Thermo-Chemistry Online Mcqs Test

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Question 1

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

Answer

Photochemistry

Answer

Thermodynamics

Answer

Thermochemistry

Question 2

2. 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

-339.3 kJ mol¯¹

Answer

-439.3 kJ mol¯¹

Answer

-523.3 kJ mol¯¹

Question 3

3. Which one is not state function?

Answer

Gibbs free energy

Answer

Internal energy

Question 4

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

Answer

Electron – volt

Question 5

5. Unit of heat in S.I system is

Question 6

6. 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 7

7. 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 8

8. 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 energy

Answer

The principle of conservation of matter

Question 9

9. In general, for exothermic reactions to be spontaneous

Answer

Temperature should be zero

Answer

Temperature should be low

Answer

Temperature has no effect

Answer

Temperature should be high

Question 10

10. Total energy of a system is

Answer

K.E + heat energy

Answer

P.E + mechanical energy

Answer

P.E + heat energy

Question 11

11. Two fundamental ways to transfer energy are

Answer

Heat and work

Answer

Pressure and volume

Answer

Pressure and temperature

Answer

Heat and volume

Question 12

12. 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 13

13. When a bond breaks

Answer

Heat is absorbed

Answer

Heat is evolved

Answer

No change in heat contents takes place

Answer

Temperature increases

Question 14

14. 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 15

15. Most of the thermodynamic parameters are

Answer

Surrounding

Answer

State function

Question 16

16. For a reaction to occur spontaneously

Answer

∆ H must be unity

Answer

∆ H must be zero

Answer

∆ H must be negative

Answer

∆ H must be positive

Question 17

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

Answer

Surrounding

Answer

State function

Answer

Any substance

Question 18

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

Answer

Electron vol

Question 19

19. 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 20

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

Answer

Endothermic

Answer

Exothermic

Answer

Both a and b

Question 21

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

Answer

Electron – volt

Question 22

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

Answer

Thermodynamics

Answer

Stoichiometry

Answer

Thermochemistry

Question 23

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

Answer

Joule deg¯¹ mol¯¹

Answer

Joule deg¯¹ Kg¯¹

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ atom¯¹

Question 24

24. An adiabatic expansion of an ideal gas always has

Answer

Decrease in temperature

Question 25

25. 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 26

26. Free energy change for a reversible process is:

Answer

Equal to zero

Answer

Unpredictable

Question 27

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

Answer

Temperature

Question 28

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

Answer

Bond strength

Answer

Bond length

Answer

None of these

Answer

Bond energy

Question 29

29. Which one is not a state function?

Answer

Gibbs free energy

Answer

Internal energy

Question 30

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

Answer

None of these

Answer

Not change

Question 31

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

Question 32

32. Evaporation of water is

Answer

An endothermic change

Answer

A process accompanied by chemical reaction

Answer

A process where no heat changes occur

Answer

An exothermic change

Question 33

33. 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

Spontaneous

Answer

Reversible

Answer

Irreversible

Answer

Non-spontaneous

Question 34

34. Most of the reactions which give stable products are

Answer

Endothermic

Answer

None of these

Answer

Isothermal

Answer

Exothermic

Question 35

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

Question 36

36. Mechanical work is especially important in systems that contain

Answer

Solid-liquid

Answer

Liquid-liquid

Answer

Solid-solid

Question 37

37. Enthalpy of a reaction can be measured by

Answer

Thermometer

Answer

Glass calorimeter

Question 38

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

Answer

Respiration

Answer

Neutralization

Answer

Thermal decomposition

Answer

Combustion

Question 39

39. 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

+64.8 kcal mol¯¹

Answer

-231.6 kcal mol¯¹

Question 40

40. In endothermic reactions, the heat content of the

Answer

Products is more than that of reactants

Answer

Reactants is more than that of products

Answer

Both a and b

Answer

Reactants and products are equal

Question 41

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

Answer

Isothermal

Question 42

42. 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 43

43. The enthalpy of formation of carbon monoxide will be

Answer

2x – y/2

Answer

Y – 2x/2

Question 44

44. 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

-668 kJ mol¯¹

Answer

-112 kJ mol¯¹

Answer

668 kJ mol¯¹

Question 45

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

Answer

Both are equally stable

Answer

Graphite is more stable than diamond

Answer

Stability cannot to predicated

Answer

Graphite has more energy than diamond

Question 46

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

Answer

Energy and volume

Answer

Pressure and volume

Answer

Temperature and pressure

Answer

Temperature and volume

Question 47

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

Answer

It has a large + ve value for enthalpy change

Answer

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

Answer

It has small + ve value for enthalpy change

Answer

It has a large – ve value for the entropy change

Question 48

48. A spontaneous change means

Answer

An increase in internal energy

Answer

A lowering of energy

Answer

A lowering of free energy

Answer

No energy change

Question 49

49. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 50

