Thermo-Chemistry Online Mcqs Test

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Question 1

1. If internal energy of the system is increased

Answer

Chemical reaction may take place

Answer

Temperature of the system may rise

Answer

Change in state of the system is increased

Question 2

2. 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 3

3. 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 4

4. The law of Lavoisier and Laplace illustrates

Answer

Equivalence of mechanical and thermal energy

Answer

The principle of conservation of matter

Answer

Equivalent of mechanical and chemical energy

Answer

The principle of conservation of energy

Question 5

5. A spontaneous change means

Answer

No energy change

Answer

An increase in internal energy

Answer

A lowering of energy

Answer

A lowering of free energy

Question 6

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

Answer

Pressure and volume

Answer

Temperature and volume

Answer

Energy and volume

Answer

Temperature and pressure

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. 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

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

Answer

The lattice energy of the crystalline substances can be calculated easily

Question 9

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

Question 10

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

Answer

Any substance

Answer

Surrounding

Answer

State function

Question 11

11. Unit of heat is SI system is

Question 12

12. Hess’s law deals with

Answer

Influence of pressure on volume of a gas

Answer

Changes in heat or reaction

Answer

Equilibrium constant

Answer

Rate of reaction

Question 13

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

Answer

Rotational motion

Answer

Vibrational motion

Answer

Translational motion

Answer

The sum of all motions which are possible

Question 14

14. 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 15

15. Which of the following is not correct?

Answer

Neutralization is always exothermic

Answer

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

Answer

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

Answer

Dissolution on NH₄Cl in excess of water is an endothermic process

Question 16

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

Question 17

17. Pumping of water uphill is

Answer

None of these

Answer

Non spontaneous

Answer

Spontaneous process

Answer

Irreversible process

Question 18

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

Answer

Surrounding

Question 19

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

Answer

Free energy change

Answer

Enthalpy change

Answer

Entropy change

Answer

Internal energy change

Question 20

20. Total energy depends upon the state of system

Answer

Free energy of reaction

Answer

Entropy of reaction

Question 21

21. 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 22

22. Which type of reactions cannot occur spontaneously?

Answer

Both a and b

Answer

Exothermic

Answer

Endothermic

Question 23

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

Answer

Joule deg¯¹ atom¯¹

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ Kg¯¹

Answer

Joule deg¯¹ mol¯¹

Question 24

24. If internal energy of a system is increased

Answer

Chemical reaction can take place

Answer

Change in state of system can occur

Answer

Temperature of the system may rise

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

Spontaneous

Answer

Reversible

Answer

Irreversible

Question 26

26. The enthalpy of formation of carbon monoxide will be

Answer

Y – 2x/2

Answer

2x – y/2

Question 27

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

Question 28

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

Answer

Thermodynamics

Answer

Chemical kinetics

Answer

Thermochemistry

Question 29

29. 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

Hat of formation

Answer

Enthalpy of reaction

Answer

Heat of combustion

Question 30

30. 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 31

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

Answer

State function

Answer

Physical property

Answer

Energy of the system

Answer

Chemical property

Question 32

32. 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 33

33. 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 34

34. 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

668 kJ mol¯¹

Answer

-112 kJ mol¯¹

Answer

112 kJ mol¯¹

Question 35

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

Answer

Stoichiometry

Answer

Thermodynamics

Answer

Thermochemistry

Question 36

36. 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 37

37. Which one is not state function?

Answer

Internal energy

Answer

Gibbs free energy

Question 38

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

Answer

None of these

Question 39

39. 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

Unpredictable

Answer

Absorption of 218 kcal of energy

Answer

Release of 218 kcal of energy

Question 40

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

Answer

+21.4 kcal mol¯¹

Answer

+64.8 kcal mol¯¹

Answer

-94.0 kcal mol¯¹

Answer

-231.6 kcal mol¯¹

Question 41

41. 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 42

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

Answer

Increase of free energy

Answer

Decrease of free energy

Answer

Increase of enthalpy

Answer

Decrease of entropy

Question 43

43. Endothermic changes are indicated through

Answer

Making of chemical bond

Answer

Burning of carbon

Answer

All of these

Answer

Breaking of chemical bonds

Question 44

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

Answer

Second law

Answer

Zeroth law

Question 45

45. When a bond breaks

Answer

Heat is absorbed

Answer

No change in heat contents takes place

Answer

Heat is evolved

Answer

Temperature increases

Question 46

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

Answer

Water equivalent

Answer

Specific heat

Answer

None of these

Answer

Thermal capacity

Question 47

47. 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

-27 KJ/mole

Answer

395 KJ/mole

Answer

190 KJ/mole

Answer

386 KJ/mole

Question 48

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

