Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. The Vant Hoff factor (i) accounts for

Answer

The degree of decomposition of solution

Answer

The extent of dissociation of solute

Answer

The extent of dissolution of solute

Answer

Degree of solubilization of solute

Question 2

2. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 3

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

Question 4

4. Best way to prevent rusting iron is by

Answer

Putting it in saline water

Answer

Both of these

Answer

Making iron cathode

Answer

None of these

Question 5

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

Answer

Galvanization

Answer

Cathodic protection

Answer

Electrolysis

Answer

Photo electrolysis

Question 6

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

Answer

Weak acid and its salt of strong base

Answer

Strong acid and its salt of weak base

Answer

A strong acid and its salt of a strong base

Answer

Weak acid and its salt of weak base

Question 7

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

Question 8

8. Molarity of water is

Question 9

9. 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 BaCl₂

Answer

0.1 M Sucrose

Question 10

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

Question 11

11. Calculate the amount of charge flowing in 2 minute in a wire of resistance 10 Ω when a potential difference of 20 V is applied

Question 12

12. 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 13

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

Question 14

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

Question 15

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

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

Li is smaller in size as compared to Cu

Answer

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

Question 16

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

Answer

Not particular

Question 17

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

Question 18

18. Which of the following statements is FALSE?

Answer

Reduction occurs at cathode

Answer

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

Answer

All electrochemical reactions involve the transfer of electrons

Answer

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

Question 19

19. Molton NaCl conducts electricity due to the presence of

Answer

Free molecules

Answer

Free electrons

Answer

Atoms of Na and Cl.

Question 20

20. The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

Answer

Boiling point

Answer

Inversion point

Answer

Melting point

Answer

Sublimation point

Question 21

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

Question 22

22. Metals usually conduct electricity because

Answer

Metals have high resistance

Answer

In metals the ions are free to more

Answer

Metals are decomposed by current

Answer

They are mobile electrons in the metallic structure

Question 23

23. Corrosion reactions are

Answer

None of these

Answer

Spontaneous acid–base reactions

Answer

Spontaneous redox reactions

Answer

Non-spontaneous redox reactions

Question 24

24. 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 25

25. 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 26

26. The degree of dissociation of weak electrolyte increases as

Answer

Pressure increases

Answer

Dilution increases

Answer

Dilution decreases

Question 27

27. If the standard electrode potential of CU²⁺/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu²⁺? (T = 298 K)

Question 28

28. Decrease in oxidation number is called

Answer

All of these

Question 29

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

Answer

Acts as a catalyst

Answer

pH is changed

Answer

Loses electrons

Answer

Gains electrons

Question 30

30. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 31

31. If liquids A and B form an ideal solution

Answer

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

Answer

The enthalpy of mixing is zero

Answer

The entropy of mixing is zero

Answer

The free energy of mixing is zero

Question 32

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

Answer

Remove adsorbed oxygen from electrode surfaces

Answer

Create potential difference between two electrodes

Answer

Produce high purity water

Answer

Generate heat

Question 33

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

Answer

780 mm of Hg

Answer

750 mm of Hg

Answer

760 mm of Hg

Answer

800 mm of Hg

Question 34

34. In alkaline battery the anode is made up of

Question 35

35. 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 36

36. 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 37

37. 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 water decreases by the addition of nitric acid

Answer

Boiling point of pure water decreases by the addition of ethanol

Answer

Vapour pressure of pure benzene decreases by the addition of naphthalene

Question 38

38. 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 39

39. The art of electroplating was given by

Answer

Thomas Gradam

Question 40

40. Colligative properties are the properties of

Answer

Dilute solution which behave as nearly ideal solution

Answer

Both a and b

Answer

Neither a nor b

Answer

Concentration solutions behave as nearly non – ideal solutions

Question 41

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

Answer

Flow of solvent from a concentrated to a dilute solution

Answer

Diffusion rate of the solute

Answer

Ionic concentration

Answer

Elevation in boiling point

Question 42

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

Answer

176 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Answer

278 S cm² mol¯¹

Answer

128 S cm² mol¯¹

Question 43

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 44

44. 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 45

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

Question 46

46. 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 47

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

Question 48

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

Answer

Gold has lower reduction potential then iron

Answer

Iron rusts

Answer

Gold has higher reduction potential then iron

Answer

Gold is denser

Question 49

49. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 50

50. In a Galvanic cell

Answer

Chemical energy is converted into electricity

Answer

Chemical energy is converted into heat

Answer

Electrical energy is converted into chemical energy

Answer

Electrical energy is converted into heat

Question 51

51. Secondary cell is

Answer

Rechargeable

Answer

Daniel cell

Answer

Non rechargeable

Answer

Electrolytic cell

Question 52

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

Question 53

53. 50 mL of 10 N H₂SO₄. 25 mL of 12 N HCl and 40 mL of 5N HNO₃ are mixed and the volume of the mixture is made 1000 mL by adding water. The normality of resulting solution will be

