Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. The Vant Hoff factor (i) accounts for

Answer

Degree of solubilization of solute

Answer

The extent of dissolution of solute

Answer

The extent of dissociation of solute

Answer

The degree of decomposition of solution

Question 2

2. Units of molarity are

Answer

None of these

Question 3

3. The substance having highest conductivity at room temperature among the following is

Answer

0.1 N NaCl

Question 4

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

Question 5

5. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

Question 6

6. The solubility of a gas in water depends upon

Answer

Pressure of the gas

Answer

Nature of the gas

Answer

All of these

Answer

Temperature

Question 7

7. Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of NO¯₃ ions in the mixture will be

Question 8

8. 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 9

9. If a salt bridge is removed between the two half cells, the voltage

Answer

Does not change

Answer

Increases rapidly

Answer

Increases gradually

Answer

Drops to zero

Question 10

10. Which of the following is the strongest oxidizing agent?

Question 11

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

Answer

Ionization potential

Answer

Standard electrode potential

Answer

Electric change

Answer

Electroplating

Question 12

12. The volume of 0.1 M H₂SO₄ required to neutralize completely 40 ml of 0.2 M NaOH solution is

Question 13

13. 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 14

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

Question 15

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

Answer

2.15 cm¯³

Answer

1.15 cm¯³

Answer

1.81 cm¯³

Answer

1.25 cm¯³

Question 16

16. The standard EMF of Daniel cell is 1.10 volt. The maximum electrical work obtained from the Daniel cell is

Question 17

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

Question 18

18. What will be the weight of deposited silver on passing 965 coulombs of electricity in solution of AgNO₃?

Question 19

19. How much of NaOH is required to neutralize 1500 cm³ of 0.1 N HCl?

Question 20

20. Decrease in oxidation number is called

Answer

All of these

Question 21

21. Maximum freezing point falls in

Answer

Naphthalene

Question 22

22. The molality of 2% NaCl. W/W solution is approximately

Question 23

23. Which one of the following will be good conductor of electricity?

Answer

Molten NaCl

Answer

Pure distilled water

Answer

Dilute solution of glucose

Answer

Chloroform

Question 24

24. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 25

25. An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is

Question 26

26. A certain current liberate 0.5 g of hydrogen in 2 h. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

Question 27

27. The cathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrodes is

Answer

Both oxidation and reduction

Answer

Neither oxidation and reduction

Question 28

28. Metals usually conduct electricity because

Answer

Metals are decomposed by current

Answer

Metals have high resistance

Answer

In metals the ions are free to more

Answer

They are mobile electrons in the metallic structure

Question 29

29. The osmotic pressure of 1 m solution at 27°C is

Question 30

30. 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 31

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

Question 32

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

Question 33

33. The best reducing agent is

Question 34

34. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

Question 35

35. The amount of electricity that can deposit 108 g of silver from silver nitrate solution is

Question 36

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

Question 37

37. Specific conductivity of a solution

Answer

Increases with dilution

Answer

Decreases with dilution

Answer

Remains unchanged with dilution

Answer

Depends on mass of electrolyte

Question 38

38. Oxidation state of hydrogen in CaH₂ is

Question 39

39. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

Question 40

40. An oxidizing agent in a chemical reaction in the substance which

Answer

Acts as a catalyst

Answer

pH is changed

Answer

Gains electrons

Answer

Loses electrons

Question 41

41. When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

Question 42

42. When electricity is passed through molten Al₂O₃ + Na₃AIF₆ and 13.5 gms of Al are deposited, the number of faraday must be

Question 43

43. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

Answer

278 S cm² mol¯¹

Answer

176 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Answer

128 S cm² mol¯¹

Question 44

44. When common salt is dissolved in water

Answer

B.P of water increase

Answer

B.P of water remain constant

Answer

B.P of water decrease

Answer

Any possibility

Question 45

45. Corrosion is basically a

Answer

Altered reaction in presence of H₂O

Answer

Union between two light metals and a heavy metal

Answer

Interaction

Answer

Electrochemical phenomenon

Question 46

46. By means of fuel cells, chemical energy may be converted into

Answer

Sound energy

Answer

Magnetic energy

Answer

Heat energy

Answer

Electrical energy

Question 47

47. The reference calomel electrode is made from which of the following?

Answer

Hg₂Cl₂

Question 48

48. Electrochemical series is a list of elements arranged into increasing order to either

Answer

Standard oxidation potential

Answer

Cell voltage

Answer

Standard reduction potential

Answer

Ionization potential

Question 49

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

Question 50

50. Calculate the percentage by weight if NaCl, if 2.0 g of NaCl is dissolved in 20g of water

Question 51

51. Conductivity (Unit : siemen’s S) is directly proportionally to the area of the vessel and the concentration of the solution in it and is inversely proportional to the length of vessel, then the unit of constant of proportionality is

