Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. The + 1 oxidation state of P is found in

Answer

H₄P₃O₇

Question 2

2. Secondary cell is

Answer

Rechargeable

Answer

Electrolytic cell

Answer

Daniel cell

Answer

Non rechargeable

Question 3

3. For spontaneity of a cell, which is correct?

Answer

∆ G = -ve, ∆ E = 0

Answer

∆ G = -ve

Answer

∆ G = +ve, ∆ E = 0

Answer

∆ G = 0, ∆E = 0

Question 4

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

Answer

Hg₂Cl₂

Question 5

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

Question 6

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

Question 7

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

Question 8

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

Answer

Electroplating

Answer

Electrolysis

Answer

Conduction

Question 9

9. Alkaline battery has a voltage of

Question 10

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

Question 11

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

Answer

0.1 M Sucrose

Answer

0.1 M NaCl

Answer

0.1 M BaCl₂

Answer

0.1 M Glucose

Question 12

12. 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 13

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

Answer

Gram per million

Answer

Parts per million

Answer

Milligram percent

Answer

Microgram percent

Question 14

14. Salt bridge transfers

Question 15

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

Question 16

16. The degree of dissociation of weak electrolyte increases as

Answer

Dilution decreases

Answer

Pressure increases

Answer

Dilution increases

Question 17

17. Maximum freezing point falls in

Answer

Naphthalene

Question 18

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

Answer

Equal to that of water

Answer

Less than that of water

Answer

Equal to that of ethanol

Answer

More than that of H₂O

Question 19

19. In alkaline battery the anode is made up of

Question 20

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

Question 21

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

Question 22

22. Metals usually conduct electricity because

Answer

Metals have high resistance

Answer

In metals the ions are free to more

Answer

They are mobile electrons in the metallic structure

Answer

Metals are decomposed by current

Question 23

23. 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 24

24. Which has maximum oxidation number

Question 25

25. 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 26

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

Answer

Does not change

Answer

Decrease rapidly

Answer

Drops to zero

Answer

Decreases slowly

Question 27

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

Question 28

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

Question 29

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

Question 30

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

Question 31

31. 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 32

32. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

Question 33

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

Question 34

34. 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

128 S cm² mol¯¹

Answer

278 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Question 35

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

Question 36

36. The best reducing agent is

Question 37

37. 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 38

38. Camphor is often used in molecular mass determination because

Answer

It is volatile

Answer

It is readily available

Answer

It has a very high cryoscopic constant

Answer

It is solvent for organic substances

Question 39

39. When common salt is dissolved in water

Answer

B.P of water decrease

Answer

Any possibility

Answer

B.P of water increase

Answer

B.P of water remain constant

Question 40

40. 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 high positive value of reduction potential

