Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Cathode provides electrons to

Answer

Does not provide any electron

Answer

Neutral atom

Question 2

2. In a chemical reaction, oxidation process involves

Answer

Increase in oxidation number of element

Answer

Oxidation number neither increases nor decreases

Answer

Increase in oxidation number of the elements in reactants

Answer

Decrease in oxidation number of element

Question 3

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 4

4. Metals usually conduct electricity because

Answer

Metals are decomposed by current

Answer

Metals have high resistance

Answer

They are mobile electrons in the metallic structure

Answer

In metals the ions are free to more

Question 5

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

Question 6

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

Question 7

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

Answer

Unsaturated

Answer

Supersaturated

Question 8

8. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 9

9. Which of the following (IM) conducts more electricity?

Answer

Phosphorus acid

Answer

Boric acid

Answer

Nitric acid

Answer

Sulphuric acid

Question 10

10. The electrode with more negative value of reduction potential acts as

Answer

None of these

Question 11

11. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 12

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

Question 13

13. 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 14

14. During a redox reaction, an oxidizing agent

Answer

Is hydrolysed

Answer

Loses electrons

Answer

Gains electrons

Answer

Is oxidized

Question 15

15. In an electrolytic cell current flows

Answer

From cathode to anode in outer circuit

Answer

From anode to cathode inside the cell

Answer

From cathode to anode inside the cell

Answer

From anode to cathode in an outer circuit

Question 16

16. 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 17

17. When common salt is dissolved in water

Answer

B.P of water remain constant

Answer

B.P of water decrease

Answer

Any possibility

Answer

B.P of water increase

Question 18

18. Half cells are interconnected through

Answer

Salt Bridge

Answer

Electric circuit

Answer

No connection exists

Question 19

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

Question 20

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

Question 21

21. 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

1.0 x 10¹⁰

Answer

2.0 x 10¹¹

Answer

1.0 x 10²

Answer

4.0 x 10¹²

Question 22

22. Reduction always occurs

Answer

At cathode

Answer

None of these

Answer

Both A and B

Question 23

23. A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If Kf for water is 1.80, the correct formulation for the above molecule is

Answer

[Pt(NH₃)₄Cl₃]Cl

Answer

[Pt(NH₃)₄Cl]Cl₃

Answer

[Pt(NH₃)₄Cl₄]

