Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. During a redox reaction, an oxidizing agent

Answer

Loses electrons

Answer

Gains electrons

Answer

Is oxidized

Answer

Is hydrolysed

Question 2

2. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 3

3. 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 4

4. In a chemical reaction, oxidation process involves

Answer

Decrease in oxidation number of element

Answer

Oxidation number neither increases nor decreases

Answer

Increase in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Question 5

5. In alkaline battery the anode is made up of

Question 6

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

Answer

Drops to zero

Answer

Increases gradually

Answer

Increases rapidly

Answer

Does not change

Question 7

7. Salt bridge transfers

Answer

Solvent particles

Question 8

8. In galvanic cell Zn acts as an anode so its value of standard reduction potential in comparison to coupled electrode would be

Answer

Sum of reduction and oxidation potentials

Question 9

9. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

Answer

0.66 cm¯¹

Answer

0.142 cm¯¹

Answer

0.918 cm¯¹

Answer

1.12 cm¯¹

Question 10

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

Question 11

11. The conductivity of strong electrolyte

Answer

Depends on density of electrolyte itself.

Answer

Decreases on dilution

Answer

Increases on dilution slightly

Answer

Does not change on dilution

Question 12

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

Answer

58.5g NaCl/100ml

Answer

5.58g NaCl/100m

Answer

20g NaCl/100ml

Answer

10.0g NaCl/100ml

Question 13

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

Answer

Precipitated

Answer

Hydrolyzed

Question 14

14. Corrosion is basically a

Answer

Union between two light metals and a heavy metal

Answer

Altered reaction in presence of H₂O

Answer

Electrochemical phenomenon

Answer

Interaction

Question 15

15. 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

S m² mol¯¹

Answer

S m mol¯¹

Answer

S² m² mol¯²

Question 16

16. 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)₄Cl₂]Cl₂

Answer

[Pt(NH₃)₄Cl]Cl₃

Answer

[Pt(NH₃)₄Cl₄]

Answer

[Pt(NH₃)₄Cl₃]Cl

Question 17

17. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

Answer

2Br– → Br₂ + 2e –

Answer

Na⁺ + e– → Na

Answer

Na → Na⁺ + e–

Answer

Br₂ + 2e – → 2Br –

Question 18

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

Question 19

19. Decrease in oxidation number is called

Answer

All of these

Question 20

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

Answer

0.1 N NaCl

Question 21

21. Alkaline battery has a voltage of

Question 22

22. Specific conductivity of a solution

Answer

Decreases with dilution

Answer

Remains unchanged with dilution

Answer

Increases with dilution

Answer

Depends on mass of electrolyte

Question 23

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

Answer

Refractive index

Answer

Surface tension

Answer

Osmotic pressure

Question 24

24. 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

None of these

Answer

One gm. atomic weight

Question 25

25. Which of the following statements is FALSE?

Answer

Reduction occurs at cathode

Answer

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

Answer

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

Answer

All electrochemical reactions involve the transfer of electrons

Question 26

26. Best way to prevent rusting iron is by

Answer

Putting it in saline water

Answer

None of these

Answer

Making iron cathode

Answer

Both of these

Question 27

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

Answer

Electrolytic cell

Answer

Galvanic cell

Answer

Daniel cell

Question 28

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

Answer

None of these

Answer

Distillation

Answer

Fractional distillation

Answer

Vacuum distillation

Question 29

29. 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 30

30. Molton NaCl conducts electricity due to the presence of

Answer

Free electrons

Answer

Atoms of Na and Cl.

Answer

Free molecules

Question 31

31. Mole fraction of pure water is

Answer

None of these

Answer

Exactly equal to one

Answer

Slightly greater than one

Answer

Slightly less than one

Question 32

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

Answer

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

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

Question 33

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 34

34. Cathode provides electrons to

Answer

Does not provide any electron

Answer

Neutral atom

Question 35

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

Question 36

36. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 37

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

Answer

Slightly more than 1 atom

Answer

760 mm of Hg

Question 38

38. Density of H₂SO₄ in lead accumulator is

Question 39

39. Which of the substances Na, Hg, S Pt and graphite can be used as electrodes in electrolytic cells having aqueous solution?

