Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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 2

2. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 3

3. Strong reducing agents have

Answer

Greater positive value of standard reduction potential

Answer

None of these

Answer

Lesser positive value of standard reduction potential

Answer

Greater negative value of standard reduction potential

Question 4

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

Question 5

5. Which has maximum oxidation number

Question 6

6. What are the ions present in water?

Answer

H+ and OH-

Question 7

7. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 8

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

Answer

Increases rapidly

Answer

Does not change

Answer

Drops to zero

Answer

Increases gradually

Question 9

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

Answer

Diffusion rate of the solute

Answer

Flow of solvent from a concentrated to a dilute solution

Answer

Elevation in boiling point

Answer

Ionic concentration

Question 10

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

Answer

Li is smaller in size as compared to Cu

Answer

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

Answer

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

Answer

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

Question 11

11. 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 12

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

Question 13

13. Choose the best reducing agent among the following

Question 14

14. 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 15

15. During a redox reaction, an oxidizing agent

Answer

Loses electrons

Answer

Gains electrons

Answer

Is oxidized

Answer

Is hydrolysed

Question 16

16. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 17

17. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 18

18. Molton NaCl conducts electricity due to the presence of

Answer

Free electrons

Answer

Free molecules

Answer

Atoms of Na and Cl.

Question 19

19. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 20

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

Answer

Rust removal

Answer

Making leather

Answer

Manufacture of bleach

Answer

Electroplating

Question 21

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

Question 22

22. 96500 C of electricity liberates from CuSO₄ solution

Answer

31.75 g of Cu

Answer

100 g of Cu

Answer

96500 g of CU

Answer

63.5 g of Cu

Question 23

23. 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 24

24. Which one of the following substance when dissolved in water give acidic solution

Answer

Na₂SO₄

Answer

CH₃ CooNH₄

Question 25

25. 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 26

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

Answer

Galvanic cell

Answer

Electrolytic cell

Question 27

27. Half cells are interconnected through

Answer

Salt Bridge

Answer

No connection exists

Answer

Electric circuit

Question 28

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 29

29. 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 10²

Answer

1.06 x 10³

Answer

1.06 x 10⁴

Question 30

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

Question 31

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

Answer

A strong acid and its salt of a strong base

Answer

Weak acid and its salt of weak base

Answer

Strong acid and its salt of weak base

Answer

Weak acid and its salt of strong base

Question 32

32. Cathode provides electrons to

Answer

Does not provide any electron

Answer

Neutral atom

Question 33

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

Question 34

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

Answer

Hydrolyzed

Answer

Precipitated

Question 35

35. The best reducing agent is

Question 36

36. 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 37

37. Salt bridge transfers

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. 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

