Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. A device which converts electrical energy into chemical energy is called

Answer

A chemical cell

Answer

A galvanic cell

Answer

An electrolytic cell

Answer

A voltaic cell

Question 2

2. Oxidation in a chemical reaction involves

Answer

Decrease in oxidation number

Answer

Increase in oxidation number of all the elements on reactant side

Answer

Both are possible

Answer

Increase in oxidation number

Question 3

3. A smuggler could not carry gold by chemically depositing iron on the gold surface since

Answer

Iron rusts

Answer

Gold is denser

Answer

Gold has higher reduction potential then iron

Answer

Gold has lower reduction potential then iron

Question 4

4. Pure water does not conduct electricity because it

Answer

Has low boiling point

Answer

Is neutral

Answer

Is readily decomposed

Answer

Is almost unionized

Question 5

5. Li occupies higher position in the electrochemical series of metals as compared to Cu since

Answer

Li is smaller in size as compared to Cu

Answer

The standard reduction potential of Cu²+/Cu is lower than that of Li⁺/Li

Answer

The standard reduction potential of Li⁺/Li is lower than that of Cu²+/Cu

Answer

The standard oxidation potential of Li/Li⁺ is lower than that of CuCu²⁺

Question 6

6. A dry alkaline cell has porous Zn anode & MnO₂ as cathode the electrolyte used is

Question 7

7. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 8

8. Specific conductivity of a solution

Answer

Depends on mass of electrolyte

Answer

Decreases with dilution

Answer

Increases with dilution

Answer

Remains unchanged with dilution

Question 9

9. Azeotropic mixture of HCl and water has

Question 10

10. Oxidation number of carbon in NaHCO₃ is

Question 11

11. Time required to deposit one millimole of aluminum metal by the passage of 9.65 amperes through molten electrolyte containing aluminum ion is

Question 12

12. The EMF of the cell rection Fe²⁺ + zn = Zn²⁺ + feis

Answer

– 1.17 V

Answer

– 0.35 V

Question 13

13. Under the process of rusting of iron, 4Fe + 3O₂ → 2Fe₂O₃, iron is

Answer

Precipitated

Answer

Hydrolyzed

Question 14

14. The conductivity of strong electrolyte

Answer

Does not change on dilution

Answer

Increases on dilution slightly

Answer

Decreases on dilution

Answer

Depends on density of electrolyte itself.

