Thermo-Chemistry Online Mcqs Test

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Question 1

1. 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

2.33 JK¯¹

Answer

Insufficient data

Answer

9.75 JK¯¹

Answer

11.272 JK¯¹

Question 2

2. Enthalpy of formation of HF and HCl are – 161 kJ and -92 kJ respectively. Which of the following statements is incorrect?

Answer

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

Answer

HF and HCl are endothermic compounds

Answer

HCl is more stable than HF

Answer

HF is more stable than HCl

Question 3

3. 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

-439.3 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Answer

-221.1 kJ mol¯¹

Question 4

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

Answer

Vibrational motion

Answer

Translational motion

Answer

The sum of all motions which are possible

Answer

Rotational motion

Question 5

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

Answer

None of these

Question 6

6. 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

None of these

Answer

Burning of coal in air releases large amount of energy

Answer

Burning of coal is and endothermic process

Question 7

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

Answer

State function

Answer

Surrounding

Answer

Any substance

Question 8

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

Question 9

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

Answer

Photochemical

Answer

Exothermic

Answer

Endothermic

Question 10

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

Answer

Not change

Answer

None of these

Question 11

11. Which of the following is not correct?

Answer

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer

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

Answer

Neutralization is always exothermic

Answer

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

Question 12

12. Unit of heat is SI system is

Question 13

13. Reaction in which heat is evolved

Answer

Endothermic

Answer

Spontaneous

Answer

Non-spontaneous

Answer

Exothermic

Question 14

14. Unit of heat in S.I system is

Question 15

15. Hess’s law deals with

Answer

Changes in heat or reaction

Answer

Equilibrium constant

Answer

Influence of pressure on volume of a gas

Answer

Rate of reaction

Question 16

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

Answer

Both a and b

Answer

Endothermic

Answer

Exothermic

Answer

Decomposition

Question 17

17. 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

Irreversible

Answer

Non-spontaneous

Answer

Spontaneous

Answer

Reversible

Question 18

18. If internal energy of the system is increased

Answer

Temperature of the system may rise

Answer

Change in state of the system is increased

Answer

Chemical reaction may take place

Question 19

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

Answer

Endothermic

Answer

Spontaneous

Answer

Non-spontaneous

Answer

Exothermic

Question 20

20. Pumping of water uphill is

Answer

Spontaneous process

Answer

None of these

Answer

Irreversible process

Answer

Non spontaneous

Question 21

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

Answer

Bond length

Answer

None of these

Answer

Bond energy

Answer

Bond strength

Question 22

22. 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 23

23. 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

668 kJ mol¯¹

Answer

112 kJ mol¯¹

Question 24

24. Enthalpy of a reaction can be measured by

Answer

Glass calorimeter

Answer

Thermometer

Question 25

25. The law of Lavoisier and Laplace illustrates

Answer

The principle of conservation of energy

Answer

Equivalence of mechanical and thermal energy

Answer

The principle of conservation of matter

Answer

Equivalent of mechanical and chemical energy

Question 26

26. 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 27

27. 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 28

28. 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 29

29. 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 30

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

Answer

Electron vol

Question 31

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

Answer

Electron – volt

Question 32

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

Answer

+64.8 kcal mol¯¹

Answer

+21.4 kcal mol¯¹

Answer

-94.0 kcal mol¯¹

Answer

-231.6 kcal mol¯¹

Question 33

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

Answer

It is not irreversible

Answer

It is reversible

Answer

None of these

Answer

It is irreversible

Question 34

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

Answer

Have the same energy as the products

Answer

Are at a higher temperature than the products

Answer

Have less energy than the products

Answer

Have more energy than the products

Question 35

35. All of the following are state function except

Question 36

36. Calorie is equivalent to

Question 37

37. Evaporation of water is

Answer

A process where no heat changes occur

Answer

An endothermic change

Answer

An exothermic change

Answer

A process accompanied by chemical reaction

Question 38

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

Answer

Isothermal

Question 39

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

Answer

Physical property

Answer

Energy of the system

Answer

State function

Answer

Chemical property

Question 40

40. 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

Ice will melt

Answer

Water will vaporize

Answer

Ice will sublime

Answer

Water will freeze

Question 41

41. 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 42

42. A spontaneous change means

Answer

A lowering of free energy

Answer

A lowering of energy

Answer

An increase in internal energy

Answer

No energy change

Question 43

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

Answer

∆H = ∆E + Pv

Answer

∆H = ∆E – PV

Answer

∆H = ∆E + d

Answer

∆H = ∆E – d

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 same

Answer

Remains constant

Question 45

45. Which one is not a state function?

Answer

Gibbs free energy

Answer

Internal energy

Question 46

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

Answer

Neutralization

Answer

Thermal decomposition

Answer

Combustion

Answer

Respiration

Question 47

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

Answer

Temperature

Question 48

48. Endothermic changes are indicated through

Answer

Breaking of chemical bonds

Answer

All of these

Answer

Making of chemical bond

Answer