Answer

S² m² mol

Answer

S² m² mol¯²

Answer

S m mol¯¹

Answer

S m² mol¯¹

Question 52

52. Half cells are interconnected through

Answer

Electric circuit

Answer

No connection exists

Answer

Salt Bridge

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. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 55

55. Camphor is often used in molecular mass determination because

Answer

It is volatile

Answer

It has a very high cryoscopic constant

Answer

It is readily available

Answer

It is solvent for organic substances

Question 56

56. During a redox reaction, an oxidizing agent

Answer

Gains electrons

Answer

Is hydrolysed

Answer

Loses electrons

Answer

Is oxidized

Question 57

57. Which of the following statements is FALSE?

Answer

All electrochemical reactions involve the transfer of electrons

Answer

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

Answer

Reduction occurs at cathode

Answer

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

Question 58

58. Corrosion reactions are

Answer

Non-spontaneous redox reactions

Answer

Spontaneous redox reactions

Answer

None of these

Answer

Spontaneous acid–base reactions

Question 59

59. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

Answer

None of these

Question 60

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

Answer

One gm. Equivalent weight

Answer

Electrochemical equivalent

Answer

One gm. atomic weight

Answer

None of these

Question 61

61. In a Galvanic cell

Answer

Electrical energy is converted into chemical energy

Answer

Electrical energy is converted into heat

Answer

Chemical energy is converted into heat

Answer

Chemical energy is converted into electricity

Question 62

62. Strong reducing agents have

Answer

Greater positive value of standard reduction potential

Answer

Lesser positive value of standard reduction potential

Answer

None of these

Answer

Greater negative value of standard reduction potential

Question 63

63. Choose the best reducing agent among the following

Question 64

64. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Answer 104

Both Na⁺ and CI¯

Answer 105

None of these

Answer 106

31.75 g of Cu

Answer 107

100 g of Cu

Answer 108

96500 g of CU

Answer 109

63.5 g of Cu

Answer 110

Ion combination reaction

Answer 111

Proton transfer

Answer 112

Electron transfer

Answer 113

A reaction in a solution

Answer 114

0.1 M BaCl₂

Answer 115

0.1 M Sucrose

Answer 116

0.1 M Glucose

Answer 117

0.1 M NaCl

Answer 118

10.0g NaCl/100ml

Answer 119

20g NaCl/100ml

Answer 120

5.58g NaCl/100m

Answer 121

58.5g NaCl/100ml

Answer 122

Depends on the nature of the coupled electrode

Answer 123

Oxidation-reduction

Answer 124

Has low boiling point

Answer 125

Is neutral

Answer 126

Is almost unionized

Answer 127

Is readily decomposed

Answer 128

Boiling point

Answer 129

Sublimation point

Answer 130

Inversion point

Answer 131

Melting point

Answer 132

CH₃ CooNH₄

Answer 133

Na₂SO₄

Answer 134

1.15 g/Cm³

Answer 135

120 g Cm³

Answer 136

1.2 g/Cm³

Answer 137

1.25g/Cm³

Answer 138

Does not provide any electron

Answer 139

Neutral atom

Answer 140

Weak acid and its salt of strong base

Answer 141

Strong acid and its salt of weak base

Answer 142

A strong acid and its salt of a strong base

Answer 143

Weak acid and its salt of weak base

Answer 144

It has not potential

Answer 145

Gives ions only when dissolved in water

Answer 146

Possesses ions even in solid state

Answer 147

Forms complex ions in solution

Answer 148

Gives ions only when electricity is passed

Answer 149

H+ and OH-

Answer 150

Increase in oxidation number of element

Answer 151

Increase in oxidation number of the elements in reactants

Answer 152

Decrease in oxidation number of element

Answer 153

Oxidation number neither increases nor decreases

Answer 154

– 0.35 V

Answer 155

– 1.17 V

Answer 156

∆ G = -ve

Answer 157

∆ G = +ve, ∆ E = 0

Answer 158

∆ G = -ve, ∆ E = 0

Answer 159

∆ G = 0, ∆E = 0

Answer 160

Not particular

Answer 161

Conduction

Answer 162

Electrolysis

Answer 163

Electroplating

Answer 164

Galvanic cell

Answer 165

Electrolytic cell

Answer 166

760 mm of Hg

Answer 167

Slightly more than 1 atom

Answer 168

None of these

Answer 169

Spontaneous reaction

Answer 170

Non-spontaneous reaction

Answer 171

Neutralization

Answer 172

Raoult’s law

Answer 173

Henry’s law

Answer 174

Ostwald’s dilution law

Answer 175

Distribution law

Answer 176

Ostwald’s law

Answer 177

Raoult’s law

Answer 178

Henry’s law

Answer 179

Arrhenius law

Answer 180

1 – 2 α

Answer 181

A galvanic cell

Answer 182

A voltaic cell

Answer 183

A chemical cell

Answer 184

An electrolytic cell

Answer 185

Mole fraction of the solution

Answer 186

Molality of the solution

Answer 187

Molarity of the solvent

Answer 188

Molarity of the solution

Answer 189

Precipitated

Answer 190

Hydrolyzed

Answer 191

None of these

Answer 192

Electroplating

Answer 193

Both A and B

Answer 194

Electrorefining

Answer 195

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 196

Boiling point of pure water decreases by the addition of ethanol

Answer 197

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

Answer 198

Boiling point of pure benzene increases by the addition of toluene

Answer 199

Daniel cell

Answer 200

Electrolytic cell

Answer 201

Galvanic cell

Answer 202

[Pt(NH₃)₄Cl₃]Cl

Answer 203

[Pt(NH₃)₄Cl₂]Cl₂

Answer 204

[Pt(NH₃)₄Cl₄]

