of these

Answer 220

Bond length

Answer 221

Bond energy

Answer 222

Bond strength

Answer 223

Glass Calorimeter

Answer 224

Thermometer

Answer 225

Bomb Calorimeter

Answer 226

Energy of the system

Answer 227

Physical property

Answer 228

Chemical property

Answer 229

State function

Answer 230

Physical process

Answer 231

Biochemical process

Answer 232

Chemical process

Answer 233

Endothermic process

Answer 234

Born Haber cycle is different from Hess’s law

Answer 235

The lattice energy of the crystalline substances can be calculated easily

Answer 236

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

Answer 237

The energy change in a cyclic process is not zero

Answer 238

Non-spontaneous

Answer 239

Reversible

Answer 240

Irreversible

Answer 241

Spontaneous

Answer 242

11.272 JK¯¹

Answer 243

Insufficient data

Answer 244

9.75 JK¯¹

Answer 245

2.33 JK¯¹

Answer 246

∆ H must be zero

Answer 247

∆ H must be unity

Answer 248

∆ H must be negative

Answer 249

∆ H must be positive

Answer 250

Entropy change

Answer 251

Free energy change

Answer 252

Internal energy change

Answer 253

Enthalpy change

Answer 254

Any substance

Answer 255

Surrounding

Answer 256

State function

Answer 257

Surrounding

Answer 258

Internal energy

Answer 259

Gibbs free energy

Answer 260

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

Answer 261

HCl is more stable than HF

Answer 262

HF is more stable than HCl

Answer 263

HF and HCl are endothermic compounds

Answer 264

It has a large – ve value for the entropy change

Answer 265

It has a large + ve value for enthalpy change

Answer 266

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

Answer 267

It has small + ve value for enthalpy change

Answer 268

Stability cannot to predicated

Answer 269

Graphite is more stable than diamond

Answer 270

Graphite has more energy than diamond

Answer 271

Both are equally stable

Answer 272

2x – y/2

Answer 273

Y – 2x/2

Answer 274

Thermodynamics

Answer 275

Thermochemistry

Answer 276

Chemical kinetics

Answer 277

Pressure and volume

Answer 278

Heat and volume

Answer 279

Pressure and temperature

Answer 280

Heat and work

Answer 281

Non spontaneous

Answer 282

Spontaneous process

Answer 283

Irreversible process

Answer 284

None of these

Answer 285

∆H = ∆E + d

Answer 286

∆H = ∆E – d

Answer 287

∆H = ∆E + Pv

Answer 288

∆H = ∆E – PV

Answer 289

Electron – volt

Answer 290

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

Answer 291

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

Answer 292

Work done is independent of its path

Answer 293

One form of energy can be transferred to an equivalent amount of the kind of energy

Total Questions:	108
Time Allowed:	60 Minutes
Total Marks:	108
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