Answer

Na, Pt and graphite

Answer

Pt and graphite only

Answer

Na and S only

Question 40

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

Answer

None of these

Question 41

41. Units of molarity are

Answer

None of these

Question 42

42. Stronger the oxidizing agent, greater is the

Answer

Redox potential

Answer

Oxidation potential

Answer

e.m.f of cell

Answer

Reduction potential

Question 43

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

Answer

750 mm of Hg

Answer

760 mm of Hg

Answer

780 mm of Hg

Answer

800 mm of Hg

Question 44

44. Oxidation in a chemical reaction involves

Answer

Decrease in oxidation number

Answer

Both are possible

Answer

Increase in oxidation number

Answer

Increase in oxidation number of all the elements on reactant side

Question 45

45. Potential of Zn is called

Answer

It has not potential

Question 46

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

Question 47

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

Question 48

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

Question 49

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

Answer

Decreases slowly

Answer

Drops to zero

Answer

Decrease rapidly

Answer

Does not change

Question 50

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

Question 51

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

Answer

Arrhenius law

Answer

Henry’s law

Answer

Ostwald’s law

Answer

Raoult’s law

Question 52

52. 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 53

53. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 54

54. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 55

55. In the conversion of Br2 to BrO₃¯¹ the oxidation state of bromine changes from

Question 56

56. 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 57

57. When the solute is present in trace quantities the following expression is used?

Answer

Gram per million

Answer

Microgram percent

Answer

Milligram percent

Answer

Parts per million

Question 58

58. The degree of dissociation of weak electrolyte increases as

Answer

Dilution increases

Answer

Dilution decreases

Answer

Pressure increases

Question 59

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

Question 60

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

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

None of these

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

Question 61

61. 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 62

62. The specific conductance of 0.1 M NaCl solution is 1.06 x 10¯² ohm¯¹mol¯¹. Its molar conductance in ohm¯¹ cm² mol¯¹ is