Answer 205

[Pt(NH₃)₄Cl]Cl₃

Answer 206

Electrons flow from cathode to anode through the external battery

Answer 207

Electrons flow cathode to anode within the electrolytic solution

Answer 208

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

Answer 209

None of these

Answer 210

Sufficient date not given

Answer 211

Chemical energy is converted into electrical energy

Answer 212

Salt bridge maintains the electrical neutrality of the solution

Answer 213

Electrons are released at anode

Answer 214

Cathode is regarded as negative electrode

Answer 215

Gold is denser

Answer 216

Iron rusts

Answer 217

Gold has higher reduction potential then iron

Answer 218

Gold has lower reduction potential then iron

Answer 219

None of these

Answer 220

Create potential difference between two electrodes

Answer 221

Generate heat

Answer 222

Remove adsorbed oxygen from electrode surfaces

Answer 223

Produce high purity water

Answer 224

Solvent particles

Answer 225

2.0 x 10¹¹

Answer 226

1.0 x 10²

Answer 227

4.0 x 10¹²

Answer 228

1.0 x 10¹⁰

Answer 229

Cathode to anode through the external circuit

Answer 230

Anode to cathode through the external circuit

Answer 231

Anode to cathode through the solution

Answer 232

Cathode to anode through the solution

Answer 233

None of these

Answer 234

O₂, SO₂

Answer 235

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

Answer 236

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

Answer 237

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

Answer 238

Li is smaller in size as compared to Cu

Answer 239

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

Answer 240

The enthalpy of mixing is zero

Answer 241

The free energy of mixing is zero

Answer 242

The entropy of mixing is zero

Answer 243

None of these

Answer 244

Slightly greater than one

Answer 245

Exactly equal to one

Answer 246

Slightly less than one

Answer 247

Slightly more than the total volume of the components

Answer 248

Equal to the total volume of the components

Answer 249

Slightly less than the total volume of the components

Answer 250

None of these

Answer 251

Hypertonic

Answer 252

H₄P₃O₇

Answer 253

Hg₂Cl₂

Answer 254

22400 cm³

Answer 255

Rechargeable

Answer 256

Daniel cell

Answer 257

Non rechargeable

Answer 258

Electrolytic cell

Answer 259

1.06 x 10⁴

Answer 260

1.06 x 10³

Answer 261

1.06 x 10²

Answer 262

Electrolysis

Answer 263

Galvanization

Answer 264

Photo electrolysis

Answer 265

Cathodic protection

Answer 266

Elevation in boiling point

Answer 267

Flow of solvent from a concentrated to a dilute solution

Answer 268

Diffusion rate of the solute

Answer 269

Ionic concentration

Answer 270

Concentration solutions behave as nearly non – ideal solutions

Answer 271

Dilute solution which behave as nearly ideal solution

Answer 272

Neither a nor b

Answer 273

Both a and b

Answer 274

Neutralization

Answer 275

None of these

Answer 276

Heat energy

Answer 277

Electrical energy

Answer 278

Chemical energy

Answer 279

12157.48 sec

Answer 280

By replacing external circuit with external source of electricity