Question 15

15. If 18 g of glucose (C₆H₁₂C₆) is present in 1000 g of an aqueous solution of glucose it is said to be

Question 16

16. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

Question 17

17. Which of the following element act as inert electrode?

Question 18

18. What will be the density of H₂SO₄ when lead accumulator is recharged?

Answer

1.25 cm¯³

Answer

1.81 cm¯³

Answer

2.15 cm¯³

Answer

1.15 cm¯³

Question 19

19. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 20

20. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

Answer

Electric change

Answer

Standard electrode potential

Answer

Ionization potential

Answer

Electroplating

Question 21

21. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 22

22. A solution of sodium sulphate was electrolyzed using some inert electrodes. The products at the electrodes are

Answer

O₂, SO₂

Answer

None of these

Question 23

23. The best reducing agent is

Question 24

24. The weight of pure NaOH required to prepare 250 cm³ of 0.1 N solution is

Question 25

25. The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be

Answer

2.0 x 10¹¹

Answer

1.0 x 10¹⁰

Answer

1.0 x 10²

Answer

4.0 x 10¹²

Question 26

26. Wen quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

Answer

Electrochemical equivalent

Answer

One gm. Equivalent weight

Answer

One gm. atomic weight

Answer

None of these

Question 27

27. When molten sodium undergoes electrolysis, the ion reduces is

Answer

Both Na⁺ and CI¯

Answer

None of these

Question 28

28. Decrease in oxidation number is called

Answer

All of these

Question 29

29. If 5.85 g of NaCl are dissolved in 90g of water, the mole fraction of NaCl is

Question 30

30. How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

Question 31

31. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 32

32. What is the molality of a solution prepared by dissolving 5 g of toluene in 250 g of Benzene.

Question 33

33. In the electrolysis of molten sodium chloride, what is the yellow green gas formed?

Question 34

34. The art of electroplating was given by

Answer

Thomas Gradam

Question 35

35. In alkaline battery anode is made up of

Question 36

36. Reaction takes place at anode is

Answer

Hydrolysis

Answer

Ionization

Question 37

37. Cathode provides electrons to

Answer

Neutral atom

Answer

Does not provide any electron

Question 38

38. If liquids A and B form an ideal solution

Answer

The entropy of mixing is zero

Answer

The enthalpy of mixing is zero

Answer

The free energy as well as the entropy of mixing are each zero

Answer

The free energy of mixing is zero

Question 39

39. Which one of the following is a colligative property?

Answer

Refractive index

Answer

Osmotic pressure

Answer

Surface tension

Question 40

40. Potential of Zn is called

Answer

It has not potential

Question 41

41. Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as

Answer

Distribution law

Answer

Ostwald’s dilution law

Answer

Raoult’s law

Answer

Henry’s law

Question 42

42. The number of coulombs required for the deposition of 107.870 g of silver is

Question 43

43. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

Question 44

44. A solution contains A, B and C components. The mole fraction A and C are 0.25 and 0.35 respectively. The mole fraction B will be

Question 45

45. Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Kf of water 1.86 K mol¯¹ kg and specific gravity of ethylene glycol is 1.11)

Question 46

46. In alkaline battery the anode is made up of

Question 47

47. Electrode potential of Zn is

Answer

Depends on the nature of the coupled electrode

Answer

Oxidation-reduction

Question 48

48. When common salt is dissolved in water

Answer

B.P of water remain constant

Answer

Any possibility

Answer

B.P of water decrease

Answer

B.P of water increase

Question 49

49. In a chemical reaction, oxidation process involves

Answer

Decrease in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Answer

Oxidation number neither increases nor decreases

Answer

Increase in oxidation number of element

Question 50

50. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 51

51. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

Question 52

52. Which of the following solution of H₂SO₄ is more concentrated?

Question 53

53. If the ionic product of a solution is less than the solubility product, the solution is

Answer

Unsaturated

Answer

Supersaturated

Question 54

54. Anode electrode element always have _________ position in electrochemical series

Answer

Not particular

Question 55

55. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 56

56. Mole fraction of pure water is

Answer

Exactly equal to one

Answer

None of these

Answer

Slightly less than one

Answer

Slightly greater than one

Question 57

57. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 58

58. The solubility of a gas in water depends upon

Answer

All of these

Answer

Pressure of the gas

Answer

Temperature

Answer

Nature of the gas

Question 59

59. Camphor is often used in molecular mass determination because

Answer

It has a very high cryoscopic constant

Answer

It is readily available

Answer

It is solvent for organic substances

Answer

It is volatile

Question 60

60. A cell in which chemical energy is converted into electrical energy is called

Answer

Galvanic cell

Answer

Electrolytic cell

Question 61

61. The cryoscopic constant of water is 1.86. The elevation of B.P for a 0.1m solution of a solute in water is

Answer

Sufficient date not given

Question 62

62. An electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of the silver voltammeter is 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is