S m mol¯¹

Answer

S² m² mol¯²

Answer

S m² mol¯¹

Answer

S² m² mol

Question 40

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

Question 41

41. Potential of Zn is called

Answer

It has not potential

Question 42

42. The molarity of the solution containing x grams (NH₄)SO₄ in 500 cm³ of the solution is 0.6. What is x

Question 43

43. Electrode potential of Zn is

Answer

Depends on the nature of the coupled electrode

Answer

Oxidation-reduction

Question 44

44. Pure water does not conduct electricity because it

Answer

Is almost unionized

Answer

Is readily decomposed

Answer

Is neutral

Answer

Has low boiling point

Question 45

45. 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 46

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

Answer

Ostwald’s dilution law

Answer

Henry’s law

Answer

Raoult’s law

Answer

Distribution law

Question 47

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

Answer

Pt and graphite only

Answer

Na and S only

Answer

Na, Pt and graphite

Question 48

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

Answer

0.1 N NaCl

Question 49

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

Answer

None of these

Answer

Both Na⁺ and CI¯

Question 50

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

Answer

Gold has higher reduction potential then iron

Answer

Gold has lower reduction potential then iron

Answer

Iron rusts

Answer

Gold is denser

Question 51

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

Answer

58.5g NaCl/100ml

Answer

20g NaCl/100ml

Answer

5.58g NaCl/100m

Answer

10.0g NaCl/100ml

Question 52

52. 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 53

53. Voltaic cell can be recharged by

Answer

By replacing external circuit with external source of electricity

Answer

By addition of fresh solution

Answer

By removal of solution

Answer

By heating it

Question 54

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

Answer

Both oxidation and reduction

Answer

Neither oxidation and reduction

Question 55

55. Stronger the oxidizing agent, greater is the

Answer

Reduction potential

Answer

e.m.f of cell

Answer

Oxidation potential

Answer

Redox potential

Question 56

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

Answer

Produce high purity water

Answer

Remove adsorbed oxygen from electrode surfaces

Answer

Generate heat

Answer

Create potential difference between two electrodes

Question 57

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

Question 58

58. 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 59

59. In an electrolytic cell current flows

Answer

From anode to cathode inside the cell

Answer

From cathode to anode in outer circuit

Answer

From anode to cathode in an outer circuit

Answer

From cathode to anode inside the cell

Question 60

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

Answer

Supersaturated

Answer

Unsaturated

Question 61

61. Specific conductivity of a solution

Answer

Depends on mass of electrolyte

Answer

Remains unchanged with dilution

Answer

Increases with dilution

Answer

Decreases with dilution

Question 62

62. Standard reduction electrode potential of three metals A, B and C are respectively + 0.05 V, - 3.0 and -1.2V. The reducing power of