Answer

Very low ionization potential values

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Question 41

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

Answer

– 0.35 V

Answer

– 1.17 V

Question 42

42. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

Answer

Ionization potential

Answer

Electric change

Answer

Standard electrode potential

Answer

Electroplating

Question 43

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

Question 44

44. The art of electroplating was given by

Answer

Thomas Gradam

Question 45

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 46

46. Units of molarity are

Answer

None of these

Question 47

47. In alkaline battery anode is made up of

Question 48

48. The unit of specific conductivity is

Answer

Ohm cm¯²

Answer

Ohm cm¯¹

Answer

Ohm¯¹ cm¯¹

Answer

Ohm¯¹ cm

Question 49

49. 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 50

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

Answer

Na₂SO₄

Answer

CH₃ CooNH₄

Question 51

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

Answer

O₂, SO₂

Answer

None of these

Question 52

52. A device which converts electrical energy into chemical energy is called

Answer

A galvanic cell

Answer

An electrolytic cell

Answer

A voltaic cell

Answer

A chemical cell

Question 53

53. Azeotropic mixture of HCl and water has

Question 54

54. Which oxide has +2 oxidation number of oxygen?

Question 55

55. 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 56

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

Answer

Flow of solvent from a concentrated to a dilute solution

Answer

Ionic concentration

Answer

Elevation in boiling point

Answer

Diffusion rate of the solute

Question 57

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

Question 58

58. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 59

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

Question 60

60. Reaction takes place at anode is

Answer

Hydrolysis

Answer

Ionization

Question 61

61. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 62

62. Voltaic cell can be recharged by

Answer

By addition of fresh solution

Answer

By removal of solution

Answer

By replacing external circuit with external source of electricity

Answer

By heating it

Question 63

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

Answer

Create potential difference between two electrodes

Answer

Produce high purity water

Answer

Remove adsorbed oxygen from electrode surfaces

Answer

Generate heat

Question 64

64. Pick out the wrong statement. In electrochemical cell

Answer

Electrons are released at anode

Answer

Chemical energy is converted into electrical energy

Answer

Salt bridge maintains the electrical neutrality of the solution

Answer

Cathode is regarded as negative electrode

Answer 97

At cathode

Answer 98

None of these

Answer 99

Both A and B

Answer 100

Electrolytic cell

Answer 101

Daniel cell

Answer 102

Galvanic cell

Answer 103

Melting point

Answer 104

Boiling point

Answer 105

Sublimation point

Answer 106

Inversion point

Answer 107

Osmotic pressure

Answer 108

Surface tension

Answer 109

Refractive index

Answer 110

Slightly more than the total volume of the components

Answer 111

None of these

Answer 112

Slightly less than the total volume of the components

Answer 113

Equal to the total volume of the components

Answer 114

Nature of the gas

Answer 115

Temperature

Answer 116

Pressure of the gas

Answer 117

All of these

Answer 118

Gains electrons

Answer 119

Acts as a catalyst

Answer 120

Loses electrons

Answer 121

pH is changed

Answer 122

From anode to cathode in an outer circuit

Answer 123

From cathode to anode in outer circuit

Answer 124

From anode to cathode inside the cell

Answer 125

From cathode to anode inside the cell

Answer 126

Nitric acid

Answer 127

Sulphuric acid

Answer 128

Boric acid

Answer 129

Phosphorus acid

Answer 130

1.81 cm¯³

Answer 131

1.15 cm¯³

Answer 132

1.25 cm¯³

Answer 133

2.15 cm¯³

Answer 134

2Br– → Br₂ + 2e –

Answer 135

Br₂ + 2e – → 2Br –

Answer 136

Na⁺ + e– → Na

Answer 137

Na → Na⁺ + e–

Answer 138

Hg is more inert than Pt

Answer 139

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

Answer 140

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

Answer 141

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

Answer 142

Gold has lower reduction potential then iron

Answer 143

Gold has higher reduction potential then iron

Answer 144

Gold is denser

Answer 145

Iron rusts

Answer 146

H+ and OH-

Answer 147

Reduction potential

Answer 148

Redox potential

Answer 149

Oxidation potential

Answer 150

e.m.f of cell

Answer 151

Electroplating

Answer 152

Making leather

Answer 153

Manufacture of bleach

Answer 154

Rust removal

Answer 155

Anode to cathode through the external circuit

Answer 156

Cathode to anode through the external circuit

Answer 157

Anode to cathode through the solution

Answer 158

Cathode to anode through the solution

Answer 159

Does not provide any electron

Answer 160

Neutral atom

Answer 161

Loses electrons

Answer 162

Is oxidized

Answer 163

Gains electrons

Answer 164

Is hydrolysed

Answer 165

Spontaneous redox reactions

Answer 166

Non-spontaneous redox reactions

Answer 167

Spontaneous acid–base reactions

Answer 168

None of these

Answer 169

Galvanic cell

Answer 170

Electrolytic cell

Answer 171

760 mm of Hg

Answer 172

Slightly more than 1 atom

Answer 173

Greater positive value of standard reduction potential

Answer 174

None of these

Answer 175

Lesser positive value of standard reduction potential

Answer 176

Greater negative value of standard reduction potential

Answer 177

Both Na⁺ and CI¯

Answer 178

None of these

Answer 179

Salt Bridge

Answer 180

No connection exists

Answer 181

Electric circuit

Answer 182

Decreases on dilution

Answer 183

Increases on dilution slightly

Answer 184

Depends on density of electrolyte itself.

