Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer

Boiling point of pure water decreases by the addition of ethanol

Question 2

2. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

Question 3

3. Density of H₂SO₄ in lead accumulator is

Question 4

4. 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 5

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

Answer

Rust removal

Answer

Making leather

Answer

Electroplating

Answer

Manufacture of bleach

Question 6

6. The art of electroplating was given by

Answer

Thomas Gradam

Question 7

7. The unit of specific conductivity is

Answer

Ohm¯¹ cm

Answer

Ohm cm¯²

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯¹

Question 8

8. Temperature for standard electrode potential is

Question 9

9. Potential of Zn is called

Answer

It has not potential

Question 10

10. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 11

11. After adding a solute freezing point of solvent decreases to -0.186. Calculate ∆ Tb if Kf = 1.86 and Kb = 0.521

Question 12

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

Answer

Standard electrode potential

Answer

Ionization potential

Answer

Electroplating

Answer

Electric change

Question 13

13. Azeotropic mixture of HCl and water has

Question 14

14. 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 15

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

Answer

Not particular

Question 16

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

Answer

CH₃ CooNH₄

Answer

Na₂SO₄

Question 17

17. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 18

18. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 19

19. 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 20

20. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 21

21. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

Question 22

22. In a Galvanic cell, the electrons flow from

Answer

Cathode to anode through the external circuit

Answer

Anode to cathode through the external circuit

Answer

Anode to cathode through the solution

Answer

Cathode to anode through the solution

Question 23

23. 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 24

24. Voltaic cell can be recharged by

Answer

By heating it

Answer

By replacing external circuit with external source of electricity

Answer

By addition of fresh solution

Answer

By removal of solution

Question 25

25. Maximum freezing point falls in

Answer

Naphthalene

Question 26

26. Colligative properties are the properties of

Answer

Concentration solutions behave as nearly non – ideal solutions

Answer

Both a and b

Answer

Neither a nor b

Answer

Dilute solution which behave as nearly ideal solution

Question 27

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

Answer

A chemical cell

Answer

A galvanic cell

Answer

A voltaic cell

Answer

An electrolytic cell

Question 28

28. A redox reaction involves

Answer

Ion combination reaction

Answer

A reaction in a solution

Answer

Proton transfer

Answer

Electron transfer

Question 29

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

Question 30

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

Question 31

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

Answer

Gold has lower reduction potential then iron

Answer

Gold has higher reduction potential then iron

Answer

Iron rusts

Answer

Gold is denser

Question 32

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

Question 33

33. Oxidation state of hydrogen in CaH₂ is

Question 34

34. Which has maximum oxidation number

Question 35

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

Answer

Electrolysis

Answer

Photo electrolysis

Answer

Galvanization

Answer

Cathodic protection

Question 36

36. Alkaline battery has a voltage of

Question 37

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

Question 38

38. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 39

39. 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 40

40. Half cells are interconnected through

Answer

Electric circuit

Answer

Salt Bridge

Answer

No connection exists

Question 41

41. What are the ions present in water?

Answer

H+ and OH-

Question 42

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

Question 43

43. In alkaline battery anode is made up of

Question 44

44. 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

S² m² mol¯²

Answer

S m² mol¯¹

Answer

S m mol¯¹

Question 45

45. Electrolysis is the process in which a chemical reaction takes place at the expense of

Answer

Heat energy

Answer

Chemical energy

Answer

None of these

Answer

Electrical energy

Question 46

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

Answer

58.5g NaCl/100ml

Answer

10.0g NaCl/100ml

Answer

5.58g NaCl/100m

Answer

20g NaCl/100ml

Question 47

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

Question 48

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

Question 49

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

Question 50

50. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

Answer

Slightly more than the total volume of the components

Answer

Slightly less than the total volume of the components

Answer

Equal to the total volume of the components

Answer

None of these

Question 51

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

Answer

Reduction potentials are negative

Answer

Very high positive value of reduction potential

Answer

Very low ionization potential values

Answer

Very high negative values reduction potential

Question 52

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

Answer

Slightly more than 1 atom

Answer

760 mm of Hg

Question 53

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

Question 54

54. The best reducing agent is

Question 55

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 56

56. What is the molarity of H₂SO₄ solution that has density of 1.84 gm/cm³ which was at 35°C and contains 98% by weight?

Question 57

57. Units of molarity are

Answer

None of these

Question 58

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

Answer

None of these

Answer

Both Na⁺ and CI¯