Answer

[Pt(NH₃)₄Cl₂]Cl₂

Question 24

24. In a Galvanic cell

Answer

Chemical energy is converted into electricity

Answer

Electrical energy is converted into heat

Answer

Chemical energy is converted into heat

Answer

Electrical energy is converted into chemical energy

Question 25

25. In a Galvanic cell, the electrons flow from

Answer

Cathode to anode through the external circuit

Answer

Anode to cathode through the solution

Answer

Cathode to anode through the solution

Answer

Anode to cathode through the external circuit

Question 26

26. The osmotic pressure of a dilute solution is directly proportional to the

Answer

Ionic concentration

Answer

Diffusion rate of the solute

Answer

Flow of solvent from a concentrated to a dilute solution

Answer

Elevation in boiling point

Question 27

27. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 28

28. Electrode potential of Zn is

Answer

Oxidation-reduction

Answer

Depends on the nature of the coupled electrode

Question 29

29. 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 30

30. Choose the cell among the following list in which conversation of electrical energy into chemical energy takes place

Answer

Galvanic cell

Answer

Electrolytic cell

Answer

Daniel cell

Question 31

31. A cell constant is generally found by measuring the conductivity of aqueous solution of

Question 32

32. Of the following, the metal that cannot be obtained by electrolysis of aqueous solution of their salts are:

Question 33

33. Density of H₂SO₄ in lead accumulator is

Question 34

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

Answer

Electroplating

Answer

Electrorefining

Answer

None of these

Answer

Both A and B

Question 35

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

Answer

Very low ionization potential values

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Answer

Very high positive value of reduction potential

Question 36

36. In a solution of CuSO₄ how much time will be required to precipitate 2g copper by 0.5 ampere current?

Answer

12157.48 sec

Question 37

37. The best reducing agent is

Question 38

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

Answer

Fractional distillation

Answer

Distillation

Answer

Vacuum distillation

Answer

None of these

Question 39

39. What are the ions present in water?

Answer

H+ and OH-

Question 40

40. If α is the degree of dissociation of Na₂SO₄ the Vant Hoff’s factor (i) used for calculating the molecular mass is

Answer

1 – 2 α

Question 41

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

Answer

0.1 N NaCl

Question 42

42. 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 43

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

Answer

0.1 M BaCl₂

Answer

0.1 M Sucrose

Answer

0.1 M NaCl

Answer

0.1 M Glucose

Question 44

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

Answer

Iron rusts

Answer

Gold has higher reduction potential then iron

Answer

Gold has lower reduction potential then iron

Answer

Gold is denser

Question 45

45. 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 46

46. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 47

47. H₂ gas in SHE is filled at a pressure of

Answer

760 mm of Hg

Answer

780 mm of Hg

Answer

750 mm of Hg

Answer

800 mm of Hg

Question 48

48. The pressure at which water boils at 101.5 °c is

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 49

49. In alkaline battery anode is made up of

Question 50

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

Question 51

51. Camphor is often used in molecular mass determination because

Answer

It is readily available

Answer

It is solvent for organic substances

Answer

It has a very high cryoscopic constant

Answer

It is volatile

Question 52

52. Oxidation in a chemical reaction involves

Answer

Increase in oxidation number

Answer

Decrease in oxidation number

Answer

Increase in oxidation number of all the elements on reactant side

Answer

Both are possible

Question 53

53. 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 54

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

Answer

None of these

Answer

Both Na⁺ and CI¯

Question 55

55. 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 56

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 57

57. A redox reaction involves

Answer

Electron transfer

Answer

A reaction in a solution

Answer

Ion combination reaction

Answer

Proton transfer

Question 58

58. Salt bridge transfers

Answer

Solvent particles

Question 59

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

Question 60

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

Question 61

61. Azeotropic mixture of HCl and water has

Question 62

62. 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 63

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

Question 64

64. The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO₄ is

Answer 117

Henry’s law

Answer 118

Raoult’s law

Answer 119

Arrhenius law

Answer 120

Ostwald’s law

Answer 121

Sufficient date not given

Answer 122

Electrons flow from cathode to anode through the external battery

Answer 123

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

Answer 124

None of these

Answer 125

Electrons flow cathode to anode within the electrolytic solution

Answer 126

Electrical energy

Answer 127

Heat energy

Answer 128

Magnetic energy

Answer 129

Sound energy

Answer 130

Making leather

Answer 131

Electroplating

Answer 132

Rust removal

Answer 133

Manufacture of bleach

Answer 134

Non rechargeable

Answer 135

Electrolytic cell

Answer 136

Daniel cell

Answer 137

Rechargeable

Answer 138

Atoms of Na and Cl.

Answer 139

Free electrons

Answer 140

Free molecules

Answer 141

Ohm¯¹ cm¯¹

Answer 142

Ohm cm¯¹

Answer 143

Ohm cm¯²

Answer 144

Ohm¯¹ cm

Answer 145

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

Answer 146

The free energy of mixing is zero

Answer 147

The entropy of mixing is zero

Answer 148

The enthalpy of mixing is zero

Answer 149

Does not change on dilution

Answer 150

Increases on dilution slightly

Answer 151

Depends on density of electrolyte itself.

