Thermo-Chemistry Online Mcqs Test

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Question 1

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

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ mol¯¹

Answer

Joule deg¯¹ Kg¯¹

Answer

Joule deg¯¹ atom¯¹

Question 2

2. Total energy of a system is

Answer

P.E + mechanical energy

Answer

K.E + heat energy

Answer

P.E + heat energy

Question 3

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

Answer

Electron – volt

Question 4

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

Answer

Glass Calorimeter

Answer

Thermometer

Answer

Bomb Calorimeter

Question 5

5. Free energy change for a reversible process is:

Answer

Unpredictable

Answer

Equal to zero

Question 6

6. 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

Question 7

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

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 8

8. 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

Answer

9.75 JK¯¹

Answer

11.272 JK¯¹

Answer

Insufficient data

Answer

2.33 JK¯¹

Question 9

9. 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 neutralization

Answer

Enthalpy of reaction

Answer

Heat of combustion

Question 10

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

Answer

Heat of combustion

Answer

Heat of sublimation

Answer

Heat of neutralization

Answer

Heat of reaction

Question 11

11. Mechanical work is especially important in systems that contain

Answer

Liquid-liquid

Answer

Solid-liquid

Answer

Solid-solid

Question 12

12. Unit of heat in S.I system is

Question 13

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

Answer

Chemical process

Answer

Biochemical process

Answer

Endothermic process

Answer

Physical process

Question 14

14. 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

70960 calories

Answer

+70 calories

Answer

71030 calories

Question 15

15. 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)

Question 16

16. Hess’s law deals with

Answer

Changes in heat or reaction

Answer

Influence of pressure on volume of a gas

Answer

Rate of reaction

Answer

Equilibrium constant

Question 17

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

Answer

Thermal capacity

Answer

Specific heat

Answer

None of these

Answer

Water equivalent

Question 18

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

Answer

Isothermal

Question 19

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

Question 20

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

Answer

1 kg H₂O

Answer

4 kg H₂O

Answer

2 kg H₂O

Answer

3 kg H₂O

Question 21

21. Enthalpy of a reaction can be measured by

Answer

Thermometer

Answer

Glass calorimeter

Question 22

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

Answer

Are at a higher temperature than the products

Answer

Have less energy than the products

Answer

Have the same energy as the products

Answer

Have more energy than the products

Question 23

23. 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

-523.3 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Answer

-221.1 kJ mol¯¹

Answer

-439.3 kJ mol¯¹

Question 24

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

Answer

Decrease of entropy

Answer

Decrease of free energy

Answer

Increase of free energy

Answer

Increase of enthalpy

Question 25

25. 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

Question 26

26. Most of the thermodynamic parameters are

Answer

Surrounding

Answer

State function

Question 27

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

Answer

Combustion

Answer

Neutralization

Answer

Thermal decomposition

Answer

Respiration

Question 28

28. 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

Water will freeze

Answer

Water will vaporize

Answer

Ice will sublime

Answer

Ice will melt

Question 29

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

Question 30

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

Answer

The energy change in a cyclic process is not zero

Answer

The lattice energy of the crystalline substances can be calculated easily

Answer

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

Answer

Born Haber cycle is different from Hess’s law

Question 31

31. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 32

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

Answer

Endothermic

Answer

Photochemical

Answer

Exothermic

Question 33

33. In endothermic reactions, the heat content of the

Answer

Products is more than that of reactants

Answer

Reactants and products are equal

Answer

Reactants is more than that of products

Answer

Both a and b

Question 34

34. If internal energy of a system is increased

Answer

Change in state of system can occur

Answer

Chemical reaction can take place

Answer

Temperature of the system may rise

Question 35

35. 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 36

36. All of the following are state function except

Question 37

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

Answer

Thermochemistry

Answer

Thermodynamics

Answer

Stoichiometry

Question 38

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

Answer

Temperature

Question 39

39. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Answer

2 x 57.3 kJ

Answer

Cannot be predicted

Question 40

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

Answer

Both are equally stable

Answer

Graphite is more stable than diamond

Answer

Graphite has more energy than diamond

Answer

Stability cannot to predicated

Question 41

41. 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 42

42. 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 43

43. 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

Release of 218 kcal of energy

Answer

Absorption of 218 kcal of energy

Answer

Unpredictable

Answer

Release of 109 kcal of energy

Question 44

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

Answer

Remains constant

Answer

Remains same

Question 45

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

Answer

Enthalpy change

Answer

Entropy change

Answer

Free energy change

Answer

Internal energy change

Question 46

46. 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 47

47. Two fundamental ways to transfer energy are

Answer

Pressure and volume

Answer

Pressure and temperature

Answer

Heat and work

Answer

Heat and volume

Question 48

48. Evaporation of water is

Answer

An exothermic change

Answer

An endothermic change

Answer

A process where no heat changes occur

Answer

A process accompanied by chemical reaction

Question 49

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

Answer

Burning of coal is and endothermic process

Answer

Burning of coal in air releases large amount of energy

Answer

Coal and air react giving a reversible reaction

Answer

None of these

Question 50

50. When a bond breaks

Answer

Heat is absorbed

Answer

No change in heat contents takes place

Answer

Temperature increases

Answer

Heat is evolved

Question 51

51. Total energy of a system is

Answer

P.E. + heat energy

Answer

K.E, + heat energy

Answer

P.E, + mechanical energy

Answer

P.E, + K.E.