Question 59

59. Which one of the following will be good conductor of electricity?

Answer

Molten NaCl

Answer

Pure distilled water

Answer

Chloroform

Answer

Dilute solution of glucose

Question 60

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

Answer

0.1 M Sucrose

Answer

0.1 M Glucose

Answer

0.1 M NaCl

Answer

0.1 M BaCl₂

Question 61

61. 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 62

62. 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

4.0 x 10¹²

Answer

1.0 x 10¹⁰

Answer

2.0 x 10¹¹

Answer

1.0 x 10²

Question 63

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

Question 64

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

Answer 105

Neutral atom

Answer 106

Does not provide any electron

Answer 107

Galvanic cell

Answer 108

Electrolytic cell

Answer 109

The extent of dissociation of solute

Answer 110

The extent of dissolution of solute

Answer 111

Degree of solubilization of solute

Answer 112

The degree of decomposition of solution

Answer 113

It is readily available

Answer 114

It is solvent for organic substances

Answer 115

It is volatile

Answer 116

It has a very high cryoscopic constant

Answer 117

Remains unchanged with dilution

Answer 118

Increases with dilution

Answer 119

Depends on mass of electrolyte

Answer 120

Decreases with dilution

Answer 121

Na, Pt and graphite

Answer 122

Na and S only

Answer 123

Pt and graphite only

Answer 124

None of these

Answer 125

Both A and B

Answer 126

At cathode

Answer 127

Remove adsorbed oxygen from electrode surfaces

Answer 128

Produce high purity water

Answer 129

Create potential difference between two electrodes

Answer 130

Generate heat

Answer 131

Oxidation-reduction

Answer 132

Depends on the nature of the coupled electrode

Answer 133

Sum of reduction and oxidation potentials

Answer 134

Mole fraction of the solution

Answer 135

Molality of the solution

Answer 136

Molarity of the solution

Answer 137

Molarity of the solvent

Answer 138

Galvanic cell

Answer 139

Electrolytic cell

Answer 140

Daniel cell

Answer 141

Neutralization

Answer 142

Non-spontaneous reaction

Answer 143

Spontaneous reaction

Answer 144

Ca(NO₃)₂

Answer 145

22400 cm³

Answer 146

Dilution decreases

Answer 147

Dilution increases

Answer 148

Pressure increases

Answer 149

Electroplating

Answer 150

Both A and B

Answer 151

None of these

Answer 152

Electrorefining

Answer 153

Osmotic pressure

Answer 154

Surface tension

Answer 155

Refractive index

Answer 156

O₂, SO₂

Answer 157

None of these

Answer 158

Standard reduction potential

Answer 159

Cell voltage

Answer 160

Standard oxidation potential

Answer 161

Ionization potential

Answer 162

All of these

Answer 163

Henry’s law

Answer 164

Raoult’s law

Answer 165

Ostwald’s law

Answer 166

Arrhenius law

Answer 167

Gram per million

Answer 168

Milligram percent

Answer 169

Parts per million

Answer 170

Microgram percent

Answer 171

Increase in oxidation number of the elements in reactants

Answer 172

Oxidation number neither increases nor decreases

Answer 173

Increase in oxidation number of element

Answer 174

Decrease in oxidation number of element

Answer 175

Hydrolysis

Answer 176

Ionization

Answer 177

Free molecules

Answer 178

Free electrons

Answer 179

Atoms of Na and Cl.

Answer 180

2.15 cm¯³

Answer 181

1.15 cm¯³

Answer 182

1.81 cm¯³

Answer 183

1.25 cm¯³

Answer 184

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

Answer 185

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

Answer 186

Li is smaller in size as compared to Cu

Answer 187

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

Answer 188

From cathode to anode in outer circuit

Answer 189

From anode to cathode inside the cell

Answer 190

From anode to cathode in an outer circuit

Answer 191

From cathode to anode inside the cell

Answer 192

31.75 g of Cu

Answer 193

96500 g of CU

Answer 194

63.5 g of Cu

Answer 195

100 g of Cu

Answer 196

0.1 N NaCl

Answer 197

760 mm of Hg

Answer 198

800 mm of Hg

Answer 199

750 mm of Hg

Answer 200

780 mm of Hg

Answer 201

None of these

Answer 202

Fractional distillation

Answer 203

Vacuum distillation

Answer 204

Distillation

Answer 205

1 – 2 α

Answer 206

Hg₂Cl₂

Answer 207

None of these

Answer 208

One gm. atomic weight

Answer 209

Electrochemical equivalent

Answer 210

One gm. Equivalent weight

Answer 211

Solvent particles

Answer 212

Precipitated

Answer 213

Hydrolyzed

Answer 214

12157.48 sec

Answer 215

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

Answer 216

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

Answer 217

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

Answer 218

Hg is more inert than Pt

Answer 219

B.P of water increase

Answer 220

Any possibility

Answer 221

B.P of water decrease

Answer 222

B.P of water remain constant

Answer 223

[Pt(NH₃)₄Cl₂]Cl₂

Answer 224

[Pt(NH₃)₄Cl₄]

Answer 225

[Pt(NH₃)₄Cl₃]Cl

Answer 226

[Pt(NH₃)₄Cl]Cl₃

Answer 227

∆ G = +ve, ∆ E = 0

Answer 228

∆ G = -ve

Answer 229

∆ G = 0, ∆E = 0

Answer 230

∆ G = -ve, ∆ E = 0

Answer 231

176 S cm² mol¯¹

Answer 232

128 S cm² mol¯¹

Answer 233

278 S cm² mol¯¹

Answer 234

302 S cm² mol¯¹

Answer 235

Chemical energy is converted into electrical energy

Answer 236

Electrons are released at anode

Answer 237

Cathode is regarded as negative electrode

Answer 238

Salt bridge maintains the electrical neutrality of the solution

Answer 239

None of these

Answer 240

Electrons flow cathode to anode within the electrolytic solution

Answer 241

None of these

Answer 242

Electrons flow from cathode to anode through the external battery

Answer 243

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

Answer 244

H₄P₃O₇

Answer 245

1.25g/Cm³

Answer 246

1.2 g/Cm³

Answer 247

1.15 g/Cm³

Answer 248

120 g Cm³

Answer 249

Electrochemical phenomenon

Answer 250

Union between two light metals and a heavy metal

Answer 251

Altered reaction in presence of H₂O

Answer 252

Interaction

Answer 253

Increases on dilution slightly

Answer 254

Depends on density of electrolyte itself.