Answer 152

Decreases on dilution

Answer 153

Putting it in saline water

Answer 154

Making iron cathode

Answer 155

Both of these

Answer 156

None of these

Answer 157

1.2 g/Cm³

Answer 158

1.25g/Cm³

Answer 159

120 g Cm³

Answer 160

1.15 g/Cm³

Answer 161

1.06 x 10²

Answer 162

1.06 x 10³

Answer 163

1.06 x 10⁴

Answer 164

None of these

Answer 165

Boiling point of pure water decreases by the addition of ethanol

Answer 166

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

Answer 167

Boiling point of pure benzene increases by the addition of toluene

Answer 168

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 169

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

Answer 170

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

Answer 171

Li is smaller in size as compared to Cu

Answer 172

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

Answer 173

Cathodic protection

Answer 174

Galvanization

Answer 175

Electrolysis

Answer 176

Photo electrolysis

Answer 177

The extent of dissolution of solute

Answer 178

The extent of dissociation of solute

Answer 179

The degree of decomposition of solution

Answer 180

Degree of solubilization of solute

Answer 181

Is neutral

Answer 182

Has low boiling point

Answer 183

Is almost unionized

Answer 184

Is readily decomposed

Answer 185

Surface tension

Answer 186

Refractive index

Answer 187

Osmotic pressure

Answer 188

Reduction potential

Answer 189

Redox potential

Answer 190

e.m.f of cell

Answer 191

Oxidation potential

Answer 192

Dilute solution which behave as nearly ideal solution

Answer 193

Neither a nor b

Answer 194

Concentration solutions behave as nearly non – ideal solutions

Answer 195

Both a and b

Answer 196

∆ G = 0, ∆E = 0

Answer 197

∆ G = +ve, ∆ E = 0

Answer 198

∆ G = -ve

Answer 199

∆ G = -ve, ∆ E = 0

Answer 200

Electrons are released at anode

Answer 201

Chemical energy is converted into electrical energy

Answer 202

Cathode is regarded as negative electrode

Answer 203

Salt bridge maintains the electrical neutrality of the solution

Answer 204

None of these

Answer 205

128 S cm² mol¯¹

Answer 206

176 S cm² mol¯¹

Answer 207

302 S cm² mol¯¹

Answer 208

278 S cm² mol¯¹

Answer 209

Thomas Gradam

Answer 210

Hypertonic

Answer 211

Increases gradually

Answer 212

Drops to zero

Answer 213

Increases rapidly

Answer 214

Does not change

Answer 215

It has not potential

Answer 216

1.81 cm¯³

Answer 217

2.15 cm¯³

Answer 218

1.25 cm¯³

Answer 219

1.15 cm¯³

Answer 220

Precipitated

Answer 221

Hydrolyzed

Answer 222

Ostwald’s dilution law

Answer 223

Raoult’s law

Answer 224

Henry’s law

Answer 225

Distribution law

Answer 226

Ionization

Answer 227

Hydrolysis

Answer 228

All of these

Answer 229

Temperature

Answer 230

Nature of the gas

Answer 231

Pressure of the gas

Answer 232

Sum of reduction and oxidation potentials

Answer 233

Not particular

Answer 234

Increases with dilution

Answer 235

Depends on mass of electrolyte

Answer 236

Decreases with dilution

Answer 237

Remains unchanged with dilution

Answer 238

Melting point

Answer 239

Boiling point

Answer 240

Inversion point

Answer 241

Sublimation point

Answer 242

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

Answer 243

All electrochemical reactions involve the transfer of electrons

Answer 244

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

Answer 245

Reduction occurs at cathode

Answer 246

Cell voltage

Answer 247

Standard oxidation potential

Answer 248

Ionization potential

Answer 249

Standard reduction potential

Answer 250

Electroplating

Answer 251

Electric change

Answer 252

Ionization potential

Answer 253

Standard electrode potential

Answer 254

CH₃ CooNH₄

Answer 255

Na₂SO₄

Answer 256

Hg₂Cl₂

Answer 257

Possesses ions even in solid state

Answer 258

Gives ions only when electricity is passed

Answer 259

Forms complex ions in solution

