Thermo-Chemistry Online Mcqs Test

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Question 1

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

Question 2

2. Reaction in which heat is evolved

Answer

Non-spontaneous

Answer

Exothermic

Answer

Spontaneous

Answer

Endothermic

Question 3

3. 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 4

4. 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 5

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

Answer

Surrounding

Question 6

6. 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

Unpredictable

Answer

Absorption of 218 kcal of energy

Answer

Release of 109 kcal of energy

Answer

Release of 218 kcal of energy

Question 7

7. 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 8

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

Question 9

9. 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 10

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

Answer

Isothermal

Question 11

11. Free energy change for a reversible process is:

Answer

Unpredictable

Answer

Equal to zero

Question 12

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

Question 13

13. Evaporation of water is

Answer

An exothermic change

Answer

A process where no heat changes occur

Answer

A process accompanied by chemical reaction

Answer

An endothermic change

Question 14

14. 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 15

15. 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 16

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

Answer

Henry’s law

Answer

Graham’s law

Answer

Hess’s law

Answer

Boyle’s law

Question 17

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

Answer

Respiration

Answer

Combustion

Answer

Thermal decomposition

Answer

Neutralization

Question 18

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

Answer

Endothermic

Answer

Exothermic

Answer

Both a and b

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. An adiabatic expansion of an ideal gas always has

Answer

Decrease in temperature

Question 21

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

Answer

Heat of neutralization

Answer

Heat of reaction

Answer

Heat of sublimation

Answer

Heat of combustion

Question 22

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

Answer

Not change

Answer

None of these

Question 23

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

Answer

Electron – volt

Question 24

24. Two fundamental ways to transfer energy are

Answer

Heat and volume

Answer

Heat and work

Answer

Pressure and volume

Answer

Pressure and temperature

Question 25

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

Answer

Translational motion

Answer

Rotational motion

Answer

Vibrational motion

Answer

The sum of all motions which are possible

Question 26

26. 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 27

27. 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 28

28. Which one is not a state function?

Answer

Gibbs free energy

Answer

Internal energy

Question 29

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

Answer

Joule deg¯¹ atom¯¹

Answer

Joule deg¯¹ mol¯¹

Answer

Joule cm¯¹ deg¯¹

Answer

Joule deg¯¹ Kg¯¹

Question 30

30. For a reaction to occur spontaneously

Answer

∆ H must be unity

Answer

∆ H must be negative

Answer

∆ H must be zero

Answer

∆ H must be positive

Question 31

31. Most of the reactions which give stable products are

Answer

Exothermic

Answer

None of these

Answer

Isothermal

Answer

Endothermic

Question 32

32. 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

Reversible

Answer

Irreversible

Answer

Non-spontaneous

Answer

Spontaneous

Question 33

33. Two fundamental ways to transfer energy are

Answer

Heat and volume

Answer

Pressure and volume

Answer

Pressure and temperature

Answer

Heat and work

Question 34

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

Answer

HF is more stable than HCl

Answer

HF and HCl are endothermic compounds

Answer

HCl is more stable than HF

Answer

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

Question 35

35. Hess’s law deals with

Answer

Influence of pressure on volume of a gas

Answer

Changes in heat or reaction

Answer

Rate of reaction

Answer

Equilibrium constant

Question 36

36. 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 37

37. Unit of heat is SI system is

Question 38

38. Which statement describes characteristics of an endothermic reaction?

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

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 39

39. 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 40

40. Total energy of a system is

Answer

P.E, + K.E.

Answer

K.E, + heat energy

Answer

P.E, + mechanical energy

Answer

P.E. + heat energy

Question 41

41. 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 42

42. 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 43

43. Mechanical work is especially important in systems that contain

Answer

Solid-solid

Answer

Solid-liquid

Answer

Liquid-liquid

Question 44

44. The enthalpy of formation of carbon monoxide will be

Answer

2x – y/2

Answer

Y – 2x/2

Question 45

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

Question 46

46. 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 47

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

Answer

Internal energy change

Answer

Entropy change

Answer

Free energy change

Answer

Enthalpy change

Question 48

48. 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 49

49. An endothermic reaction is one in which

Answer

Heat is converted into mechanical work

Answer

Heat is evolved

Answer

Heat is absorbed

Answer

Heat is converted into electricity

Question 50

50. 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 51

51. When a bond breaks

Answer

Heat is evolved

Answer

Heat is absorbed

Answer

Temperature increases

Answer

No change in heat contents takes place

Question 52

52. Which type of reactions cannot occur spontaneously?

Answer

Endothermic

Answer

Exothermic

Answer

Both a and b

Question 53

53. 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 small + ve value for enthalpy change