Question 54

54. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 55

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

Answer

Electrolytic cell

Answer

Daniel cell

Answer

Galvanic cell

Question 56

56. 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 57

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

Answer

Electrolytic cell

Answer

Galvanic cell

Question 58

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

Answer

None of these

Answer

Electroplating

Answer

Both A and B

Answer

Electrorefining

Question 59

59. An aqueous solution of ethanol in water has vapour pressure

Answer

Less than that of water

Answer

Equal to that of water

Answer

More than that of H₂O

Answer

Equal to that of ethanol

Question 60

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

Answer

Magnetic energy

Answer

Sound energy

Answer

Electrical energy

Answer

Heat energy

Question 61

61. Which of these is not an application of electrolysis?

Answer

Making leather

Answer

Rust removal

Answer

Manufacture of bleach

Answer

Electroplating

Question 62

62. Azeotropic mixture of HCl and water has

Question 63

63. A redox reaction involves

Answer

Electron transfer

Answer

A reaction in a solution

Answer

Proton transfer

Answer

Ion combination reaction

Question 64

64. In electrolytic cell, electricity in carried out by

Answer

Spontaneous reaction

Answer

Non-spontaneous reaction

Answer

Neutralization

Answer 139

Depends on mass of electrolyte

Answer 140

Decreases with dilution

Answer 141

Remains unchanged with dilution

Answer 142

Increases with dilution

Answer 143

H+ and OH-

Answer 144

Sulphuric acid

Answer 145

Boric acid

Answer 146

Phosphorus acid

Answer 147

Nitric acid

Answer 148

Greater positive value of standard reduction potential

Answer 149

Lesser positive value of standard reduction potential

Answer 150

None of these

Answer 151

Greater negative value of standard reduction potential

Answer 152

Hypertonic

Answer 153

Naphthalene

Answer 154

None of these

Answer 155

Altered reaction in presence of H₂O

Answer 156

Interaction

Answer 157

Electrochemical phenomenon

Answer 158

Union between two light metals and a heavy metal

Answer 159

No connection exists

Answer 160

Electric circuit

Answer 161

Salt Bridge

Answer 162

Na → Na⁺ + e–

Answer 163

2Br– → Br₂ + 2e –

Answer 164

Na⁺ + e– → Na

Answer 165

Br₂ + 2e – → 2Br –

Answer 166

Does not provide any electron

Answer 167

Neutral atom

Answer 168

Drops to zero

Answer 169

Decreases slowly

Answer 170

Decrease rapidly

Answer 171

Does not change

Answer 172

Distribution law

Answer 173

Raoult’s law

Answer 174

Henry’s law

Answer 175

Ostwald’s dilution law

Answer 176

Increases rapidly

Answer 177

Does not change

Answer 178

Increases gradually

Answer 179

Drops to zero

Answer 180

0.66 cm¯¹

Answer 181

0.918 cm¯¹

Answer 182

1.12 cm¯¹

Answer 183

0.142 cm¯¹

Answer 184

2.0 x 10¹¹

Answer 185

1.0 x 10²

Answer 186

4.0 x 10¹²

Answer 187

1.0 x 10¹⁰

Answer 188

It has not potential

Answer 189

S² m² mol¯²

Answer 190

S² m² mol

Answer 191

S m mol¯¹

Answer 192

S m² mol¯¹

Answer 193

Possesses ions even in solid state

Answer 194

Gives ions only when dissolved in water

Answer 195

Forms complex ions in solution

Answer 196

Gives ions only when electricity is passed

Answer 197

A chemical cell

Answer 198

A galvanic cell

Answer 199

A voltaic cell

Answer 200

An electrolytic cell

Answer 201

One gm. Equivalent weight

Answer 202

None of these

Answer 203

One gm. atomic weight

Answer 204

Electrochemical equivalent

Answer 205

Chemical energy

Answer 206

None of these

Answer 207

Electrical energy

Answer 208

Heat energy

Answer 209

[Pt(NH₃)₄Cl₄]

Answer 210

[Pt(NH₃)₄Cl₃]Cl

Answer 211

[Pt(NH₃)₄Cl₂]Cl₂

Answer 212

[Pt(NH₃)₄Cl]Cl₃

Answer 213

Raoult’s law

Answer 214

Arrhenius law

Answer 215

Henry’s law

Answer 216

Ostwald’s law

Answer 217

Exactly equal to one

Answer 218

Slightly less than one

Answer 219

None of these

Answer 220

Slightly greater than one

Answer 221

Depends on the nature of the coupled electrode

Answer 222

Oxidation-reduction

Answer 223

Does not change on dilution

Answer 224

Increases on dilution slightly

Answer 225

Decreases on dilution

Answer 226

Depends on density of electrolyte itself.