Answer 260

Gives ions only when dissolved in water

Answer 261

Na and S only

Answer 262

Na, Pt and graphite

Answer 263

Pt and graphite only

Answer 264

Union between two light metals and a heavy metal

Answer 265

Altered reaction in presence of H₂O

Answer 266

Interaction

Answer 267

Electrochemical phenomenon

Answer 268

Galvanic cell

Answer 269

Electrolytic cell

Answer 270

Neutralization

Answer 271

Non-spontaneous reaction

Answer 272

Spontaneous reaction

Answer 273

Equal to that of water

Answer 274

Less than that of water

Answer 275

More than that of H₂O

Answer 276

Equal to that of ethanol

Answer 277

Pressure increases

Answer 278

Dilution decreases

Answer 279

Dilution increases

Answer 280

Lesser positive value of standard reduction potential

Answer 281

Greater positive value of standard reduction potential

Answer 282

Greater negative value of standard reduction potential

Answer 283

None of these

Answer 284

2Br– → Br₂ + 2e –

Answer 285

Na⁺ + e– → Na

Answer 286

Na → Na⁺ + e–

Answer 287

Br₂ + 2e – → 2Br –

Answer 288

0.66 cm¯¹

Answer 289

0.918 cm¯¹

Answer 290

1.12 cm¯¹

Answer 291

0.142 cm¯¹

Answer 292

H₄P₃O₇

Answer 293

Dilute solution of glucose

Answer 294

Chloroform

Answer 295

Molten NaCl

Answer 296

Pure distilled water

Answer 297

Exactly equal to one

Answer 298

Slightly greater than one

Answer 299

Slightly less than one

Answer 300

None of these

Answer 301

Ca(NO₃)₂

Answer 302

Weak acid and its salt of weak base

Answer 303

Strong acid and its salt of weak base

Answer 304

Weak acid and its salt of strong base

Answer 305

A strong acid and its salt of a strong base

Answer 306

Electrical energy

Answer 307

Heat energy

Answer 308

Chemical energy

Answer 309

None of these

Answer 310

A galvanic cell

Answer 311

An electrolytic cell

Answer 312

A chemical cell

Answer 313

A voltaic cell

Answer 314

By removal of solution

Answer 315

By heating it

Answer 316

By replacing external circuit with external source of electricity

Answer 317

By addition of fresh solution

Answer 318

All of these

Answer 319

Mole fraction of the solution

Answer 320

Molality of the solution

Answer 321

Molarity of the solution

Answer 322

Molarity of the solvent

Answer 323

Non-spontaneous redox reactions

Answer 324

Spontaneous acid–base reactions

Answer 325

Spontaneous redox reactions

Answer 326

None of these

Answer 327

Acts as a catalyst

Answer 328

pH is changed

Answer 329

Loses electrons

Answer 330

Gains electrons

Answer 331

10.0g NaCl/100ml

Answer 332

5.58g NaCl/100m

Answer 333

58.5g NaCl/100ml

Answer 334

20g NaCl/100ml

Answer 335

None of these

Answer 336

O₂, SO₂

Answer 337

S² m² mol

Answer 338

S m² mol¯¹

Answer 339

S² m² mol¯²

Answer 340

S m mol¯¹

Answer 341

Decrease rapidly

Answer 342

Does not change

Answer 343

Decreases slowly

Answer 344

Drops to zero

Answer 345

100 g of Cu

Answer 346

96500 g of CU

Answer 347

31.75 g of Cu

Answer 348

63.5 g of Cu

Answer 349

Parts per million

Answer 350

Milligram percent

Answer 351

Microgram percent

Answer 352

Gram per million

Answer 353

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

Answer 354

Hg is more inert than Pt

Answer 355

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

Answer 356

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

Answer 357

Hg₂Cl₂

Answer 358

Slightly more than the total volume of the components

Answer 359

None of these

Answer 360

Slightly less than the total volume of the components

Answer 361

Equal to the total volume of the components

Answer 362

Conduction

Answer 363

Electrolysis

Answer 364

Electroplating

Answer 365

Naphthalene

Answer 366

Remove adsorbed oxygen from electrode surfaces

Answer 367

Generate heat

Answer 368

Produce high purity water

Answer 369

Create potential difference between two electrodes

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