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

Question 54

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

Answer

Electron – volt

Question 55

55. 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

112 kJ mol¯¹

Answer

668 kJ mol¯¹

Answer

-668 kJ mol¯¹

Question 56

56. Total energy depends upon the state of system

Answer

Entropy of reaction

Answer

Free energy of reaction

Question 57

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

Answer

Temperature

Question 58

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

Answer

Spontaneous

Answer

Endothermic

Answer

Non-spontaneous

Answer

Exothermic

Question 59

59. Endothermic changes are indicated through

Answer

Burning of carbon

Answer

Breaking of chemical bonds

Answer

Making of chemical bond

Answer

All of these

Question 60

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

Answer

Glass Calorimeter

Answer

Thermometer

Answer

Bomb Calorimeter

Question 61

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

Answer

Have the same energy as the products

Answer

Have less energy than the products

Answer

Are at a higher temperature than the products

Answer

Have more energy than the products

Question 62

62. Enthalpy of a reaction can be measured by

Answer

Glass calorimeter

Answer

Thermometer

Question 63

63. 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

Burning of coal in air releases large amount of energy

Answer

Burning of coal is and endothermic process

Answer

None of these

Question 64

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

Answer

Decomposition

Answer

Both a and b

Answer

Exothermic

Answer

Endothermic

Answer 173

Graphite is more stable than diamond

Answer 174

Both are equally stable

Answer 175

Graphite has more energy than diamond

Answer 176

Stability cannot to predicated

Answer 177

Work done is independent of its path

Answer 178

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

Answer 179

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

Answer 180

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

Answer 181

2 kg H₂O

Answer 182

4 kg H₂O

Answer 183

3 kg H₂O

Answer 184

1 kg H₂O

Answer 185

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

Answer 186

The lattice energy of the crystalline substances can be calculated easily

Answer 187

Born Haber cycle is different from Hess’s law

Answer 188

The energy change in a cyclic process is not zero

Answer 189

Decrease of free energy

Answer 190

Increase of free energy

Answer 191

Increase of enthalpy

Answer 192

Decrease of entropy

Answer 193

∆E = q + w

Answer 194

P∆V + nRT

Answer 195

∆H = ∆E + P∆V

Answer 196

Q = m x X x ∆ T

Answer 197

Enthalpy of reaction

Answer 198

Heat of neutralization

Answer 199

Heat of combustion

Answer 200

Hat of formation

Answer 201

Copper calorimeter

Answer 202

Bomb calorimeter

Answer 203

Glass calorimeter

Answer 204

Ice will melt

Answer 205

Ice will sublime

Answer 206

Water will freeze

Answer 207

Water will vaporize

Answer 208

P.E + heat energy

Answer 209

P.E + mechanical energy

Answer 210

K.E + heat energy

Answer 211

Thermodynamics

Answer 212

Stoichiometry

Answer 213

Thermochemistry

Answer 214

State function

Answer 215

Physical property

Answer 216

Chemical property

Answer 217

Energy of the system

Answer 218

State function

Answer 219

Any substance

Answer 220

Surrounding

Answer 221

It is reversible

Answer 222

It is irreversible

Answer 223

None of these

Answer 224

It is not irreversible

Answer 225

Gibbs free energy

Answer 226

Internal energy

Answer 227

Exothermic

Answer 228

Photochemical

Answer 229

Endothermic

Answer 230

Both a and b

Answer 231

Reactants is more than that of products

Answer 232

Products is more than that of reactants

Answer 233

Reactants and products are equal

Answer 234

Second law

Answer 235

Zeroth law

Answer 236

Biochemical process

Answer 237

Endothermic process

Answer 238

Chemical process

Answer 239

Physical process

Answer 240

Water equivalent

Answer 241

None of these

Answer 242

Specific heat

Answer 243

Thermal capacity

Answer 244

State function

Answer 245

Surrounding

Answer 246

None of these

Answer 247

Irreversible process

Answer 248

Spontaneous process

Answer 249

Non spontaneous

Answer 250

Non-spontaneous

Answer 251

Spontaneous

Answer 252

Exothermic

Answer 253

Endothermic

Answer 254

None of these

Answer 255

Henry’s law

Answer 256

Graham’s law

Answer 257

Hess’s law

Answer 258

Charles’s law

Answer 259

Photochemistry

Answer 260

Thermochemistry

Answer 261

Thermodynamics

Answer 262

71030 calories

Answer 263

+70 calories

Answer 264

70960 calories

Answer 265

-70 calories

Answer 266

Chemical kinetics

Answer 267

Thermochemistry

Answer 268

Thermodynamics

Answer 269

Temperature should be high

Answer 270

Temperature has no effect

Answer 271

Temperature should be zero

Answer 272

Temperature should be low

Answer 273

Electron vol

Answer 274

11.272 JK¯¹

Answer 275

9.75 JK¯¹

Answer 276

Insufficient data

Answer 277

2.33 JK¯¹

Answer 278

∆H = ∆E – PV

Answer 279

∆H = ∆E + d

Answer 280

∆H = ∆E – d

Answer 281

∆H = ∆E + Pv

Answer 282

Dissolution on NH₄Cl in excess of water is an endothermic process

Answer 283

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

Answer 284

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

Answer 285

Neutralization is always exothermic

Answer 286

None of these

Answer 287

Bond length

Answer 288

Bond strength

Answer 289

Bond energy

Answer 290

A lowering of free energy

Answer 291

A lowering of energy

Answer 292

An increase in internal energy

Answer 293

No energy change

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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