Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Voltaic cell can be recharged by

Answer

By replacing external circuit with external source of electricity

Answer

By heating it

Answer

By removal of solution

Answer

By addition of fresh solution

Question 2

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

Question 3

3. Cathodic reaction in the electrolysis of dil. H₂SO₄ is always

Question 4

4. In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

Answer

Produce high purity water

Answer

Generate heat

Answer

Create potential difference between two electrodes

Answer

Remove adsorbed oxygen from electrode surfaces

Question 5

5. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

Answer

Slightly less than the total volume of the components

Answer

None of these

Answer

Slightly more than the total volume of the components

Answer

Equal to the total volume of the components

Question 6

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

Answer

Distribution law

Answer

Henry’s law

Answer

Raoult’s law

Answer

Ostwald’s dilution law

Question 7

7. The process of electrical coating of one metal on another to protect, decorate or to have a greater resistance to corrosion is called

Answer

Electrolysis

Answer

Electroplating

Answer

Conduction

Question 8

8. Which substances are mixed to form a buffer solution?

Answer

Weak acid and its salt of strong base

Answer

Weak acid and its salt of weak base

Answer

A strong acid and its salt of a strong base

Answer

Strong acid and its salt of weak base

Question 9

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

Question 10

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

Answer

1.15 cm¯³

Answer

1.81 cm¯³

Answer

2.15 cm¯³

Answer

1.25 cm¯³

Question 11

11. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 12

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

Question 13

13. After adding a solute freezing point of solvent decreases to -0.186. Calculate ∆ Tb if Kf = 1.86 and Kb = 0.521

Question 14

14. In alkaline battery anode is made up of

Question 15

15. Azeotropic mixture of HCl and water has

Question 16

16. Best way to prevent rusting iron is by

Answer

Making iron cathode

Answer

Both of these

Answer

None of these

Answer

Putting it in saline water

Question 17

17. Density of H₂SO₄ in lead accumulator is

Answer

1.15 g/Cm³

Answer

1.25g/Cm³

Answer

1.2 g/Cm³

Answer

120 g Cm³

Question 18

18. Which of the following is the use of electrolysis?

Answer

Both A and B

Answer

None of these

Answer

Electroplating

Answer

Electrorefining

Question 19

19. If the salt bridge is not used between two half cells, then the voltage

Answer

Decrease rapidly

Answer

Does not change

Answer

Drops to zero

Answer

Decreases slowly

Question 20

20. Reaction takes place at anode is

Answer

Hydrolysis

Answer

Ionization

Question 21

21. 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 22

22. The degree of dissociation of weak electrolyte increases as

Answer

Pressure increases

Answer

Dilution decreases

Answer

Dilution increases

Question 23

23. 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 24

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

Answer

Hg₂Cl₂

Question 25

25. Electrolysis is the process in which a chemical reaction takes place at the expense of

Answer

Heat energy

Answer

Electrical energy

Answer

None of these

Answer

Chemical energy

Question 26

26. Cathode provides electrons to

Answer

Neutral atom

Answer

Does not provide any electron

Question 27

27. 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¯²

Answer

S m² mol¯¹

Answer

S² m² mol

Answer

S m mol¯¹

Question 28

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

Question 29

29. 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 30

30. Corrosion is basically a

Answer

Interaction

Answer

Electrochemical phenomenon

Answer

Union between two light metals and a heavy metal

Answer

Altered reaction in presence of H₂O

Question 31

31. When Cu, Ag, Au and Pt are reacted with acids, these metals do not liberate hydrogen, this is due to the reason that

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Answer

Very high positive value of reduction potential

Answer

Very low ionization potential values

Question 32

32. A solution contains 1.2046 x 10²⁴ hydrochloric acid molecules in one dm³ of the solution. The strength of the solution is