Answer

1.06 x 10³

Answer

1.06 x 10⁴

Answer

1.06 x 10²

Question 63

63. The art of electroplating was given by

Answer

Thomas Gradam

Question 64

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

Answer 139

The entropy of mixing is zero

Answer 140

The enthalpy of mixing is zero

Answer 141

The free energy of mixing is zero

Answer 142

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

Answer 143

Gold has higher reduction potential then iron

Answer 144

Gold is denser

Answer 145

Gold has lower reduction potential then iron

Answer 146

Iron rusts

Answer 147

Neither oxidation and reduction

Answer 148

Both oxidation and reduction

Answer 149

Neutralization

Answer 150

Spontaneous reaction

Answer 151

Non-spontaneous reaction

Answer 152

It has a very high cryoscopic constant

Answer 153

It is volatile

Answer 154

It is solvent for organic substances

Answer 155

It is readily available

Answer 156

Standard reduction potential

Answer 157

Standard oxidation potential

Answer 158

Cell voltage

Answer 159

Ionization potential

Answer 160

H₄P₃O₇

Answer 161

B.P of water increase

Answer 162

B.P of water remain constant

Answer 163

Any possibility

Answer 164

B.P of water decrease

Answer 165

0.1 M Glucose

Answer 166

0.1 M Sucrose

Answer 167

0.1 M BaCl₂

Answer 168

0.1 M NaCl

Answer 169

1.25g/Cm³

Answer 170

120 g Cm³

Answer 171

1.2 g/Cm³

Answer 172

1.15 g/Cm³

Answer 173

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

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

Boiling point of pure water decreases by the addition of ethanol

Answer 177

Neither a nor b

Answer 178

Dilute solution which behave as nearly ideal solution

Answer 179

Both a and b

Answer 180

Concentration solutions behave as nearly non – ideal solutions

Answer 181

Hg₂Cl₂

Answer 182

Is readily decomposed

Answer 183

Has low boiling point

Answer 184

Is almost unionized

Answer 185

Is neutral

Answer 186

None of these

Answer 187

Slightly less than the total volume of the components

Answer 188

Equal to the total volume of the components

Answer 189

Slightly more than the total volume of the components

Answer 190

Gives ions only when dissolved in water

Answer 191

Forms complex ions in solution

Answer 192

Possesses ions even in solid state

Answer 193

Gives ions only when electricity is passed

Answer 194

Sufficient date not given

Answer 195

None of these

Answer 196

Both Na⁺ and CI¯

Answer 197

63.5 g of Cu

Answer 198

100 g of Cu

Answer 199

96500 g of CU

Answer 200

31.75 g of Cu

Answer 201

Electrical energy is converted into heat

Answer 202

Electrical energy is converted into chemical energy

Answer 203

Chemical energy is converted into heat

Answer 204

Chemical energy is converted into electricity

Answer 205

22400 cm³

Answer 206

Degree of solubilization of solute

Answer 207

The extent of dissolution of solute

Answer 208

The extent of dissociation of solute

Answer 209

The degree of decomposition of solution

Answer 210

O₂, SO₂

Answer 211

None of these

Answer 212

Remove adsorbed oxygen from electrode surfaces

Answer 213

Create potential difference between two electrodes

Answer 214

Generate heat

Answer 215

Produce high purity water

Answer 216

Standard electrode potential

Answer 217

Electric change

Answer 218

Electroplating

Answer 219

Ionization potential

Answer 220

Rust removal

Answer 221

Manufacture of bleach

Answer 222

Making leather

Answer 223

Electroplating

Answer 224

Nitric acid

Answer 225

Sulphuric acid

Answer 226

Phosphorus acid

Answer 227

Boric acid

Answer 228

Electrical energy

Answer 229

Sound energy

Answer 230

Magnetic energy

Answer 231

Heat energy

Answer 232

Diffusion rate of the solute

Answer 233

Flow of solvent from a concentrated to a dilute solution

Answer 234

Ionic concentration

Answer 235

Elevation in boiling point

Answer 236

Oxidation-reduction

Answer 237

Depends on the nature of the coupled electrode

Answer 238

Molten NaCl

Answer 239

Dilute solution of glucose

Answer 240

Pure distilled water

Answer 241

Chloroform

Answer 242

128 S cm² mol¯¹

Answer 243

176 S cm² mol¯¹

Answer 244

302 S cm² mol¯¹

Answer 245

278 S cm² mol¯¹

Answer 246

Sublimation point

Answer 247

Boiling point

Answer 248

Melting point

Answer 249

Inversion point

Answer 250

Lesser positive value of standard reduction potential

Answer 251

Greater negative value of standard reduction potential

Answer 252

Greater positive value of standard reduction potential

Answer 253

None of these

Answer 254

By addition of fresh solution

Answer 255

By heating it

Answer 256

By removal of solution

Answer 257

By replacing external circuit with external source of electricity

Answer 258

12157.48 sec

Answer 259

More than that of H₂O

Answer 260

Equal to that of ethanol

Answer 261

Equal to that of water

Answer 262

Less than that of water

Answer 263

Ohm cm¯¹

Answer 264

Ohm¯¹ cm

Answer 265

Ohm¯¹ cm¯¹

Answer 266

Ohm cm¯²

Answer 267

1.25 cm¯³

Answer 268

1.15 cm¯³

Answer 269

2.15 cm¯³

Answer 270

1.81 cm¯³

Answer 271

Temperature

Answer 272

All of these

Answer 273

Pressure of the gas

Answer 274

Nature of the gas

Answer 275

A voltaic cell

Answer 276

A galvanic cell

Answer 277

An electrolytic cell

Answer 278

A chemical cell

Answer 279

Photo electrolysis

Answer 280

Electrolysis

Answer 281

Cathodic protection

Answer 282

Galvanization

Answer 283

Loses electrons

Answer 284

pH is changed

Answer 285

Acts as a catalyst

Answer 286

Gains electrons

Answer 287

Electrolytic cell

Answer 288

Daniel cell

Answer 289

Non rechargeable

Answer 290

Rechargeable

Answer 291

At cathode

Answer 292

None of these

Answer 293

Both A and B

Answer 294

Hg₂Cl₂

Answer 295

1.0 x 10¹⁰

Answer 296

2.0 x 10¹¹

Answer 297

1.0 x 10²

Answer 298

4.0 x 10¹²

Answer 299

Electrons are released at anode

Answer 300

Cathode is regarded as negative electrode

Answer 301

Chemical energy is converted into electrical energy

Answer 302

Salt bridge maintains the electrical neutrality of the solution

Answer 303

Salt Bridge

Answer 304

No connection exists

Answer 305

Electric circuit

Answer 306

Raoult’s law

Answer 307

Distribution law

Answer 308

Henry’s law

Answer 309

Ostwald’s dilution law

Answer 310

Electron transfer

Answer 311

Proton transfer

Answer 312

Ion combination reaction

Answer 313

A reaction in a solution

Answer 314

From cathode to anode inside the cell

Answer 315

From cathode to anode in outer circuit

Answer 316

From anode to cathode inside the cell

Answer 317

From anode to cathode in an outer circuit

Answer 318

Not particular

Answer 319

Na₂SO₄

Answer 320

CH₃ CooNH₄

Answer 321

None of these

Answer 322

Naphthalene

Answer 323

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

Answer 324

Hg is more inert than Pt

Answer 325

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

Answer 326

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

Answer 327

Spontaneous redox reactions

Answer 328

Spontaneous acid–base reactions

Answer 329

None of these

Answer 330

Non-spontaneous redox reactions

Answer 331

Weak acid and its salt of weak base

Answer 332

A strong acid and its salt of a strong base

Answer 333

Strong acid and its salt of weak base

Answer 334

Weak acid and its salt of strong base

Answer 335

In metals the ions are free to more

Answer 336

They are mobile electrons in the metallic structure

Answer 337

Metals are decomposed by current

Answer 338

Metals have high resistance

Answer 339

Ca(NO₃)₂

Answer 340

None of these

Answer 341

Heat energy

Answer 342

Electrical energy

Answer 343

Chemical energy

Answer 344

Electrolytic cell

Answer 345

Galvanic cell

Answer 346

Reduction potentials are negative

Answer 347

Very high negative values reduction potential

Answer 348

Very high positive value of reduction potential

Answer 349

Very low ionization potential values

Answer 350

Supersaturated

Answer 351

Unsaturated

Answer 352

∆ G = +ve, ∆ E = 0

Answer 353

∆ G = -ve

Answer 354

∆ G = -ve, ∆ E = 0

Answer 355

∆ G = 0, ∆E = 0

Answer 356

Molality of the solution

Answer 357

Mole fraction of the solution

Answer 358

Molarity of the solution

Answer 359

Molarity of the solvent

Answer 360

1 – 2 α

Answer 361

Anode to cathode through the solution

Answer 362

Anode to cathode through the external circuit

Answer 363

Cathode to anode through the external circuit

Answer 364

Cathode to anode through the solution

Answer 365

H+ and OH-

Answer 366

Both A and B

Answer 367

None of these

Answer 368

Electrorefining

Answer 369

Electroplating

Total Questions:	192
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Total Marks:	192
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