Answer

Heat of sublimation

Answer

Heat of neutralization

Answer

Heat of combustion

Answer

Heat of reaction

Question 49

49. Which statement describes characteristics of an endothermic reaction?

Answer

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

Answer

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

Question 50

50. In endothermic reactions, the heat content of the

Answer

Reactants is more than that of products

Answer

Both a and b

Answer

Reactants and products are equal

Answer

Products is more than that of reactants

Question 51

51. Total energy of a system is

Answer

P.E + heat energy

Answer

P.E + mechanical energy

Answer

K.E + heat energy

Question 52

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

Answer

None of these

Answer

Not change

Question 53

53. 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

-221.1 kJ mol¯¹

Answer

-523.3 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Answer

-439.3 kJ mol¯¹

Question 54

54. 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

Work done is independent of its path

Answer

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

Answer

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

Question 55

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

Answer

Electron – volt

Question 56

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

Answer

Bond length

Answer

Bond energy

Answer

None of these

Answer

Bond strength

Question 57

57. An endothermic reaction is one in which

Answer

Heat is converted into electricity

Answer

Heat is absorbed

Answer

Heat is evolved

Answer

Heat is converted into mechanical work

Question 58

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

Answer

Combustion

Answer

Thermal decomposition

Answer

Neutralization

Answer

Respiration

Question 59

59. Enthalpy of a reaction can be measured by

Answer

Glass calorimeter

Answer

Thermometer

Question 60

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

Question 61

61. Two fundamental ways to transfer energy are

Answer

Heat and volume

Answer

Heat and work

Answer

Pressure and temperature

Answer

Pressure and volume

Question 62

62. Unit of heat in S.I system is

Question 63

63. 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 64

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

Answer

Isothermal

Answer 171

Henry’s law

Answer 172

Boyle’s law

Answer 173

Graham’s law

Answer 174

Hess’s law

Answer 175

Solid-liquid

Answer 176

Liquid-liquid

Answer 177

Solid-solid

Answer 178

Electron – volt

Answer 179

None of these

Answer 180

Endothermic

Answer 181

Exothermic

Answer 182

Isothermal

Answer 183

An exothermic change

Answer 184

A process where no heat changes occur

Answer 185

An endothermic change

Answer 186

A process accompanied by chemical reaction

Answer 187

11.272 JK¯¹

Answer 188

Insufficient data

Answer 189

9.75 JK¯¹

Answer 190

2.33 JK¯¹

Answer 191

Charles’s law

Answer 192

Hess’s law

Answer 193

Graham’s law

Answer 194

Henry’s law

Answer 195

Endothermic process

Answer 196

Biochemical process

Answer 197

Physical process

Answer 198

Chemical process

Answer 199

Temperature

Answer 200

Pressure and temperature

Answer 201

Pressure and volume

Answer 202

Heat and volume

Answer 203

Heat and work

Answer 204

Internal energy

Answer 205

Gibbs free energy

Answer 206

Thermochemistry

Answer 207

Photochemistry

Answer 208

Thermodynamics

Answer 209

State function

Answer 210

Surrounding

Answer 211

Electron vol

Answer 212

Endothermic

Answer 213

Photochemical

Answer 214

Exothermic

Answer 215

HF is more stable than HCl

Answer 216

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

Answer 217

HF and HCl are endothermic compounds

Answer 218

HCl is more stable than HF

Answer 219

Glass Calorimeter

Answer 220

Thermometer

Answer 221

Bomb Calorimeter

Answer 222

It has a large + ve value for enthalpy change

Answer 223

It has a large – ve value for the entropy change

Answer 224

It has small + ve value for enthalpy change

Answer 225

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

Answer 226

∆H = ∆E – d

Answer 227

∆H = ∆E + Pv

Answer 228

∆H = ∆E – PV

Answer 229

∆H = ∆E + d

Answer 230

It is not irreversible

Answer 231

None of these

Answer 232

It is irreversible

Answer 233

It is reversible

Answer 234

– 68 – 48 + 14

Answer 235

– 68 + 48 – 14

Answer 236

68 + 48 + 14

Answer 237

68 – 48 + 14

Answer 238

Bomb calorimeter

Answer 239

Copper calorimeter

Answer 240

Glass calorimeter

Answer 241

Burning of coal is and endothermic process

Answer 242

None of these

Answer 243

Burning of coal in air releases large amount of energy

Answer 244

Coal and air react giving a reversible reaction

Answer 245

3 kg H₂O

Answer 246

2 kg H₂O

Answer 247

4 kg H₂O

Answer 248

1 kg H₂O

Answer 249

Non-spontaneous

Answer 250

Exothermic

Answer 251

Spontaneous

Answer 252

Endothermic

Answer 253

Decomposition

Answer 254

Exothermic

Answer 255

Both a and b

Answer 256

Endothermic

Answer 257

Both are equally stable

Answer 258

Graphite has more energy than diamond

Answer 259

Graphite is more stable than diamond

Answer 260

Stability cannot to predicated

Answer 261

Q = m x X x ∆ T

Answer 262

P∆V + nRT

Answer 263

∆E = q + w

Answer 264

∆H = ∆E + P∆V

Answer 265

Unpredictable

Answer 266

Equal to zero

Answer 267

Remains constant

Answer 268

Remains same

Answer 269

Decrease in temperature

Answer 270

+70 calories

Answer 271

71030 calories

Answer 272

70960 calories

Answer 273

-70 calories

Answer 274

∆ H must be unity

Answer 275

∆ H must be zero

Answer 276

∆ H must be positive

Answer 277

∆ H must be negative

Answer 278

Spontaneous

Answer 279

Non-spontaneous

Answer 280

Endothermic

Answer 281

Exothermic

Answer 282

Endothermic

Answer 283

Non-spontaneous

Answer 284

Exothermic

Answer 285

Spontaneous

Answer 286

P.E, + mechanical energy

Answer 287

P.E. + heat energy

Answer 288

P.E, + K.E.

Answer 289

K.E, + heat energy

Answer 290

Temperature should be zero

Answer 291

Temperature should be high

Answer 292

Temperature should be low

Answer 293

Temperature has no effect

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