Answer 255

Decreases on dilution

Answer 256

Does not change on dilution

Answer 257

Slightly greater than one

Answer 258

Slightly less than one

Answer 259

Exactly equal to one

Answer 260

None of these

Answer 261

Is neutral

Answer 262

Is readily decomposed

Answer 263

Has low boiling point

Answer 264

Is almost unionized

Answer 265

All of these

Answer 266

Pressure of the gas

Answer 267

Nature of the gas

Answer 268

Temperature

Answer 269

Strong acid and its salt of weak base

Answer 270

A strong acid and its salt of a strong base

Answer 271

Weak acid and its salt of strong base

Answer 272

Weak acid and its salt of weak base

Answer 273

Heat energy

Answer 274

Electrical energy

Answer 275

Magnetic energy

Answer 276

Sound energy

Answer 277

1.12 cm¯¹

Answer 278

0.142 cm¯¹

Answer 279

0.918 cm¯¹

Answer 280

0.66 cm¯¹

Answer 281

Na → Na⁺ + e–

Answer 282

2Br– → Br₂ + 2e –

Answer 283

Na⁺ + e– → Na

Answer 284

Br₂ + 2e – → 2Br –

Answer 285

Melting point

Answer 286

Boiling point

Answer 287

Sublimation point

Answer 288

Inversion point

Answer 289

Electrolytic cell

Answer 290

Non rechargeable

Answer 291

Daniel cell

Answer 292

Rechargeable

Answer 293

Forms complex ions in solution

Answer 294

Possesses ions even in solid state

Answer 295

Gives ions only when electricity is passed

Answer 296

Gives ions only when dissolved in water

Answer 297

Sufficient date not given

Answer 298

Hg₂Cl₂

Answer 299

More than that of H₂O

Answer 300

Equal to that of water

Answer 301

Less than that of water

Answer 302

Equal to that of ethanol

Answer 303

Electrolysis

Answer 304

Electroplating

Answer 305

Conduction

Answer 306

None of these

Answer 307

Ostwald’s dilution law

Answer 308

Raoult’s law

Answer 309

Henry’s law

Answer 310

Distribution law

Answer 311

Electrical energy is converted into chemical energy

Answer 312

Chemical energy is converted into electricity

Answer 313

Chemical energy is converted into heat

Answer 314

Electrical energy is converted into heat

Answer 315

Spontaneous redox reactions

Answer 316

Spontaneous acid–base reactions

Answer 317

None of these

Answer 318

Non-spontaneous redox reactions

Answer 319

Putting it in saline water

Answer 320

Both of these

Answer 321

Making iron cathode

Answer 322

None of these

Answer 323

In metals the ions are free to more

Answer 324

Metals have high resistance

Answer 325

Metals are decomposed by current

Answer 326

They are mobile electrons in the metallic structure

Answer 327

Elevation in boiling point

Answer 328

Ionic concentration

Answer 329

Flow of solvent from a concentrated to a dilute solution

Answer 330

Diffusion rate of the solute

Answer 331

The entropy of mixing is zero

Answer 332

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

Answer 333

The enthalpy of mixing is zero

Answer 334

The free energy of mixing is zero

Answer 335

Decrease in oxidation number

Answer 336

Increase in oxidation number of all the elements on reactant side

Answer 337

Both are possible

Answer 338

Increase in oxidation number

Answer 339

Increases gradually

Answer 340

Drops to zero

Answer 341

Does not change

Answer 342

Increases rapidly

Answer 343

Oxidation potential

Answer 344

Reduction potential

Answer 345

e.m.f of cell

Answer 346

Redox potential

Answer 347

Reduction occurs at cathode

Answer 348

All electrochemical reactions involve the transfer of electrons

Answer 349

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

Answer 350

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

Answer 351

Is oxidized

Answer 352

Is hydrolysed

Answer 353

Gains electrons

Answer 354

Loses electrons

Answer 355

Greater negative value of standard reduction potential

Answer 356

Greater positive value of standard reduction potential

Answer 357

None of these

Answer 358

Lesser positive value of standard reduction potential

Answer 359

– 1.17 V

Answer 360

– 0.35 V

Answer 361

1.06 x 10⁴

Answer 362

1.06 x 10²

Answer 363

1.06 x 10³

Answer 364

Supersaturated

Answer 365

Unsaturated

Answer 366

Nitric acid

Answer 367

Sulphuric acid

Answer 368

Boric acid

Answer 369

Phosphorus acid

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