Thermo-Chemistry Online Mcqs Test

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Question 1

1. 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

71030 calories

Answer

+70 calories

Answer

70960 calories

Question 2

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

Answer

Translational motion

Answer

The sum of all motions which are possible

Answer

Rotational motion

Answer

Vibrational motion

Question 3

3. 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 4

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

Answer

Glass Calorimeter

Answer

Bomb Calorimeter

Answer

Thermometer

Question 5

5. Which statement describes characteristics of an endothermic reaction?

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 less potential energy than the reactants

Answer

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

Question 6

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

Answer

State function

Answer

Any substance

Answer

Surrounding

Question 7

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

Question 8

8. 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

Question 9

9. 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 10

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

Answer

Pressure and volume

Answer

Temperature and pressure

Answer

Energy and volume

Answer

Temperature and volume

Question 11

11. 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 12

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

Answer

∆H = ∆E – PV

Answer

∆H = ∆E – d

Answer

∆H = ∆E + d

Answer

∆H = ∆E + Pv

Question 13

13. 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 14

14. Unit of heat in S.I system is

Question 15

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

Answer

Second law

Answer

Zeroth law

Question 16

16. 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 vaporize

Answer

Ice will sublime

Answer

Ice will melt

Answer

Water will freeze

Question 17

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

Answer

The lattice energy of the crystalline substances can be calculated easily

Answer

Born Haber cycle is different from Hess’s law

Answer

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

Answer

The energy change in a cyclic process is not zero

Question 18

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

Answer

Heat of neutralization

Answer

Heat of combustion

Answer

Hat of formation

Answer

Enthalpy of reaction

Question 19

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

Answer

Chemical process

Answer

Physical process

Answer

Biochemical process

Answer

Endothermic process

Question 20

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

Answer

Isothermal

Question 21

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

Answer

∆H = ∆E + P∆V

Answer

P∆V + nRT

Answer

∆E = q + w

Answer

Q = m x X x ∆ T

Question 22

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

Answer

+21.4 kcal mol¯¹

Answer

-94.0 kcal mol¯¹

Answer

-231.6 kcal mol¯¹

Answer

+64.8 kcal mol¯¹

Question 23

23. 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 24

24. 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

-112 kJ mol¯¹

Answer

112 kJ mol¯¹

Answer

668 kJ mol¯¹

Answer

-668 kJ mol¯¹

Question 25

25. 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

Answer

Non-spontaneous

Answer

Reversible

Answer

Irreversible

Answer

Spontaneous

Question 26

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

Answer

Thermochemistry

Answer

Stoichiometry

Answer

Thermodynamics

Question 27

27. Unit of heat is SI system is

Question 28

28. 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

386 KJ/mole

Answer

395 KJ/mole

Answer

-27 KJ/mole

Answer

190 KJ/mole

Question 29

29. 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 30

30. Most of the reactions which give stable products are

Answer

Isothermal

Answer

Endothermic

Answer

None of these

Answer

Exothermic

Question 31

31. Which type of reactions cannot occur spontaneously?

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 32

32. Total energy of a system is

Answer

K.E + heat energy

Answer

P.E + mechanical energy

Answer

P.E + heat energy

Question 33

33. In general, for exothermic reactions to be spontaneous

Answer

Temperature should be zero

Answer

Temperature should be high

Answer

Temperature should be low

Answer

Temperature has no effect

Question 34

34. Reaction in which heat is evolved

Answer

Spontaneous

Answer

Exothermic

Answer

Non-spontaneous

Answer

Endothermic

Question 35

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

Answer

Have more energy than the products

Answer

Are at a higher temperature than the products

Answer

Have less energy than the products

Answer

Have the same energy as the products

Question 36

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

Answer

Graham’s law

Answer

Hess’s law

Answer

Boyle’s law

Answer

Henry’s law

Question 37

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

Answer

Spontaneous

Answer

Exothermic

Answer

Non-spontaneous

Answer

Endothermic

Question 38

38. 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 109 kcal of energy

Answer

Absorption of 218 kcal of energy

Answer

Release of 218 kcal of energy

Answer

Unpredictable

Question 39

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

Answer

1 kg H₂O

Answer

3 kg H₂O

Answer

2 kg H₂O

Answer

4 kg H₂O

Question 40

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

Question 41

41. Two fundamental ways to transfer energy are

Answer

Heat and volume

Answer

Heat and work

Answer

Pressure and volume

Answer

Pressure and temperature

Question 42

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

Answer

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

Answer

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

Answer

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

Answer

Work done is independent of its path

Question 43

43. Hess’s law deals with

Answer

Equilibrium constant

Answer

Changes in heat or reaction

Answer

Influence of pressure on volume of a gas

Answer

Rate of reaction

Question 44

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

Answer

Endothermic

Answer

Photochemical

Answer

Exothermic

Question 45

45. 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 46

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

Answer

Coal and air react giving a reversible reaction

Answer

Burning of coal is and endothermic process

Answer

None of these

Answer

Burning of coal in air releases large amount of energy

Question 47

47. Two fundamental ways to transfer energy are

Answer

Heat and work

Answer

Pressure and temperature

Answer

Heat and volume

Answer

Pressure and volume

Question 48

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

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ atom¯¹

Answer

Joule deg¯¹ mol¯¹

Answer

Joule deg¯¹ Kg¯¹

Question 49

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

Answer

Electron – volt

Question 50

50. Enthalpy of a reaction can be measured by

Answer

Glass calorimeter

Answer

Thermometer

Question 51

51. The reaction is spontaneous if the cell potential is

Question 52

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

Answer

Combustion

Answer

Neutralization

Answer

Thermal decomposition

Answer

Respiration

Question 53

53. Total energy of a system is

Answer

P.E, + K.E.

