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

70960 calories

Answer

71030 calories

Answer

+70 calories

Question 2

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

Answer

3 kg H₂O

Answer

2 kg H₂O

Answer

4 kg H₂O

Answer

1 kg H₂O

Question 3

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

Answer

None of these

Answer

Thermal capacity

Answer

Water equivalent

Answer

Specific heat

Question 4

4. 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

-439.3 kJ mol¯¹

Answer

-221.1 kJ mol¯¹

Answer

-339.3 kJ mol¯¹

Answer

-523.3 kJ mol¯¹

Question 5

5. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 6

6. Reaction in which heat is evolved

Answer

Exothermic

Answer

Non-spontaneous

Answer

Endothermic

Answer

Spontaneous

Question 7

7. 1 mole of H₂SO₄ is mixed with 2 mole of NaOH. The heat evolved will be

Answer

Cannot be predicted

Answer

2 x 57.3 kJ

Question 8

8. Most of the thermodynamic parameters are

Answer

Surrounding

Answer

State function

Question 9

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

Answer

P∆V + nRT

Answer

∆H = ∆E + P∆V

Answer

Q = m x X x ∆ T

Answer

∆E = q + w

Question 10

10. Unit of heat is SI system is

Question 11

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

Answer

Thermodynamics

Answer

Thermochemistry

Answer

Photochemistry

Question 12

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

Answer

Heat of combustion

Answer

Heat of reaction

Answer

Heat of sublimation

Answer

Heat of neutralization

Question 13

13. 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 14

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

Answer

Temperature

Question 15

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

Answer

Decrease of free energy

Answer

Decrease of entropy

Answer

Increase of enthalpy

Answer

Increase of free energy

Question 16

16. If internal energy of the system is increased

Answer

Chemical reaction may take place

Answer

Change in state of the system is increased

Answer

Temperature of the system may rise

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

Spontaneous

Answer

Reversible

Answer

Non-spontaneous

Answer

Irreversible

Question 18

18. 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 19

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

Answer

Isothermal

Question 20

20. Evaporation of water is

Answer

A process accompanied by chemical reaction

Answer

A process where no heat changes occur

Answer

An endothermic change

Answer

An exothermic change

Question 21

21. 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 22

22. 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 23

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

Answer

Physical process

Answer

Chemical process

Answer

Endothermic process

Answer

Biochemical process

Question 24

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

Answer

Surrounding

Answer

State function

Answer

Any substance

Question 25

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

Answer

Bomb Calorimeter

Answer

Thermometer

Answer

Glass Calorimeter

Question 26

26. 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 27

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

Answer

Exothermic

Answer

Spontaneous

Answer

Non-spontaneous

Answer

Endothermic

Question 28

28. 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 29

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

Answer

None of these

Answer

Not change

Question 30

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

Answer

Chemical kinetics

Answer

Thermodynamics

Answer

Thermochemistry

Question 31

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

Answer

Henry’s law

Answer

Charles’s law

Answer

Hess’s law

Answer

Graham’s law

Question 32

32. Total energy of a system is

Answer

K.E, + heat energy

Answer

P.E, + mechanical energy

Answer

P.E. + heat energy

Answer

P.E, + K.E.

Question 33

33. 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

395 KJ/mole

Answer

190 KJ/mole

Answer

-27 KJ/mole

Answer

386 KJ/mole

Question 34

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

Answer

∆H = ∆E + d

Answer

∆H = ∆E + Pv

Answer

∆H = ∆E – d

Answer

∆H = ∆E – PV

Question 35

35. 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 36

36. Which of the following is not correct?

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

Answer

Dissolution on NH₄Cl in excess of water is an endothermic process

Question 37

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

Question 38

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

Answer

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

Answer

The lattice energy of the crystalline substances can be calculated easily

Answer

The energy change in a cyclic process is not zero

Answer

Born Haber cycle is different from Hess’s law

Question 39

39. In general, for exothermic reactions to be spontaneous

Answer

Temperature has no effect

Answer

Temperature should be zero

Answer

Temperature should be high

Answer

Temperature should be low

Question 40

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

Answer

Glass calorimeter

Answer

Bomb calorimeter

Answer

Copper calorimeter

Question 41

41. Enthalpy of a reaction can be measured by

Answer

Glass calorimeter

Answer

Thermometer

Question 42

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

Answer

Work done is independent of its path

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

Question 43

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

Answer

Endothermic

Answer

Exothermic

Answer

Photochemical

Question 44

44. 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 the same energy as the products

