Thermo-Chemistry Online Mcqs Test

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Question 1

1. 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

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 energy change in a cyclic process is not zero

Question 2

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

Answer

Endothermic

Answer

Spontaneous

Answer

Non-spontaneous

Answer

Exothermic

Question 3

3. Pumping of water uphill is

Answer

None of these

Answer

Spontaneous process

Answer

Irreversible process

Answer

Non spontaneous

Question 4

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

Answer

-231.6 kcal mol¯¹

Answer

-94.0 kcal mol¯¹

Answer

+21.4 kcal mol¯¹

Answer

+64.8 kcal mol¯¹

Question 5

5. An endothermic reaction is one in which

Answer

Heat is converted into electricity

Answer

Heat is evolved

Answer

Heat is absorbed

Answer

Heat is converted into mechanical work

Question 6

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

Answer

Pressure and volume

Answer

Energy and volume

Answer

Temperature and pressure

Answer

Temperature and volume

Question 7

7. When a bond breaks

Answer

Heat is absorbed

Answer

Temperature increases

Answer

No change in heat contents takes place

Answer

Heat is evolved

Question 8

8. Unit of heat in S.I system is

Question 9

9. 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 10

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

Answer

Thermodynamics

Answer

Chemical kinetics

Answer

Thermochemistry

Question 11

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

Answer

Water equivalent

Answer

None of these

Answer

Thermal capacity

Answer

Specific heat

Question 12

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

Question 13

13. The enthalpy of formation of carbon monoxide will be

Answer

2x – y/2

Answer

Y – 2x/2

Question 14

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

Answer

Not change

Answer

None of these

Question 15

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

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

Answer

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

Question 16

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

Answer

Copper calorimeter

Answer

Bomb calorimeter

Answer

Glass calorimeter

Question 17

17. Total energy of a system is

Answer

P.E + heat energy

Answer

K.E + heat energy

Answer

P.E + mechanical energy

Question 18

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

Answer

Henry’s law

Answer

Hess’s law

Answer

Graham’s law

Answer

Charles’s law

Question 19

19. Mechanical work is especially important in systems that contain

Answer

Solid-solid

Answer

Liquid-liquid

Answer

Solid-liquid

Question 20

20. 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 21

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

Answer

It is not irreversible

Answer

It is reversible

Answer

It is irreversible

Answer

None of these

Question 22

22. 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 23

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

Answer

Boyle’s law

Answer

Graham’s law

Answer

Hess’s law

Answer

Henry’s law

Question 24

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

Answer

Respiration

Answer

Combustion

Answer

Neutralization

Answer

Thermal decomposition

Question 25

25. Which type of reactions cannot occur spontaneously?

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 26

26. The law of Lavoisier and Laplace illustrates

Answer

The principle of conservation of matter

Answer

Equivalence of mechanical and thermal energy

Answer

The principle of conservation of energy

Answer

Equivalent of mechanical and chemical energy

Question 27

27. Evaporation of water is

Answer

A process accompanied by chemical reaction

Answer

An exothermic change

Answer

An endothermic change

Answer

A process where no heat changes occur

Question 28

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

Answer

Second law

Answer

Zeroth law

Question 29

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

Answer

Temperature

Question 30

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

Answer

Isothermal

Question 31

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

Question 32

32. 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 33

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

Answer

None of these

Question 34

34. Which of the following is not correct?

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

Answer

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

Question 35

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

Answer

Electron – volt

Question 36

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

Question 37

37. 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 38

38. 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 39

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

Answer

Physical process

Answer

Chemical process

Answer

Endothermic process

Answer

Biochemical process

Question 40

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

Answer

Entropy change

Answer

Free energy change

Answer

Enthalpy change

Answer

Internal energy change

Question 41

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

Question 42

42. 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 43

43. 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 44

44. Most of the thermodynamic parameters are

Answer

State function

Answer

Surrounding

Question 45

45. 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

-439.3 kJ mol¯¹

Answer

-523.3 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Question 46

46. 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 47

47. 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 48

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

Answer

Joule deg¯¹ Kg¯¹

Answer

Joule deg¯¹ mol¯¹

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ atom¯¹

Question 49

49. 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 50

50. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 51

51. 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 combustion

Answer

Enthalpy of reaction

Answer

Hat of formation

Answer

Heat of neutralization

Question 52