Question 33

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

Answer

Both oxidation and reduction

Answer

Neither oxidation and reduction

Question 34

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

Answer

None of these

Answer

O₂, SO₂

Question 35

35. The relative lowering of vapour pressure is equal to mole fraction of the solute. This law is called:

Answer

Arrhenius law

Answer

Ostwald’s law

Answer

Raoult’s law

Answer

Henry’s law

Question 36

36. The solubility of a gas in water depends upon

Answer

All of these

Answer

Nature of the gas

Answer

Pressure of the gas

Answer

Temperature

Question 37

37. An aqueous solution freezes at -0.186°C. (Kf = 1.86, Kb = 0.512). What is the elevation in boiling point?

Question 38

38. In alkaline battery the anode is made up of

Question 39

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

Question 40

40. A 20% solution of NaCl by weight means that

Answer

58.5g NaCl/100ml

Answer

10.0g NaCl/100ml

Answer

20g NaCl/100ml

Answer

5.58g NaCl/100m

Question 41

41. In an electrolytic cell current flows

Answer

From anode to cathode inside the cell

Answer

From anode to cathode in an outer circuit

Answer

From cathode to anode inside the cell

Answer

From cathode to anode in outer circuit

Question 42

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

Question 43

43. Sea water has 5.65 x 10¯³ g of dissolved oxygen calculate the conclusion of oxygen in sea water in ppx

Question 44

44. Which of the statements given below concerning properties of solution, describe a colligaive effect?

Answer

Boiling point of pure benzene increases by the addition of toluene

Answer

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer

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

Answer

Boiling point of pure water decreases by the addition of ethanol

Question 45

45. Metals usually conduct electricity because

Answer

In metals the ions are free to more

Answer

They are mobile electrons in the metallic structure

Answer

Metals have high resistance

Answer

Metals are decomposed by current

Question 46

46. Prevention of corrosion of iron by Zn coating is called

Answer

Galvanization

Answer

Cathodic protection

Answer

Photo electrolysis

Answer

Electrolysis

Question 47

47. Pure water does not conduct electricity because it

Answer

Has low boiling point

Answer

Is almost unionized

Answer

Is readily decomposed

Answer

Is neutral

Question 48

48. The strength of solution an element whose electrode potential is to be measured

Question 49

49. Which of the following statement is correct for electrolytic cell?

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

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

Answer

Electrons flow from cathode to anode through the external battery

Answer

None of these

Question 50

50. The art of electroplating was given by

Answer

Thomas Gradam

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. 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 53

53. Which of the following will have the highest boiling point at 1 atm pressure?

Answer

0.1 M Glucose

Answer

0.1 M NaCl

Answer

0.1 M Sucrose

Answer

0.1 M BaCl₂

Question 54

54. Salt bridge transfers

Question 55

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

Question 56

56. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 57

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

Answer

0.1 N NaCl

Question 58

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

Question 59

59. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 60

60. Separation of azeotropic mixture into pure components is carried out by

Answer

Vacuum distillation

Answer

Distillation

Answer

Fractional distillation

Answer

None of these

Question 61

61. Molton NaCl conducts electricity due to the presence of

Answer

Free electrons

Answer

Atoms of Na and Cl.