Answer 227

It has a very high cryoscopic constant

Answer 228

It is readily available

Answer 229

It is solvent for organic substances

Answer 230

It is volatile

Answer 231

Increase in oxidation number of all the elements on reactant side

Answer 232

Increase in oxidation number

Answer 233

Decrease in oxidation number

Answer 234

Both are possible

Answer 235

Oxidation number neither increases nor decreases

Answer 236

Decrease in oxidation number of element

Answer 237

Increase in oxidation number of element

Answer 238

Increase in oxidation number of the elements in reactants

Answer 239

O₂, SO₂

Answer 240

None of these

Answer 241

Electrons flow cathode to anode within the electrolytic solution

Answer 242

None of these

Answer 243

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

Answer 244

Electrons flow from cathode to anode through the external battery

Answer 245

H₄P₃O₇

Answer 246

Any possibility

Answer 247

B.P of water remain constant

Answer 248

B.P of water decrease

Answer 249

B.P of water increase

Answer 250

5.58g NaCl/100m

Answer 251

10.0g NaCl/100ml

Answer 252

58.5g NaCl/100ml

Answer 253

20g NaCl/100ml

Answer 254

0.1 N NaCl

Answer 255

1.25 cm¯³

Answer 256

1.81 cm¯³

Answer 257

2.15 cm¯³

Answer 258

1.15 cm¯³

Answer 259

Oxidation potential

Answer 260

Redox potential

Answer 261

e.m.f of cell

Answer 262

Reduction potential

Answer 263

Hydrolyzed

Answer 264

Precipitated

Answer 265

Very high positive value of reduction potential

Answer 266

Very low ionization potential values

Answer 267

Reduction potentials are negative

Answer 268

Very high negative values reduction potential

Answer 269

Pt and graphite only

Answer 270

Na and S only

Answer 271

Na, Pt and graphite

Answer 272

Equal to the total volume of the components

Answer 273

Slightly less than the total volume of the components

Answer 274

None of these

Answer 275

Slightly more than the total volume of the components

Answer 276

Mole fraction of the solution

Answer 277

Molality of the solution

Answer 278

Molarity of the solution

Answer 279

Molarity of the solvent

Answer 280

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

Answer 281

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

Answer 282

Hg is more inert than Pt

Answer 283

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

Answer 284

Both oxidation and reduction

Answer 285

Neither oxidation and reduction

Answer 286

Cathode to anode through the solution

Answer 287

Anode to cathode through the solution

Answer 288

Anode to cathode through the external circuit

Answer 289

Cathode to anode through the external circuit

Answer 290

Surface tension

Answer 291

Refractive index

Answer 292

Osmotic pressure

Answer 293

Is hydrolysed

Answer 294

Gains electrons

Answer 295

Loses electrons

Answer 296

Is oxidized

Answer 297

CH₃ CooNH₄

Answer 298

Na₂SO₄

Answer 299

96500 g of CU

Answer 300

100 g of Cu

Answer 301

63.5 g of Cu

Answer 302

31.75 g of Cu

Answer 303

Neutralization

Answer 304

Electrons are released at anode

Answer 305

Cathode is regarded as negative electrode

Answer 306

Salt bridge maintains the electrical neutrality of the solution

Answer 307

Chemical energy is converted into electrical energy

Answer 308

All of these

Answer 309

Nature of the gas

Answer 310

Pressure of the gas

Answer 311

Temperature

Answer 312

Microgram percent

Answer 313

Parts per million

Answer 314

Milligram percent

Answer 315

Gram per million

Answer 316

Hg₂Cl₂

Answer 317

By heating it

Answer 318

By addition of fresh solution

Answer 319

By removal of solution

Answer 320

By replacing external circuit with external source of electricity

Answer 321

Supersaturated

Answer 322

Unsaturated

Answer 323

Standard electrode potential

Answer 324

Electric change

Answer 325

Ionization potential

Answer 326

Electroplating

Answer 327

Hg₂Cl₂

Answer 328

Both A and B

Answer 329

At cathode

Answer 330

None of these

Answer 331

Ohm¯¹ cm

Answer 332

Ohm cm¯²

Answer 333

Ohm cm¯¹

Answer 334

Ohm¯¹ cm¯¹

Answer 335

None of these

Answer 336

None of these

Answer 337

Distillation

Answer 338

Fractional distillation

Answer 339

Vacuum distillation

Answer 340

None of these

Answer 341

Both Na⁺ and CI¯

Answer 342

Ionization potential

Answer 343

Standard reduction potential

Answer 344

Standard oxidation potential

Answer 345

Cell voltage

Answer 346

Solvent particles

Answer 347

None of these

Answer 348

760 mm of Hg

Answer 349

Slightly more than 1 atom

Answer 350

1.15 g/Cm³

Answer 351

1.2 g/Cm³

Answer 352

1.25g/Cm³

Answer 353

120 g Cm³

Answer 354

1.06 x 10²

Answer 355

1.06 x 10³

Answer 356

1.06 x 10⁴

Answer 357

Has low boiling point

Answer 358

Is almost unionized

Answer 359

Is neutral

Answer 360

Is readily decomposed

Answer 361

Dilute solution of glucose

Answer 362

Chloroform

Answer 363

Pure distilled water

Answer 364

Molten NaCl

Answer 365

∆ G = -ve

Answer 366

∆ G = -ve, ∆ E = 0

Answer 367

∆ G = +ve, ∆ E = 0

Answer 368

∆ G = 0, ∆E = 0

Answer 369

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Total Questions:	192
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Total Marks:	192
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