Question 52

52. Which one is not a state function?

Answer

Internal energy

Answer

Gibbs free energy

Question 53

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

Answer

None of these

Question 54

54. The law of Lavoisier and Laplace illustrates

Answer

The principle of conservation of matter

Answer

Equivalent of mechanical and chemical energy

Answer

The principle of conservation of energy

Answer

Equivalence of mechanical and thermal energy

Question 55

55. Calorie is equivalent to

Question 56

56. 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 57

57. The reaction is spontaneous if the cell potential is

Question 58

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

Answer

Second law

Answer

Zeroth law

Question 59

59. A spontaneous change means

Answer

An increase in internal energy

Answer

A lowering of free energy

Answer

A lowering of energy

Answer

No energy change

Question 60

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

Answer

∆E = q + w

Answer

Q = m x X x ∆ T

Answer

P∆V + nRT

Answer

∆H = ∆E + P∆V

Question 61

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

Answer

Temperature and pressure

Answer

Temperature and volume

Answer

Energy and volume

Answer

Pressure and volume

Question 62

62. The enthalpy of formation of carbon monoxide will be

Answer

2x – y/2

Answer

Y – 2x/2

Question 63

63. Most of the reactions which give stable products are

Answer

Isothermal

Answer

Exothermic

Answer

Endothermic

Answer

None of these

Question 64

64. 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)

Answer 168

Bomb calorimeter

Answer 169

Copper calorimeter

Answer 170

Glass calorimeter

Answer 171

Burning of carbon

Answer 172

Making of chemical bond

Answer 173

All of these

Answer 174

Breaking of chemical bonds

Answer 175

Thermodynamics

Answer 176

Thermochemistry

Answer 177

Chemical kinetics

Answer 178

Surrounding

Answer 179

State function

Answer 180

Any substance

Answer 181

Endothermic

Answer 182

Spontaneous

Answer 183

Exothermic

Answer 184

Non-spontaneous

Answer 185

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

Answer 186

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

Answer 187

Work done is independent of its path

Answer 188

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

Answer 189

Energy of the system

Answer 190

Chemical property

Answer 191

Physical property

Answer 192

State function

Answer 193

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

Answer 194

It has a large – ve value for the entropy change

Answer 195

It has small + ve value for enthalpy change

Answer 196

It has a large + ve value for enthalpy change

Answer 197

Hess’s law

Answer 198

Charles’s law

Answer 199

Henry’s law

Answer 200

Graham’s law

Answer 201

Endothermic

Answer 202

Exothermic

Answer 203

Both a and b

Answer 204

Decomposition

Answer 205

Irreversible process

Answer 206

None of these

Answer 207

Spontaneous process

Answer 208

Non spontaneous

Answer 209

HF and HCl are endothermic compounds

Answer 210

HCl is more stable than HF

Answer 211

HF is more stable than HCl

Answer 212

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

Answer 213

It is not irreversible

Answer 214

It is reversible

Answer 215

None of these

Answer 216

It is irreversible

Answer 217

Electron vol

Answer 218

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

Answer 219

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

Answer 220

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

Answer 221

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

Answer 222

Exothermic

Answer 223

Endothermic

Answer 224

Spontaneous

Answer 225

Non-spontaneous

Answer 226

Non-spontaneous

Answer 227

Exothermic

Answer 228

Spontaneous

Answer 229

Endothermic

Answer 230

Neutralization is always exothermic

Answer 231

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

Answer 232

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

Answer 233

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer 234

386 KJ/mole

Answer 235

190 KJ/mole

Answer 236

-27 KJ/mole

Answer 237

395 KJ/mole

Answer 238

Both a and b

Answer 239

Endothermic

Answer 240

Exothermic

Answer 241

Electron – volt

Answer 242

Temperature of the system may rise

Answer 243

Chemical reaction may take place

Answer 244

Change in state of the system is increased

Answer 245

Pressure and temperature

Answer 246

Heat and volume

Answer 247

Pressure and volume

Answer 248

Heat and work

Answer 249

-94.0 kcal mol¯¹

Answer 250

+64.8 kcal mol¯¹

Answer 251

+21.4 kcal mol¯¹

Answer 252

-231.6 kcal mol¯¹

Answer 253

Decrease in temperature

Answer 254

668 kJ mol¯¹

Answer 255

-668 kJ mol¯¹

Answer 256

-112 kJ mol¯¹

Answer 257

112 kJ mol¯¹

Answer 258

Internal energy

Answer 259

Gibbs free energy

Answer 260

∆ H must be negative

Answer 261

∆ H must be zero

Answer 262

∆ H must be unity

Answer 263

∆ H must be positive

Answer 264

Temperature should be high

Answer 265

Temperature should be low

Answer 266

Temperature has no effect

Answer 267

Temperature should be zero

Answer 268

Heat is absorbed

Answer 269

Heat is converted into mechanical work

Answer 270

Heat is evolved

Answer 271

Heat is converted into electricity

Answer 272

None of these

Answer 273

Not change

Answer 274

Reversible

Answer 275

Spontaneous

Answer 276

Non-spontaneous

Answer 277

Irreversible

Answer 278

Surrounding

Answer 279

Henry’s law

Answer 280

Hess’s law

Answer 281

Graham’s law

Answer 282

Boyle’s law

Answer 283

Photochemistry

Answer 284

Thermodynamics

Answer 285

Thermochemistry

Answer 286

Bond length

Answer 287

Bond strength

Answer 288

None of these

Answer 289

Bond energy

Answer 290

∆H = ∆E – d

Answer 291

∆H = ∆E + Pv

Answer 292

∆H = ∆E – PV

Answer 293

∆H = ∆E + d

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