Answer

Free molecules

Question 62

62. The number of moles of a solute in 500 cm³, 3M solution is

Question 63

63. Temperature for standard electrode potential is

Question 64

64. Which has maximum oxidation number

Answer 123

Ionic concentration

Answer 124

Flow of solvent from a concentrated to a dilute solution

Answer 125

Diffusion rate of the solute

Answer 126

Elevation in boiling point

Answer 127

A voltaic cell

Answer 128

An electrolytic cell

Answer 129

A chemical cell

Answer 130

A galvanic cell

Answer 131

Osmotic pressure

Answer 132

Surface tension

Answer 133

Refractive index

Answer 134

Neutralization

Answer 135

Standard reduction potential

Answer 136

Standard oxidation potential

Answer 137

Ionization potential

Answer 138

Cell voltage

Answer 139

Br₂ + 2e – → 2Br –

Answer 140

2Br– → Br₂ + 2e –

Answer 141

Na⁺ + e– → Na

Answer 142

Na → Na⁺ + e–

Answer 143

31.75 g of Cu

Answer 144

96500 g of CU

Answer 145

63.5 g of Cu

Answer 146

100 g of Cu

Answer 147

750 mm of Hg

Answer 148

780 mm of Hg

Answer 149

760 mm of Hg

Answer 150

800 mm of Hg

Answer 151

278 S cm² mol¯¹

Answer 152

302 S cm² mol¯¹

Answer 153

128 S cm² mol¯¹

Answer 154

176 S cm² mol¯¹

Answer 155

Sulphuric acid

Answer 156

Phosphorus acid

Answer 157

Nitric acid

Answer 158

Boric acid

Answer 159

Ohm cm¯²

Answer 160

Ohm¯¹ cm¯¹

Answer 161

Ohm cm¯¹

Answer 162

Ohm¯¹ cm

Answer 163

Na₂SO₄

Answer 164

CH₃ CooNH₄

Answer 165

H₄P₃O₇

Answer 166

Spontaneous redox reactions

Answer 167

Non-spontaneous redox reactions

Answer 168

Spontaneous acid–base reactions

Answer 169

None of these

Answer 170

Increases gradually

Answer 171

Increases rapidly

Answer 172

Does not change

Answer 173

Drops to zero

Answer 174

Increase in oxidation number of the elements in reactants

Answer 175

Oxidation number neither increases nor decreases

Answer 176

Increase in oxidation number of element

Answer 177

Decrease in oxidation number of element

Answer 178

It has not potential

Answer 179

Rust removal

Answer 180

Electroplating

Answer 181

Manufacture of bleach

Answer 182

Making leather

Answer 183

None of these

Answer 184

12157.48 sec

Answer 185

Non rechargeable

Answer 186

Rechargeable

Answer 187

Electrolytic cell

Answer 188

Daniel cell

Answer 189

Electron transfer

Answer 190

Proton transfer

Answer 191

Ion combination reaction

Answer 192

A reaction in a solution

Answer 193

Electrolytic cell

Answer 194

Daniel cell

Answer 195

Galvanic cell

Answer 196

Not particular

Answer 197

e.m.f of cell

Answer 198

Redox potential

Answer 199

Oxidation potential

Answer 200

Reduction potential

Answer 201

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

Answer 202

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

Answer 203

Li is smaller in size as compared to Cu

Answer 204

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

Answer 205

Gives ions only when dissolved in water

Answer 206

Forms complex ions in solution

Answer 207

Gives ions only when electricity is passed

Answer 208

Possesses ions even in solid state

Answer 209

Boiling point

Answer 210

Melting point

Answer 211

Sublimation point

Answer 212

Inversion point

Answer 213

Depends on the nature of the coupled electrode

Answer 214

Oxidation-reduction

Answer 215

Increase in oxidation number of all the elements on reactant side

Answer 216

Decrease in oxidation number

Answer 217

Both are possible

Answer 218

Increase in oxidation number

Answer 219

Hypertonic

Answer 220

Na, Pt and graphite

Answer 221

Na and S only

Answer 222

Pt and graphite only

Answer 223

Milligram percent

Answer 224

Gram per million

Answer 225

Microgram percent

Answer 226

Parts per million

Answer 227

Slightly greater than one

Answer 228

None of these

Answer 229

Exactly equal to one

Answer 230

Slightly less than one

Answer 231

– 0.35 V

Answer 232

– 1.17 V

Answer 233

Cathode to anode through the solution

Answer 234

Cathode to anode through the external circuit

Answer 235

Anode to cathode through the external circuit

Answer 236

Anode to cathode through the solution

Answer 237

Non-spontaneous reaction

Answer 238

Spontaneous reaction

Answer 239

Neutralization

Answer 240

B.P of water increase

Answer 241

B.P of water remain constant

Answer 242

Any possibility

Answer 243

B.P of water decrease

Answer 244

Less than that of water

Answer 245

Equal to that of ethanol

Answer 246

More than that of H₂O

Answer 247

Equal to that of water

Answer 248

Electrochemical equivalent

Answer 249

One gm. atomic weight

Answer 250

None of these

Answer 251

One gm. Equivalent weight

Answer 252

1 – 2 α

Answer 253

Molarity of the solvent

Answer 254

Mole fraction of the solution

Answer 255

Molarity of the solution

Answer 256

Molality of the solution

Answer 257

Decreases with dilution

Answer 258

Remains unchanged with dilution

Answer 259

Increases with dilution

Answer 260

Depends on mass of electrolyte

Answer 261

Precipitated

Answer 262

Hydrolyzed

Answer 263

Decreases on dilution

Answer 264

Does not change on dilution

Answer 265

Depends on density of electrolyte itself.