Question 63

63. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

Answer

22400 cm³

Question 64

64. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

Answer

Na is dissolved in Hg while it does not dissolve in Pt

Answer

Conc. Of H⁺ ions is when Pt electrode is taken

Answer

More voltage is required to reduce H⁺ at Hg than at Pt

Answer

Hg is more inert than Pt

Answer 107

Standard oxidation potential

Answer 108

Ionization potential

Answer 109

Cell voltage

Answer 110

Standard reduction potential

Answer 111

pH is changed

Answer 112

Gains electrons

Answer 113

Acts as a catalyst

Answer 114

Loses electrons

Answer 115

Metals have high resistance

Answer 116

They are mobile electrons in the metallic structure

Answer 117

Metals are decomposed by current

Answer 118

In metals the ions are free to more

Answer 119

Vacuum distillation

Answer 120

Fractional distillation

Answer 121

None of these

Answer 122

Distillation

Answer 123

Inversion point

Answer 124

Boiling point

Answer 125

Sublimation point

Answer 126

Melting point

Answer 127

Equal to that of water

Answer 128

Equal to that of ethanol

Answer 129

Less than that of water

Answer 130

More than that of H₂O

Answer 131

Magnetic energy

Answer 132

Sound energy

Answer 133

Heat energy

Answer 134

Electrical energy

Answer 135

Raoult’s law

Answer 136

Arrhenius law

Answer 137

Henry’s law

Answer 138

Ostwald’s law

Answer 139

None of these

Answer 140

Ohm¯¹ cm

Answer 141

Ohm cm¯¹

Answer 142

Ohm¯¹ cm¯¹

Answer 143

Ohm cm¯²

Answer 144

Non-spontaneous redox reactions

Answer 145

Spontaneous acid–base reactions

Answer 146

None of these

Answer 147

Spontaneous redox reactions

Answer 148

Mole fraction of the solution

Answer 149

Molarity of the solvent

Answer 150

Molarity of the solution

Answer 151

Molality of the solution

Answer 152

From anode to cathode in an outer circuit

Answer 153

From anode to cathode inside the cell

Answer 154

From cathode to anode inside the cell

Answer 155

From cathode to anode in outer circuit

Answer 156

Sulphuric acid

Answer 157

Phosphorus acid

Answer 158

Boric acid

Answer 159

Nitric acid

Answer 160

0.1 M NaCl

Answer 161

0.1 M BaCl₂

Answer 162

0.1 M Glucose

Answer 163

0.1 M Sucrose

Answer 164

1.15 g/Cm³

Answer 165

1.2 g/Cm³

Answer 166

120 g Cm³

Answer 167

1.25g/Cm³

Answer 168

Microgram percent

Answer 169

Gram per million

Answer 170

Milligram percent

Answer 171

Parts per million

Answer 172

Vapour pressure of pure water decreases by the addition of nitric acid

Answer 173

Boiling point of pure water decreases by the addition of ethanol

Answer 174

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 175

Boiling point of pure benzene increases by the addition of toluene

Answer 176

Diffusion rate of the solute

Answer 177

Flow of solvent from a concentrated to a dilute solution

Answer 178

Elevation in boiling point

Answer 179

Ionic concentration

Answer 180

Naphthalene

Answer 181

Hg₂Cl₂

Answer 182

Spontaneous reaction

Answer 183

Non-spontaneous reaction

Answer 184

Neutralization

Answer 185

Reduction potential

Answer 186

Oxidation potential

Answer 187

e.m.f of cell

Answer 188

Redox potential

Answer 189

Dilute solution which behave as nearly ideal solution

Answer 190

Concentration solutions behave as nearly non – ideal solutions

Answer 191

Neither a nor b

Answer 192

Both a and b

Answer 193

760 mm of Hg

Answer 194

Slightly more than 1 atom

Answer 195

Salt bridge maintains the electrical neutrality of the solution

Answer 196

Cathode is regarded as negative electrode

Answer 197

Electrons are released at anode

Answer 198

Chemical energy is converted into electrical energy

Answer 199

1.06 x 10²

Answer 200

1.06 x 10⁴

Answer 201

1.06 x 10³

Answer 202

H₄P₃O₇

Answer 203

Anode to cathode through the external circuit

Answer 204

Anode to cathode through the solution

Answer 205

Cathode to anode through the solution

Answer 206

Cathode to anode through the external circuit

Answer 207

Na, Pt and graphite

Answer 208

Na and S only

Answer 209

Pt and graphite only

Answer 210

Na₂SO₄

Answer 211

CH₃ CooNH₄

Answer 212

Dilution increases

Answer 213

Dilution decreases

Answer 214

Pressure increases

Answer 215

By replacing external circuit with external source of electricity

Answer 216

By removal of solution

Answer 217

By addition of fresh solution

Answer 218

By heating it

Answer 219

Electroplating

Answer 220

Electrorefining

Answer 221

None of these

Answer 222

Both A and B

Answer 223

None of these

Answer 224

Putting it in saline water

Answer 225

Both of these

Answer 226

Making iron cathode

Answer 227

S² m² mol

Answer 228

S² m² mol¯²

Answer 229

S m² mol¯¹

Answer 230

S m mol¯¹

Answer 231

H+ and OH-

Answer 232

Does not change

Answer 233

Decreases slowly

Answer 234

Decrease rapidly

Answer 235

Drops to zero

Answer 236

Hg₂Cl₂

Answer 237

Electrons flow from cathode to anode through the external battery

Answer 238

Migration of ions along with oxidation reaction at anode and reduction reaction at cathode