Burning of carbon

Question 49

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

Answer

Heat of sublimation

Answer

Heat of combustion

Answer

Heat of reaction

Answer

Heat of neutralization

Question 50

50. 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

190 KJ/mole

Answer

-27 KJ/mole

Question 51

51. When enthalpy of reactants is higher than product then reaction will be

Answer

Exothermic

Answer

Non-spontaneous

Answer

Spontaneous

Answer

Endothermic

Question 52

52. 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 53

53. The enthalpy of formation of carbon monoxide will be

Answer

Y – 2x/2

Answer

2x – y/2

Question 54

54. An adiabatic expansion of an ideal gas always has

Answer

Decrease in temperature

Question 55

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

Answer

It has a large – ve value for the entropy change

Answer

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

Answer

It has a large + ve value for enthalpy change

Answer

It has small + ve value for enthalpy change

Question 56

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

Answer

Thermodynamics

Answer

Stoichiometry

Answer

Thermochemistry

Question 57

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

Question 58

58. In endothermic reactions, the heat content of the

Answer

Reactants and products are equal

Answer

Reactants is more than that of products

Answer

Products is more than that of reactants

Answer

Both a and b

Question 59

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

Answer

Zeroth law

Answer

Second law

Question 60

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

Answer

Thermodynamics

Answer

Thermochemistry

Answer

Photochemistry

Question 61

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

Answer

Electron – volt

Question 62

62. In general, for exothermic reactions to be spontaneous

Answer

Temperature should be low

Answer

Temperature should be high

Answer

Temperature should be zero

Answer

Temperature has no effect

Question 63

63. Most of the reactions which give stable products are

Answer

Isothermal

Answer

Endothermic

Answer

None of these

Answer

Exothermic

Question 64

64. If internal energy of a system is increased

Answer

Temperature of the system may rise

Answer

Change in state of system can occur

Answer

Chemical reaction can take place

Answer 172

No change in heat contents takes place

Answer 173

Heat is evolved

Answer 174

Temperature increases

Answer 175

Heat is absorbed

Answer 176

Joule deg¯¹ mol¯¹

Answer 177

Joule cm¯¹ deg¯¹

Answer 178

Joule deg¯¹ atom¯¹

Answer 179

Joule deg¯¹ Kg¯¹

Answer 180

– 68 – 48 + 14

Answer 181

68 + 48 + 14

Answer 182

– 68 + 48 – 14

Answer 183

68 – 48 + 14

Answer 184

Biochemical process

Answer 185

Chemical process

Answer 186

Endothermic process

Answer 187

Physical process

Answer 188

3 kg H₂O

Answer 189

4 kg H₂O

Answer 190

2 kg H₂O

Answer 191

1 kg H₂O

Answer 192

Thermodynamics

Answer 193

Thermochemistry

Answer 194

Chemical kinetics

Answer 195

Release of 218 kcal of energy

Answer 196

Release of 109 kcal of energy

Answer 197

Unpredictable

Answer 198

Absorption of 218 kcal of energy

Answer 199

Internal energy

Answer 200

Gibbs free energy

Answer 201

Endothermic

Answer 202

Exothermic

Answer 203

Both a and b

Answer 204

Bomb Calorimeter

Answer 205

Thermometer

Answer 206

Glass Calorimeter

Answer 207

Internal energy change

Answer 208

Entropy change

Answer 209

Enthalpy change

Answer 210

Free energy change

Answer 211

Decrease of free energy

Answer 212

Increase of free energy

Answer 213

Increase of enthalpy

Answer 214

Decrease of entropy

Answer 215

The energy change in a cyclic process is not zero

Answer 216

The lattice energy of the crystalline substances can be calculated easily

Answer 217

Born Haber cycle is different from Hess’s law

Answer 218

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

Answer 219

Free energy of reaction

Answer 220

Entropy of reaction

Answer 221

Henry’s law

Answer 222

Hess’s law

Answer 223

Graham’s law

Answer 224

Boyle’s law

Answer 225

Both a and b

Answer 226

Exothermic

Answer 227

Endothermic

Answer 228

Equal to zero

Answer 229

Unpredictable

Answer 230

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

Answer 231

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

Answer 232

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

Answer 233

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

Answer 234

Heat and work

Answer 235

Heat and volume

Answer 236

Pressure and temperature

Answer 237

Pressure and volume

Answer 238

Surrounding

Answer 239

Charles’s law

Answer 240

Graham’s law

Answer 241

Hess’s law

Answer 242

Henry’s law

Answer 243

+70 calories

Answer 244

70960 calories

Answer 245

-70 calories

Answer 246

71030 calories

Answer 247

Q = m x X x ∆ T

Answer 248

∆H = ∆E + P∆V

Answer 249

P∆V + nRT

Answer 250

∆E = q + w

Answer 251

Graphite has more energy than diamond

Answer 252

Both are equally stable

Answer 253

Graphite is more stable than diamond

Answer 254

Stability cannot to predicated

Answer 255

Solid-solid

Answer 256

Liquid-liquid

Answer 257

Solid-liquid

Answer 258

Pressure and volume

Answer 259

Temperature and volume

Answer 260

Energy and volume

Answer 261

Temperature and pressure

Answer 262

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

Answer 263

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

Answer 264

Work done is independent of its path

Answer 265

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

Answer 266

Glass calorimeter

Answer 267

Bomb calorimeter

Answer 268

Copper calorimeter

Answer 269

Water equivalent

Answer 270

None of these

Answer 271

Thermal capacity

Answer 272

Specific heat

Answer 273

Surrounding

Answer 274

State function

Answer 275

Hat of formation

Answer 276

Enthalpy of reaction

Answer 277

Heat of combustion

Answer 278

Heat of neutralization

Answer 279

Heat and work

Answer 280

Pressure and volume

Answer 281

Pressure and temperature

Answer 282

Heat and volume

Answer 283

K.E + heat energy

Answer 284

P.E + heat energy

Answer 285

P.E + mechanical energy

Answer 286

K.E, + heat energy

Answer 287

P.E, + mechanical energy

Answer 288

P.E, + K.E.

Answer 289

P.E. + heat energy

Answer 290

∆ H must be positive

Answer 291

∆ H must be unity

Answer 292

∆ H must be zero

Answer 293

∆ H must be negative

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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