Answer 281

By removal of solution

Answer 282

By addition of fresh solution

Answer 283

By heating it

Answer 284

Decrease rapidly

Answer 285

Decreases slowly

Answer 286

Drops to zero

Answer 287

Does not change

Answer 288

Making leather

Answer 289

Manufacture of bleach

Answer 290

Rust removal

Answer 291

Electroplating

Answer 292

Vacuum distillation

Answer 293

None of these

Answer 294

Distillation

Answer 295

Fractional distillation

Answer 296

Very high positive value of reduction potential

Answer 297

Very low ionization potential values

Answer 298

Very high negative values reduction potential

Answer 299

Reduction potentials are negative

Answer 300

Ohm¯¹ cm

Answer 301

Ohm¯¹ cm¯¹

Answer 302

Ohm cm¯¹

Answer 303

Ohm cm¯²

Answer 304

Pt and graphite only

Answer 305

Na, Pt and graphite

Answer 306

Na and S only

Answer 307

Free molecules

Answer 308

Free electrons

Answer 309

Atoms of Na and Cl.

Answer 310

Increase in oxidation number of all the elements on reactant side

Answer 311

Decrease in oxidation number

Answer 312

Both are possible

Answer 313

Increase in oxidation number

Answer 314

Ca(NO₃)₂

Answer 315

From cathode to anode inside the cell

Answer 316

From anode to cathode in an outer circuit

Answer 317

From anode to cathode inside the cell

Answer 318

From cathode to anode in outer circuit

Answer 319

Thomas Gradam

Answer 320

Gram per million

Answer 321

Milligram percent

Answer 322

Microgram percent

Answer 323

Parts per million

Answer 324

Redox potential

Answer 325

e.m.f of cell

Answer 326

Reduction potential

Answer 327

Oxidation potential

Answer 328

Depends on density of electrolyte itself.

Answer 329

Does not change on dilution

Answer 330

Increases on dilution slightly

Answer 331

Decreases on dilution

Answer 332

Equal to that of water

Answer 333

Equal to that of ethanol

Answer 334

More than that of H₂O

Answer 335

Less than that of water

Answer 336

Sulphuric acid

Answer 337

Boric acid

Answer 338

Nitric acid

Answer 339

Phosphorus acid

Answer 340

Both A and B

Answer 341

None of these

Answer 342

At cathode

Answer 343

760 mm of Hg

Answer 344

750 mm of Hg

Answer 345

800 mm of Hg

Answer 346

780 mm of Hg

Answer 347

Both of these

Answer 348

Making iron cathode

Answer 349

Putting it in saline water

Answer 350

None of these

Answer 351

0.918 cm¯¹

Answer 352

1.12 cm¯¹

Answer 353

0.142 cm¯¹

Answer 354

0.66 cm¯¹

Answer 355

Sum of reduction and oxidation potentials

Answer 356

Surface tension

Answer 357

Refractive index

Answer 358

Osmotic pressure

Answer 359

Dilution increases

Answer 360

Dilution decreases

Answer 361

Pressure increases

Answer 362

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

Answer 363

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

Answer 364

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

Answer 365

Hg is more inert than Pt

Answer 366

Na⁺ + e– → Na

Answer 367

Br₂ + 2e – → 2Br –

Answer 368

Na → Na⁺ + e–

Answer 369

2Br– → Br₂ + 2e –

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