Answer 239

Electrons flow cathode to anode within the electrolytic solution

Answer 240

None of these

Answer 241

Dilute solution of glucose

Answer 242

Molten NaCl

Answer 243

Chloroform

Answer 244

Pure distilled water

Answer 245

750 mm of Hg

Answer 246

800 mm of Hg

Answer 247

760 mm of Hg

Answer 248

780 mm of Hg

Answer 249

A reaction in a solution

Answer 250

Ion combination reaction

Answer 251

Electron transfer

Answer 252

Proton transfer

Answer 253

Slightly more than the total volume of the components

Answer 254

Equal to the total volume of the components

Answer 255

Slightly less than the total volume of the components

Answer 256

None of these

Answer 257

1 – 2 α

Answer 258

Greater positive value of standard reduction potential

Answer 259

Lesser positive value of standard reduction potential

Answer 260

None of these

Answer 261

Greater negative value of standard reduction potential

Answer 262

Very low ionization potential values

Answer 263

Reduction potentials are negative

Answer 264

Very high negative values reduction potential

Answer 265

Very high positive value of reduction potential

Answer 266

Photo electrolysis

Answer 267

Electrolysis

Answer 268

Cathodic protection

Answer 269

Galvanization

Answer 270

Neither oxidation and reduction

Answer 271

Both oxidation and reduction

Answer 272

Solvent particles

Answer 273

Generate heat

Answer 274

Remove adsorbed oxygen from electrode surfaces

Answer 275

Produce high purity water

Answer 276

Create potential difference between two electrodes

Answer 277

Conduction

Answer 278

Electrolysis

Answer 279

Electroplating

Answer 280

Electrical energy is converted into heat

Answer 281

Chemical energy is converted into heat

Answer 282

Chemical energy is converted into electricity

Answer 283

Electrical energy is converted into chemical energy

Answer 284

12157.48 sec

Answer 285

96500 g of CU

Answer 286

100 g of Cu

Answer 287

31.75 g of Cu

Answer 288

63.5 g of Cu

Answer 289

[Pt(NH₃)₄Cl]Cl₃

Answer 290

[Pt(NH₃)₄Cl₃]Cl

Answer 291

[Pt(NH₃)₄Cl₄]

Answer 292

[Pt(NH₃)₄Cl₂]Cl₂

Answer 293

∆ G = -ve

Answer 294

∆ G = +ve, ∆ E = 0

Answer 295

∆ G = 0, ∆E = 0

Answer 296

∆ G = -ve, ∆ E = 0

Answer 297

Loses electrons

Answer 298

Gains electrons

Answer 299

Is oxidized

Answer 300

Is hydrolysed

Answer 301

Chemical energy

Answer 302

None of these

Answer 303

Electrical energy

Answer 304

Heat energy

Answer 305

Drops to zero

Answer 306

Increases rapidly

Answer 307

Increases gradually

Answer 308

Does not change

Answer 309

0.1 N NaCl

Answer 310

None of these

Answer 311

Altered reaction in presence of H₂O

Answer 312

Union between two light metals and a heavy metal

Answer 313

Electrochemical phenomenon

Answer 314

Interaction

Answer 315

Rechargeable

Answer 316

Daniel cell

Answer 317

Electrolytic cell

Answer 318

Non rechargeable

Answer 319

The degree of decomposition of solution

Answer 320

The extent of dissociation of solute

Answer 321

The extent of dissolution of solute

Answer 322

Degree of solubilization of solute

Answer 323

Possesses ions even in solid state

Answer 324

Gives ions only when dissolved in water

Answer 325

Forms complex ions in solution

Answer 326

Gives ions only when electricity is passed

Answer 327

Manufacture of bleach

Answer 328

Rust removal

Answer 329

Electroplating

Answer 330

Making leather

Answer 331

None of these

Answer 332

302 S cm² mol¯¹

Answer 333

176 S cm² mol¯¹

Answer 334

128 S cm² mol¯¹

Answer 335

278 S cm² mol¯¹

Answer 336

None of these

Answer 337

Na⁺ + e– → Na

Answer 338

Na → Na⁺ + e–

Answer 339

2Br– → Br₂ + 2e –

Answer 340

Br₂ + 2e – → 2Br –

Answer 341

Sum of reduction and oxidation potentials

Answer 342

Electric circuit

Answer 343

Salt Bridge

Answer 344

No connection exists

Answer 345

1.12 cm¯¹

Answer 346

0.66 cm¯¹

Answer 347

0.918 cm¯¹

Answer 348

0.142 cm¯¹

Answer 349

Strong acid and its salt of weak base

Answer 350

A strong acid and its salt of a strong base

Answer 351

Weak acid and its salt of strong base

Answer 352

Weak acid and its salt of weak base

Answer 353

20g NaCl/100ml

Answer 354

10.0g NaCl/100ml

Answer 355

5.58g NaCl/100m

Answer 356

58.5g NaCl/100ml

Answer 357

All electrochemical reactions involve the transfer of electrons

Answer 358

Reduction occurs at cathode

Answer 359

All voltaic (galvanic) cells involve the use of electricity to initiate nonspontaneous chemical reactions

Answer 360

Oxidation and reduction half-reactions occur at electrodes in electrochemical cells.

Answer 361

Galvanic cell

Answer 362

Electrolytic cell

Answer 363

Daniel cell

Answer 364

Both A and B

Answer 365

None of these

Answer 366

At cathode

Answer 367

Free molecules

Answer 368

Free electrons

Answer 369

Atoms of Na and Cl.

Total Questions:	192
Time Allowed:	60 Minutes
Total Marks:	192
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