Answer

P.E. + heat energy

Answer

K.E, + heat energy

Answer

P.E, + mechanical energy

Question 54

54. 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

11.272 JK¯¹

Answer

Insufficient data

Answer

2.33 JK¯¹

Answer

9.75 JK¯¹

Question 55

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

Answer

Hess’s law

Answer

Graham’s law

Answer

Henry’s law

Answer

Charles’s law

Question 56

56. 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 57

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

Answer

None of these

Answer

It is irreversible

Answer

It is reversible

Answer

It is not irreversible

Question 58

58. Most of the thermodynamic parameters are

Answer

State function

Answer

Surrounding

Question 59

59. Pumping of water uphill is

Answer

Spontaneous process

Answer

Non spontaneous

Answer

Irreversible process

Answer

None of these

Question 60

60. 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 61

61. Which one is not state function?

Answer

Internal energy

Answer

Gibbs free energy

Question 62

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

Answer

Bond length

Answer

Bond strength

Answer

None of these

Answer

Bond energy

Question 63

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

Answer

Decomposition

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 64

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

Answer

Copper calorimeter

Answer

Bomb calorimeter

Answer

Glass calorimeter

Answer 187

Y – 2x/2

Answer 188

2x – y/2

Answer 189

Photochemistry

Answer 190

Thermochemistry

Answer 191

Thermodynamics

Answer 192

Solid-liquid

Answer 193

Solid-solid

Answer 194

Liquid-liquid

Answer 195

Non-spontaneous

Answer 196

Exothermic

Answer 197

Spontaneous

Answer 198

Endothermic

Answer 199

-221.1 kJ mol¯¹

Answer 200

-523.3 kJ mol¯¹

Answer 201

-339.3 kJ mol¯¹

Answer 202

-439.3 kJ mol¯¹

Answer 203

A lowering of energy

Answer 204

An increase in internal energy

Answer 205

No energy change

Answer 206

A lowering of free energy

Answer 207

Gibbs free energy

Answer 208

Internal energy

Answer 209

Breaking of chemical bonds

Answer 210

All of these

Answer 211

Burning of carbon

Answer 212

Making of chemical bond

Answer 213

Heat is evolved

Answer 214

Heat is absorbed

Answer 215

Temperature increases

Answer 216

No change in heat contents takes place

Answer 217

2 x 57.3 kJ

Answer 218

Cannot be predicted

Answer 219

None of these

Answer 220

Reactants and products are equal

Answer 221

Both a and b

Answer 222

Products is more than that of reactants

Answer 223

Reactants is more than that of products

Answer 224

Heat is converted into mechanical work

Answer 225

Heat is evolved

Answer 226

Heat is absorbed

Answer 227

Heat is converted into electricity

Answer 228

Not change

Answer 229

None of these

Answer 230

∆ H must be zero

Answer 231

∆ H must be unity

Answer 232

∆ H must be negative

Answer 233

∆ H must be positive

Answer 234

Equal to zero

Answer 235

Unpredictable

Answer 236

Surrounding

Answer 237

Electron vol

Answer 238

Enthalpy change

Answer 239

Free energy change

Answer 240

Internal energy change

Answer 241

Entropy change

Answer 242

Increase of free energy

Answer 243

Increase of enthalpy

Answer 244

Decrease of free energy

Answer 245

Decrease of entropy

Answer 246

Remains same

Answer 247

Remains constant

Answer 248

Stability cannot to predicated

Answer 249

Graphite is more stable than diamond

Answer 250

Both are equally stable

Answer 251

Graphite has more energy than diamond

Answer 252

Free energy of reaction

Answer 253

Entropy of reaction

Answer 254

Decrease in temperature

Answer 255

Temperature

Answer 256

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

Answer 257

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

Answer 258

Neutralization is always exothermic

Answer 259

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer 260

Heat of sublimation

Answer 261

Heat of neutralization

Answer 262

Heat of reaction

Answer 263

Heat of combustion

Answer 264

Equivalence of mechanical and thermal energy

Answer 265

Equivalent of mechanical and chemical energy

Answer 266

The principle of conservation of matter

Answer 267

The principle of conservation of energy

Answer 268

State function

Answer 269

Physical property

Answer 270

Chemical property

Answer 271

Energy of the system

Answer 272

Endothermic

Answer 273

Both a and b

Answer 274

Exothermic

Answer 275

It has a large + ve value for enthalpy change

Answer 276

It has a large – ve value for the entropy change

Answer 277

It has small + ve value for enthalpy change

Answer 278

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

Answer 279

Thermochemistry

Answer 280

Chemical kinetics

Answer 281

Thermodynamics

Answer 282

Chemical reaction may take place

Answer 283

Change in state of the system is increased

Answer 284

Temperature of the system may rise

Answer 285

Electron – volt

Answer 286

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

Answer 287

HF and HCl are endothermic compounds

Answer 288

HF is more stable than HCl

Answer 289

HCl is more stable than HF

Answer 290

Specific heat

Answer 291

Water equivalent

Answer 292

None of these

Answer 293

Thermal capacity

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