Answer 266

Increases on dilution slightly

Answer 267

None of these

Answer 268

Greater positive value of standard reduction potential

Answer 269

Greater negative value of standard reduction potential

Answer 270

Lesser positive value of standard reduction potential

Answer 271

∆ G = -ve, ∆ E = 0

Answer 272

∆ G = +ve, ∆ E = 0

Answer 273

∆ G = -ve

Answer 274

∆ G = 0, ∆E = 0

Answer 275

1.06 x 10²

Answer 276

1.06 x 10⁴

Answer 277

1.06 x 10³

Answer 278

The degree of decomposition of solution

Answer 279

The extent of dissolution of solute

Answer 280

The extent of dissociation of solute

Answer 281

Degree of solubilization of solute

Answer 282

Electroplating

Answer 283

Standard electrode potential

Answer 284

Ionization potential

Answer 285

Electric change

Answer 286

Chemical energy is converted into heat

Answer 287

Chemical energy is converted into electricity

Answer 288

Electrical energy is converted into chemical energy

Answer 289

Electrical energy is converted into heat

Answer 290

Both a and b

Answer 291

Dilute solution which behave as nearly ideal solution

Answer 292

Neither a nor b

Answer 293

Concentration solutions behave as nearly non – ideal solutions

Answer 294

Gold has higher reduction potential then iron

Answer 295

Gold has lower reduction potential then iron

Answer 296

Iron rusts

Answer 297

Gold is denser

Answer 298

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

Answer 299

The enthalpy of mixing is zero

Answer 300

The free energy of mixing is zero

Answer 301

The entropy of mixing is zero

Answer 302

Cathode is regarded as negative electrode

Answer 303

Electrons are released at anode

Answer 304

Salt bridge maintains the electrical neutrality of the solution

Answer 305

Chemical energy is converted into electrical energy

Answer 306

1.12 cm¯¹

Answer 307

0.142 cm¯¹

Answer 308

0.66 cm¯¹

Answer 309

0.918 cm¯¹

Answer 310

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

Answer 311

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

Answer 312

Hg is more inert than Pt

Answer 313

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

Answer 314

Sufficient date not given

Answer 315

[Pt(NH₃)₄Cl₂]Cl₂

Answer 316

[Pt(NH₃)₄Cl₃]Cl

Answer 317

[Pt(NH₃)₄Cl₄]

Answer 318

[Pt(NH₃)₄Cl]Cl₃

Answer 319

All of these

Answer 320

Reduction occurs at cathode

Answer 321

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

Answer 322

All electrochemical reactions involve the transfer of electrons

Answer 323

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

Answer 324

Sum of reduction and oxidation potentials

Answer 325

Hg₂Cl₂

Answer 326

22400 cm³

Answer 327

None of these

Answer 328

At cathode

Answer 329

Both A and B

Answer 330

Naphthalene

Answer 331

It is volatile

Answer 332

It is solvent for organic substances

Answer 333

It has a very high cryoscopic constant

Answer 334

It is readily available

Answer 335

Ca(NO₃)₂

Answer 336

Electric circuit

Answer 337

Salt Bridge

Answer 338

No connection exists

Answer 339

760 mm of Hg

Answer 340

Slightly more than 1 atom

Answer 341

Pure distilled water

Answer 342

Chloroform

Answer 343

Molten NaCl

Answer 344

Dilute solution of glucose

Answer 345

1.0 x 10²

Answer 346

4.0 x 10¹²

Answer 347

2.0 x 10¹¹

Answer 348

1.0 x 10¹⁰

Answer 349

Solvent particles

Answer 350

H+ and OH-

Answer 351

Magnetic energy

Answer 352

Sound energy

Answer 353

Electrical energy

Answer 354

Heat energy

Answer 355

Loses electrons

Answer 356

pH is changed

Answer 357

Gains electrons

Answer 358

Acts as a catalyst

Answer 359

Unsaturated

Answer 360

Supersaturated

Answer 361

None of these

Answer 362

Electrolytic cell

Answer 363

Galvanic cell

Answer 364

Both Na⁺ and CI¯

Answer 365

None of these

Answer 366

Is hydrolysed

Answer 367

Loses electrons

Answer 368

Is oxidized

Answer 369

Gains electrons

Total Questions:	192
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Total Marks:	192
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