Answer 185

Does not change on dilution

Answer 186

100 g of Cu

Answer 187

31.75 g of Cu

Answer 188

96500 g of CU

Answer 189

63.5 g of Cu

Answer 190

2.0 x 10¹¹

Answer 191

1.0 x 10¹⁰

Answer 192

1.0 x 10²

Answer 193

4.0 x 10¹²

Answer 194

800 mm of Hg

Answer 195

750 mm of Hg

Answer 196

780 mm of Hg

Answer 197

760 mm of Hg

Answer 198

Cathodic protection

Answer 199

Galvanization

Answer 200

Electrolysis

Answer 201

Photo electrolysis

Answer 202

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

Answer 203

Li is smaller in size as compared to Cu

Answer 204

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

Answer 205

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

Answer 206

The free energy of mixing is zero

Answer 207

The enthalpy of mixing is zero

Answer 208

The entropy of mixing is zero

Answer 209

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

Answer 210

Supersaturated

Answer 211

Unsaturated

Answer 212

The degree of decomposition of solution

Answer 213

The extent of dissolution of solute

Answer 214

Degree of solubilization of solute

Answer 215

The extent of dissociation of solute

Answer 216

None of these

Answer 217

Making iron cathode

Answer 218

Putting it in saline water

Answer 219

Both of these

Answer 220

Molarity of the solvent

Answer 221

Molarity of the solution

Answer 222

Molality of the solution

Answer 223

Mole fraction of the solution

Answer 224

[Pt(NH₃)₄Cl]Cl₃

Answer 225

[Pt(NH₃)₄Cl₄]

Answer 226

[Pt(NH₃)₄Cl₂]Cl₂

Answer 227

[Pt(NH₃)₄Cl₃]Cl

Answer 228

Hg₂Cl₂

Answer 229

1.15 g/Cm³

Answer 230

1.2 g/Cm³

Answer 231

1.25g/Cm³

Answer 232

120 g Cm³

Answer 233

None of these

Answer 234

Hypertonic

Answer 235

Atoms of Na and Cl.