Answer

Have less energy than the products

Question 45

45. Unit of heat in S.I system is

Question 46

46. The law of Lavoisier and Laplace illustrates

Answer

The principle of conservation of energy

Answer

Equivalent of mechanical and chemical energy

Answer

Equivalence of mechanical and thermal energy

Answer

The principle of conservation of matter

Question 47

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

Answer

Graphite is more stable than diamond

Answer

Graphite has more energy than diamond

Answer

Both are equally stable

Answer

Stability cannot to predicated

Question 48

48. Mechanical work is especially important in systems that contain

Answer

Solid-liquid

Answer

Liquid-liquid

Answer

Solid-solid

Question 49

49. 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 freeze

Answer

Water will vaporize

Answer

Ice will sublime

Question 50

50. Most of the reactions which give stable products are

Answer

None of these

Answer

Endothermic

Answer

Isothermal

Answer

Exothermic

Question 51

51. An endothermic reaction is one in which

Answer

Heat is absorbed

Answer

Heat is evolved

Answer

Heat is converted into mechanical work

Answer

Heat is converted into electricity

Question 52

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

Answer

Electron – volt

Question 53

53. Which type of reactions cannot occur spontaneously?

Answer

Exothermic

Answer

Both a and b

Answer

Endothermic

Question 54

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

Answer

Bond energy

Answer

None of these

Answer

Bond length

Answer

Bond strength

Question 55

55. 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 56

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

Answer

Endothermic

Answer

Both a and b

Answer

Exothermic

Question 57

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

Answer

Thermochemistry

Answer

Stoichiometry

Answer

Thermodynamics

Question 58

58. 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 59

59. Calorie is equivalent to

Question 60

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

Answer

None of these

Question 61

61. For a reaction to occur spontaneously

Answer

∆ H must be unity

Answer

∆ H must be positive

Answer

∆ H must be zero

Answer

∆ H must be negative

Question 62

62. 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

Release of 218 kcal of energy

Answer

Absorption of 218 kcal of energy

Answer

Unpredictable

Question 63

63. 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 64

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

Answer

Energy and volume

Answer

Pressure and volume

Answer

Temperature and volume

Answer

Temperature and pressure

Answer 181

Zeroth law

Answer 182

Second law

Answer 183

Non spontaneous

Answer 184

Spontaneous process

Answer 185

None of these

Answer 186

Irreversible process

Answer 187

HF is more stable than HCl

Answer 188

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

Answer 189

HF and HCl are endothermic compounds

Answer 190

HCl is more stable than HF

Answer 191

Surrounding

Answer 192

It has a large – ve value for the entropy change

Answer 193

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

Answer 194

It has small + ve value for enthalpy change

Answer 195

It has a large + ve value for enthalpy change

Answer 196

Electron vol

Answer 197

Reactants is more than that of products

Answer 198

Both a and b

Answer 199

Products is more than that of reactants

Answer 200

Reactants and products are equal

Answer 201

Temperature increases

Answer 202

Heat is absorbed

Answer 203

No change in heat contents takes place

Answer 204

Heat is evolved

Answer 205

Equilibrium constant

Answer 206

Influence of pressure on volume of a gas

Answer 207

Changes in heat or reaction

Answer 208

Rate of reaction

Answer 209

Hat of formation

Answer 210

Heat of neutralization

Answer 211

Enthalpy of reaction

Answer 212

Heat of combustion

Answer 213

None of these

Answer 214

It is reversible

Answer 215

It is irreversible

Answer 216

It is not irreversible

Answer 217

An increase in internal energy

Answer 218

No energy change

Answer 219

A lowering of free energy

Answer 220

A lowering of energy

Answer 221

Translational motion

Answer 222

Vibrational motion

Answer 223

Rotational motion

Answer 224

The sum of all motions which are possible

Answer 225

Internal energy

Answer 226

Gibbs free energy

Answer 227

Henry’s law

Answer 228

Graham’s law

Answer 229

Boyle’s law

Answer 230

Hess’s law

Answer 231

Joule deg¯¹ atom¯¹

Answer 232

Joule deg¯¹ mol¯¹

Answer 233

Joule deg¯¹ Kg¯¹

Answer 234

Joule cm¯¹ deg¯¹

Answer 235

Both a and b

Answer 236

Decomposition

Answer 237

Endothermic

Answer 238

Exothermic

Answer 239

2x – y/2

Answer 240

Y – 2x/2

Answer 241

P.E + mechanical energy

Answer 242

P.E + heat energy

Answer 243

K.E + heat energy

Answer 244

Enthalpy change

Answer 245

Internal energy change

Answer 246

Free energy change

Answer 247

Entropy change

Answer 248

+21.4 kcal mol¯¹

Answer 249

+64.8 kcal mol¯¹

Answer 250

-231.6 kcal mol¯¹

Answer 251

-94.0 kcal mol¯¹

Answer 252

Decrease in temperature

Answer 253

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

Answer 254

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

Answer 255

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

Answer 256

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

Answer 257

Internal energy

Answer 258

Gibbs free energy

Answer 259

State function

Answer 260

Energy of the system

Answer 261

Physical property

Answer 262

Chemical property

Answer 263

Pressure and temperature

Answer 264

Pressure and volume

Answer 265

Heat and work

Answer 266

Heat and volume

Answer 267

-112 kJ mol¯¹

Answer 268

-668 kJ mol¯¹

Answer 269

668 kJ mol¯¹

Answer 270

112 kJ mol¯¹

Answer 271

Coal and air react giving a reversible reaction

Answer 272

None of these

Answer 273

Burning of coal in air releases large amount of energy

Answer 274

Burning of coal is and endothermic process

Answer 275

Electron – volt

Answer 276

Heat and work

Answer 277

Pressure and volume

Answer 278

Pressure and temperature

Answer 279

Heat and volume

Answer 280

Breaking of chemical bonds

Answer 281

Making of chemical bond

Answer 282

All of these

Answer 283

Burning of carbon

Answer 284

Unpredictable

Answer 285

Equal to zero

Answer 286

Exothermic

Answer 287

Spontaneous

Answer 288

Non-spontaneous

Answer 289

Endothermic

Answer 290

Neutralization

Answer 291

Thermal decomposition

Answer 292

Combustion

Answer 293

Respiration

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