50. Pumping of water uphill is

Answer

Irreversible process

Answer

Non spontaneous

Answer

None of these

Answer

Spontaneous process

Question 51

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

Answer

Second law

Answer

Zeroth law

Question 52

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

Answer

Surrounding

Question 53

53. The reaction is spontaneous if the cell potential is

Question 54

54. 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 55

55. 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 56

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

Answer

None of these

Answer

Thermal capacity

Answer

Specific heat

Answer

Water equivalent

Question 57

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

Answer

Chemical property

Answer

Physical property

Answer

State function

Answer

Energy of the system

Question 58

58. 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 59

59. 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

Release of 109 kcal of energy

Answer

Absorption of 218 kcal of energy

Answer

Unpredictable

Question 60

60. 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 61

61. 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 62

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

Answer

3 kg H₂O

Answer

4 kg H₂O

Answer

2 kg H₂O

Answer

1 kg H₂O

Question 63

63. Unit of heat is SI system is

Question 64

64. 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

Answer 161

The energy change in a cyclic process is not zero

Answer 162

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

Answer 163

The lattice energy of the crystalline substances can be calculated easily

Answer 164

Born Haber cycle is different from Hess’s law

Answer 165

386 KJ/mole

Answer 166

-27 KJ/mole

Answer 167

190 KJ/mole

Answer 168

395 KJ/mole

Answer 169

Change in state of system can occur

Answer 170

Chemical reaction can take place

Answer 171

Temperature of the system may rise

Answer 172

Glass Calorimeter

Answer 173

Bomb Calorimeter

Answer 174

Thermometer

Answer 175

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

Answer 176

Work done is independent of its path

Answer 177

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

Answer 178

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

Answer 179

None of these

Answer 180

Burning of coal in air releases large amount of energy

Answer 181

Burning of coal is and endothermic process

Answer 182

Coal and air react giving a reversible reaction

Answer 183

Copper calorimeter

Answer 184

Glass calorimeter

Answer 185

Bomb calorimeter

Answer 186

Entropy change

Answer 187

Enthalpy change

Answer 188

Free energy change

Answer 189

Internal energy change

Answer 190

Have more energy than the products

Answer 191

Are at a higher temperature than the products

Answer 192

Have less energy than the products

Answer 193

Have the same energy as the products

Answer 194

It is not irreversible

Answer 195

It is reversible

Answer 196

It is irreversible

Answer 197

None of these

Answer 198

Heat and work

Answer 199

Heat and volume

Answer 200

Pressure and temperature

Answer 201

Pressure and volume

Answer 202

Exothermic

Answer 203

Both a and b

Answer 204

Endothermic

Answer 205

Charles’s law

Answer 206

Henry’s law

Answer 207

Graham’s law

Answer 208

Hess’s law

Answer 209

Hat of formation

Answer 210

Heat of combustion

Answer 211

Heat of neutralization

Answer 212

Enthalpy of reaction

Answer 213

2 x 57.3 kJ

Answer 214

Cannot be predicted

Answer 215

Photochemical

Answer 216

Exothermic

Answer 217

Endothermic

Answer 218

Breaking of chemical bonds

Answer 219

Making of chemical bond

Answer 220

Burning of carbon

Answer 221

All of these

Answer 222

Ice will sublime

Answer 223

Water will freeze

Answer 224

Ice will melt

Answer 225

Water will vaporize

Answer 226

Graham’s law

Answer 227

Henry’s law

Answer 228

Hess’s law

Answer 229

Boyle’s law

Answer 230

Rate of reaction

Answer 231

Equilibrium constant

Answer 232

Influence of pressure on volume of a gas

Answer 233

Changes in heat or reaction

Answer 234

Physical process

Answer 235

Biochemical process

Answer 236

Endothermic process

Answer 237

Chemical process

Answer 238

Heat of sublimation

Answer 239

Heat of reaction

Answer 240

Heat of neutralization

Answer 241

Heat of combustion

Answer 242

Spontaneous

Answer 243

Non-spontaneous

Answer 244

Endothermic

Answer 245

Exothermic

Answer 246

Heat is evolved

Answer 247

Heat is converted into mechanical work

Answer 248

Heat is absorbed

Answer 249

Heat is converted into electricity

Answer 250

71030 calories

Answer 251

70960 calories

Answer 252

+70 calories

Answer 253

-70 calories

Answer 254

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

Answer 255

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer 256

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

Answer 257

Neutralization is always exothermic

Answer 258

Thermodynamics

Answer 259

Thermochemistry

Answer 260

Chemical kinetics

Answer 261

HCl is more stable than HF

Answer 262

HF and HCl are endothermic compounds

Answer 263

HF is more stable than HCl

Answer 264

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

Answer 265

Spontaneous

Answer 266

Non-spontaneous

Answer 267

Endothermic

Answer 268

Exothermic

Answer 269

None of these

Answer 270

9.75 JK¯¹

Answer 271

2.33 JK¯¹

Answer 272

11.272 JK¯¹

Answer 273

Insufficient data

Answer 274

Non-spontaneous

Answer 275

Endothermic

Answer 276

Exothermic

Answer 277

Spontaneous

Answer 278

P.E, + mechanical energy

Answer 279

K.E, + heat energy

Answer 280

P.E, + K.E.

Answer 281

P.E. + heat energy

Answer 282

∆E = q + w

Answer 283

∆H = ∆E + P∆V

Answer 284

Q = m x X x ∆ T

Answer 285

P∆V + nRT

Answer 286

Rotational motion

Answer 287

Translational motion

Answer 288

The sum of all motions which are possible

Answer 289

Vibrational motion

Answer 290

Decrease of entropy

Answer 291

Increase of free energy

Answer 292

Decrease of free energy

Answer 293

Increase of enthalpy

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