Answer 236

Free electrons

Answer 237

Free molecules

Answer 238

None of these

Answer 239

Electrons flow cathode to anode within the electrolytic solution

Answer 240

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

Answer 241

Electrons flow from cathode to anode through the external battery

Answer 242

A reaction in a solution

Answer 243

Proton transfer

Answer 244

Electron transfer

Answer 245

Ion combination reaction

Answer 246

S m² mol¯¹

Answer 247

S² m² mol¯²

Answer 248

S² m² mol

Answer 249

S m mol¯¹

Answer 250

Sufficient date not given

Answer 251

Increases gradually

Answer 252

Does not change

Answer 253

Increases rapidly

Answer 254

Drops to zero

Answer 255

0.66 cm¯¹

Answer 256

0.142 cm¯¹

Answer 257

0.918 cm¯¹

Answer 258

1.12 cm¯¹

Answer 259

All electrochemical reactions involve the transfer of electrons

Answer 260

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

Answer 261

Reduction occurs at cathode

Answer 262

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

Answer 263

Chloroform

Answer 264

Pure distilled water

Answer 265

Dilute solution of glucose

Answer 266

Molten NaCl

Answer 267

0.1 N NaCl

Answer 268

Both A and B

Answer 269

None of these

Answer 270

Electrorefining

Answer 271

Electroplating

Answer 272

Not particular

Answer 273

It has not potential

Answer 274

22400 cm³

Answer 275

Ca(NO₃)₂

Answer 276

Electrical energy is converted into heat

Answer 277

Chemical energy is converted into electricity

Answer 278

Electrical energy is converted into chemical energy

Answer 279

Chemical energy is converted into heat

Answer 280

Magnetic energy

Answer 281

Heat energy

Answer 282

Electrical energy

Answer 283

Sound energy

Answer 284

All of these

Answer 285

Oxidation-reduction

Answer 286

Depends on the nature of the coupled electrode

Answer 287

None of these

Answer 288

Exactly equal to one

Answer 289

Slightly less than one

Answer 290

Slightly greater than one

Answer 291

None of these

Answer 292

Heat energy

Answer 293

Electrical energy

Answer 294

Chemical energy

Answer 295

Weak acid and its salt of strong base

Answer 296

Weak acid and its salt of weak base

Answer 297

A strong acid and its salt of a strong base

Answer 298

Strong acid and its salt of weak base

Answer 299

Na and S only

Answer 300

Pt and graphite only

Answer 301

Na, Pt and graphite

Answer 302

Standard reduction potential

Answer 303

Ionization potential

Answer 304

Standard oxidation potential

Answer 305

Cell voltage

Answer 306

Possesses ions even in solid state

Answer 307

Forms complex ions in solution

Answer 308

Gives ions only when dissolved in water

Answer 309

Gives ions only when electricity is passed

Answer 310

1.06 x 10³

Answer 311

1.06 x 10⁴

Answer 312

1.06 x 10²

Answer 313

Electrochemical equivalent

Answer 314

One gm. Equivalent weight

Answer 315

One gm. atomic weight

Answer 316

None of these

Answer 317

1 – 2 α

Answer 318

Raoult’s law

Answer 319

Henry’s law

Answer 320

Distribution law

Answer 321

Ostwald’s dilution law

Answer 322

Sum of reduction and oxidation potentials

Answer 323

None of these

Answer 324

Fractional distillation

Answer 325

Distillation

Answer 326

Vacuum distillation

Answer 327

Neither a nor b

Answer 328

Concentration solutions behave as nearly non – ideal solutions

Answer 329

Dilute solution which behave as nearly ideal solution

Answer 330

Both a and b

Answer 331

Solvent particles

Answer 332

Hydrolyzed

Answer 333

Precipitated

Answer 334

Increase in oxidation number of all the elements on reactant side

Answer 335

Decrease in oxidation number

Answer 336

Both are possible

Answer 337

Increase in oxidation number

Answer 338

Ostwald’s law

Answer 339

Raoult’s law

Answer 340

Henry’s law

Answer 341

Arrhenius law

Answer 342

Union between two light metals and a heavy metal

Answer 343

Altered reaction in presence of H₂O

Answer 344

Electrochemical phenomenon

Answer 345

Interaction

Answer 346

Has low boiling point

Answer 347

Is readily decomposed

Answer 348

Is almost unionized

Answer 349

Is neutral

Answer 350

Oxidation number neither increases nor decreases

Answer 351

Increase in oxidation number of element

Answer 352

Decrease in oxidation number of element

Answer 353

Increase in oxidation number of the elements in reactants

Answer 354

Boiling point of pure water decreases by the addition of ethanol

Answer 355

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

Answer 356

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 357

Boiling point of pure benzene increases by the addition of toluene

Answer 358

None of these

Answer 359

Decreases with dilution

Answer 360

Increases with dilution

Answer 361

Remains unchanged with dilution

Answer 362

Depends on mass of electrolyte

Answer 363

Neutralization

Answer 364

Non-spontaneous reaction

Answer 365

Spontaneous reaction

Answer 366

58.5g NaCl/100ml

Answer 367

20g NaCl/100ml

Answer 368

5.58g NaCl/100m

Answer 369

10.0g NaCl/100ml

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