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

Answer

Heat of combustion

Answer

Heat of sublimation

Answer

Heat of reaction

Answer

Heat of neutralization

Question 53

53. 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 54

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

Answer

Electron vol

Question 55

55. 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 56

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

Answer

Vibrational motion

Answer

Rotational motion

Answer

The sum of all motions which are possible

Answer

Translational motion

Question 57

57. 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

Non-spontaneous

Answer

Reversible

Answer

Irreversible

Question 58

58. The reaction is spontaneous if the cell potential is

Question 59

59. Calorie is equivalent to

Question 60

60. A spontaneous change means

Answer

A lowering of free energy

Answer

A lowering of energy

Answer

No energy change

Answer

An increase in internal energy

Question 61

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

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 62

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

Answer

Surrounding

Question 63

63. 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

9.75 JK¯¹

Answer

2.33 JK¯¹

Question 64

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

Answer

Have less energy than the products

Answer

Have the same energy as the products

Answer

Are at a higher temperature than the products

Answer

Have more energy than the products

Answer 160

Cannot be predicted

Answer 161

2 x 57.3 kJ

Answer 162

Temperature of the system may rise

Answer 163

Chemical reaction can take place

Answer 164

Change in state of system can occur

Answer 165

Reactants and products are equal

Answer 166

Reactants is more than that of products

Answer 167

Products is more than that of reactants

Answer 168

Both a and b

Answer 169

∆ H must be negative

Answer 170

∆ H must be unity

Answer 171

∆ H must be zero

Answer 172

∆ H must be positive

Answer 173

Increase of enthalpy

Answer 174

Increase of free energy

Answer 175

Decrease of entropy

Answer 176

Decrease of free energy

Answer 177

Spontaneous

Answer 178

Exothermic

Answer 179

Endothermic

Answer 180

Non-spontaneous

Answer 181

Pressure and volume

Answer 182

Heat and work

Answer 183

Pressure and temperature

Answer 184

Heat and volume

Answer 185

State function

Answer 186

Chemical property

Answer 187

Energy of the system

Answer 188

Physical property

Answer 189

P.E, + mechanical energy

Answer 190

P.E, + K.E.

Answer 191

K.E, + heat energy

Answer 192

P.E. + heat energy

Answer 193

Burning of coal in air releases large amount of energy

Answer 194

Burning of coal is and endothermic process

Answer 195

Coal and air react giving a reversible reaction

Answer 196

None of these

Answer 197

Pressure and volume

Answer 198

Heat and work

Answer 199

Heat and volume

Answer 200

Pressure and temperature

Answer 201

Thermochemistry

Answer 202

Photochemistry

Answer 203

Thermodynamics

Answer 204

1 kg H₂O

Answer 205

2 kg H₂O

Answer 206

3 kg H₂O

Answer 207

4 kg H₂O

Answer 208

None of these

Answer 209

Exothermic

Answer 210

Endothermic

Answer 211

Isothermal

Answer 212

Internal energy

Answer 213

Gibbs free energy

Answer 214

It has a large + ve value for enthalpy change

Answer 215

It has a large – ve value for the entropy change

Answer 216

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

Answer 217

It has small + ve value for enthalpy change

Answer 218

Both are equally stable

Answer 219

Stability cannot to predicated

Answer 220

Graphite is more stable than diamond

Answer 221

Graphite has more energy than diamond

Answer 222

Bomb Calorimeter

Answer 223

Thermometer

Answer 224

Glass Calorimeter

Answer 225

∆E = q + w

Answer 226

Q = m x X x ∆ T

Answer 227

∆H = ∆E + P∆V

Answer 228

P∆V + nRT

Answer 229

Internal energy

Answer 230

Gibbs free energy

Answer 231

∆H = ∆E + d

Answer 232

∆H = ∆E + Pv

Answer 233

∆H = ∆E – PV

Answer 234

∆H = ∆E – d

Answer 235

Surrounding

Answer 236

State function

Answer 237

Any substance

Answer 238

Non-spontaneous

Answer 239

Exothermic

Answer 240

Endothermic

Answer 241

Spontaneous

Answer 242

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

Answer 243

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

Answer 244

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

Answer 245

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

Answer 246

Influence of pressure on volume of a gas

Answer 247

Changes in heat or reaction

Answer 248

Equilibrium constant

Answer 249

Rate of reaction

Answer 250

Temperature has no effect

Answer 251

Temperature should be high

Answer 252

Temperature should be low

Answer 253

Temperature should be zero

Answer 254

Bond length

Answer 255

Bond energy

Answer 256

Bond strength

Answer 257

None of these

Answer 258

Electron – volt

Answer 259

Breaking of chemical bonds

Answer 260

Burning of carbon

Answer 261

Making of chemical bond

Answer 262

All of these

Answer 263

Thermochemistry

Answer 264

Thermodynamics

Answer 265

Stoichiometry

Answer 266

668 kJ mol¯¹

Answer 267

-112 kJ mol¯¹

Answer 268

-668 kJ mol¯¹

Answer 269

112 kJ mol¯¹

Answer 270

Release of 218 kcal of energy

Answer 271

Absorption of 218 kcal of energy

Answer 272

Release of 109 kcal of energy

Answer 273

Unpredictable

Answer 274

Glass calorimeter

Answer 275

Thermometer

Answer 276

Decrease in temperature

Answer 277

395 KJ/mole

Answer 278

-27 KJ/mole

Answer 279

190 KJ/mole

Answer 280

386 KJ/mole

Answer 281

Ice will sublime

Answer 282

Water will vaporize

Answer 283

Ice will melt

Answer 284

Water will freeze

Answer 285

HF and HCl are endothermic compounds

Answer 286

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

Answer 287

HCl is more stable than HF

Answer 288

HF is more stable than HCl

Answer 289

Unpredictable

Answer 290

Equal to zero

Answer 291

Photochemical

Answer 292

Exothermic

Answer 293

Endothermic

Total Questions:	108
Time Allowed:	60 Minutes
Total Marks:	108
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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