Question 63

63. 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 64

64. 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

4.0 x 10¹²

Answer

1.0 x 10²

Answer 116

None of these

Answer 117

Electrolytic cell

Answer 118

Non rechargeable

Answer 119

Rechargeable

Answer 120

Daniel cell

Answer 121

B.P of water increase

Answer 122

B.P of water remain constant

Answer 123

B.P of water decrease

Answer 124

Any possibility

Answer 125

Daniel cell

Answer 126

Electrolytic cell

Answer 127

Galvanic cell

Answer 128

Hg₂Cl₂

Answer 129

1 – 2 α

Answer 130

None of these

Answer 131

Metals have high resistance

Answer 132

They are mobile electrons in the metallic structure

Answer 133

In metals the ions are free to more

Answer 134

Metals are decomposed by current

Answer 135

Mole fraction of the solution

Answer 136

Molarity of the solution

Answer 137

Molarity of the solvent

Answer 138

Molality of the solution

Answer 139

Both of these

Answer 140

Making iron cathode

Answer 141

None of these

Answer 142

Putting it in saline water

Answer 143

More than that of H₂O

Answer 144

Equal to that of water

Answer 145

Less than that of water

Answer 146

Equal to that of ethanol

Answer 147

Increase in oxidation number

Answer 148

Both are possible

Answer 149

Decrease in oxidation number

Answer 150

Increase in oxidation number of all the elements on reactant side

Answer 151

Electrons are released at anode

Answer 152

Chemical energy is converted into electrical energy

Answer 153

Salt bridge maintains the electrical neutrality of the solution

Answer 154

Cathode is regarded as negative electrode

Answer 155

Pressure increases

Answer 156

Dilution decreases

Answer 157

Dilution increases

Answer 158

Electrical energy

Answer 159

Sound energy

Answer 160

Heat energy

Answer 161

Magnetic energy

Answer 162

Osmotic pressure

Answer 163

Refractive index

Answer 164

Surface tension

Answer 165

Ionization potential

Answer 166

Cell voltage

Answer 167

Standard oxidation potential

Answer 168

Standard reduction potential

Answer 169

0.1 M NaCl

Answer 170

0.1 M Sucrose

Answer 171

0.1 M Glucose

Answer 172

0.1 M BaCl₂

Answer 173

12157.48 sec

Answer 174

Sufficient date not given

Answer 175

278 S cm² mol¯¹

Answer 176

128 S cm² mol¯¹

Answer 177

302 S cm² mol¯¹

Answer 178

176 S cm² mol¯¹

Answer 179

Temperature

Answer 180

All of these

Answer 181

Pressure of the gas

Answer 182

Nature of the gas

Answer 183

None of these

Answer 184

Equal to the total volume of the components

Answer 185

Slightly more than the total volume of the components

Answer 186

Slightly less than the total volume of the components

Answer 187

Ion combination reaction

Answer 188

A reaction in a solution

Answer 189

Proton transfer

Answer 190

Electron transfer

Answer 191

Electrons flow from cathode to anode through the external battery

Answer 192

None of these

Answer 193

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

Answer 194

Electrons flow cathode to anode within the electrolytic solution

Answer 195

Thomas Gradam

Answer 196

Chemical energy

Answer 197

Electrical energy

Answer 198

None of these

Answer 199

Heat energy

Answer 200

Dilute solution which behave as nearly ideal solution

Answer 201

Neither a nor b

Answer 202

Concentration solutions behave as nearly non – ideal solutions

Answer 203

Both a and b

Answer 204

Neutralization

Answer 205

Spontaneous reaction

Answer 206

Non-spontaneous reaction

Answer 207

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 208

Boiling point of pure benzene increases by the addition of toluene

Answer 209

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

Answer 210

Boiling point of pure water decreases by the addition of ethanol

Answer 211

Photo electrolysis

Answer 212

Electrolysis

Answer 213

Cathodic protection

Answer 214

Galvanization

Answer 215

Very high positive value of reduction potential

Answer 216

Very high negative values reduction potential

Answer 217

Very low ionization potential values

Answer 218

Reduction potentials are negative

Answer 219

Sum of reduction and oxidation potentials

Answer 220

∆ G = +ve, ∆ E = 0

Answer 221

∆ G = -ve, ∆ E = 0

Answer 222

∆ G = 0, ∆E = 0

Answer 223

∆ G = -ve

Answer 224

760 mm of Hg

Answer 225

Slightly more than 1 atom

Answer 226

Raoult’s law

Answer 227

Ostwald’s law

Answer 228

Henry’s law

Answer 229

Arrhenius law

Answer 230

Electroplating

Answer 231

Electrolysis

Answer 232

Conduction

Answer 233

Ca(NO₃)₂

Answer 234

Solvent particles

Answer 235

Cathode to anode through the external circuit

Answer 236

Anode to cathode through the solution

Answer 237

Anode to cathode through the external circuit

Answer 238

Cathode to anode through the solution

Answer 239

An electrolytic cell

Answer 240

A galvanic cell

Answer 241

A voltaic cell

Answer 242

A chemical cell

Answer 243

All of these

Answer 244

0.918 cm¯¹

Answer 245

0.66 cm¯¹

Answer 246

1.12 cm¯¹

Answer 247

0.142 cm¯¹

Answer 248

The degree of decomposition of solution

Answer 249

Degree of solubilization of solute

Answer 250

The extent of dissolution of solute

Answer 251

The extent of dissociation of solute

Answer 252

Gives ions only when electricity is passed

Answer 253

Forms complex ions in solution

Answer 254

Possesses ions even in solid state

Answer 255

Gives ions only when dissolved in water

Answer 256

Reduction occurs at cathode

Answer 257

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

Answer 258

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

Answer 259

All electrochemical reactions involve the transfer of electrons

Answer 260

None of these

Answer 261

O₂, SO₂

Answer 262

Ionization potential

Answer 263

Electric change

Answer 264

Electroplating

Answer 265

Standard electrode potential

Answer 266

Decrease in oxidation number of element

Answer 267

Increase in oxidation number of element

Answer 268

Increase in oxidation number of the elements in reactants

Answer 269

Oxidation number neither increases nor decreases

Answer 270

Electrochemical phenomenon

Answer 271

Interaction

Answer 272

Altered reaction in presence of H₂O

Answer 273

Union between two light metals and a heavy metal

Answer 274

Not particular

Answer 275

Neutralization

Answer 276

Naphthalene

Answer 277

[Pt(NH₃)₄Cl₂]Cl₂

Answer 278

[Pt(NH₃)₄Cl₄]

Answer 279

[Pt(NH₃)₄Cl]Cl₃

Answer 280

[Pt(NH₃)₄Cl₃]Cl

Answer 281

Does not change on dilution

Answer 282

Depends on density of electrolyte itself.

Answer 283

Decreases on dilution

Answer 284

Increases on dilution slightly

Answer 285

Parts per million

Answer 286

Milligram percent

Answer 287

Gram per million

Answer 288

Microgram percent

Answer 289

H₄P₃O₇

Answer 290

At cathode

Answer 291

Both A and B

Answer 292

None of these

Answer 293

Chemical energy is converted into heat

Answer 294

Electrical energy is converted into heat

Answer 295

Electrical energy is converted into chemical energy

Answer 296

Chemical energy is converted into electricity

Answer 297

Slightly less than one

Answer 298

Exactly equal to one

Answer 299

Slightly greater than one

Answer 300

None of these

Answer 301

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

Answer 302

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

Answer 303

Hg is more inert than Pt

Answer 304

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

Answer 305

2Br– → Br₂ + 2e –

Answer 306

Na⁺ + e– → Na

Answer 307

Na → Na⁺ + e–

Answer 308

Br₂ + 2e – → 2Br –

Answer 309

120 g Cm³

Answer 310

1.25g/Cm³

Answer 311

1.15 g/Cm³

Answer 312

1.2 g/Cm³

Answer 313

Boiling point

Answer 314

Sublimation point

Answer 315

Melting point

Answer 316

Inversion point

Answer 317

Ohm cm¯¹

Answer 318

Ohm¯¹ cm

Answer 319

Ohm cm¯²

Answer 320

Ohm¯¹ cm¯¹

Answer 321

None of these

Answer 322

Spontaneous acid–base reactions

Answer 323

Spontaneous redox reactions

Answer 324

Non-spontaneous redox reactions

Answer 325

Pure distilled water

Answer 326

Molten NaCl

Answer 327

Dilute solution of glucose

Answer 328

Chloroform

Answer 329

Loses electrons

Answer 330

pH is changed

Answer 331

Acts as a catalyst

Answer 332

Gains electrons

Answer 333

One gm. Equivalent weight

Answer 334

None of these

Answer 335

Electrochemical equivalent

Answer 336

One gm. atomic weight

Answer 337

It has a very high cryoscopic constant

Answer 338

It is readily available

Answer 339

It is volatile

Answer 340

It is solvent for organic substances

Answer 341

Electroplating

Answer 342

Both A and B

Answer 343

Electrorefining

Answer 344

None of these

Answer 345

The enthalpy of mixing is zero

Answer 346

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

Answer 347

The free energy of mixing is zero

Answer 348

The entropy of mixing is zero

Answer 349

None of these

Answer 350

None of these

Answer 351

Vacuum distillation

Answer 352

Distillation

Answer 353

Fractional distillation

Answer 354

Drops to zero

Answer 355

Decreases slowly

Answer 356

Does not change

Answer 357

Decrease rapidly

Answer 358

1.15 cm¯³

Answer 359

2.15 cm¯³

Answer 360

1.81 cm¯³

Answer 361

1.25 cm¯³

Answer 362

Boric acid

Answer 363

Phosphorus acid

Answer 364

Sulphuric acid

Answer 365

Nitric acid

Answer 366

750 mm of Hg

Answer 367

760 mm of Hg

Answer 368

780 mm of Hg

Answer 369

800 mm of Hg

Total Questions:	192
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Total Marks:	192
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