Chemistry Electro Chemistry Online Mcqs Test

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Question 1

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

Answer

800 mm of Hg

Answer

780 mm of Hg

Answer

750 mm of Hg

Answer

760 mm of Hg

Question 2

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 3

3. 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 4

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

Answer

Microgram percent

Answer

Parts per million

Answer

Gram per million

Answer

Milligram percent

Question 5

5. The osmotic pressure of 1 m solution at 27°C is

Question 6

6. In a chemical reaction, oxidation process involves

Answer

Increase in oxidation number of element

Answer

Decrease in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Answer

Oxidation number neither increases nor decreases

Question 7

7. Corrosion reactions are

Answer

Non-spontaneous redox reactions

Answer

Spontaneous acid–base reactions

Answer

None of these

Answer

Spontaneous redox reactions

Question 8

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

Answer

0.1 N NaCl

Question 9

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

Question 10

10. Decrease in oxidation number is called

Answer

All of these

Question 11

11. Oxidation number of carbon in NaHCO₃ is

Question 12

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

Answer

CH₃ CooNH₄

Answer

Na₂SO₄

Question 13

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

Question 14

14. During a redox reaction, an oxidizing agent

Answer

Loses electrons

Answer

Is hydrolysed

Answer

Gains electrons

Answer

Is oxidized

Question 15

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

Answer

Electrorefining

Answer

None of these

Answer

Both A and B

Answer

Electroplating

Question 16

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

Answer

∆ G = -ve

Answer

∆ G = -ve, ∆ E = 0

Answer

∆ G = +ve, ∆ E = 0

Answer

∆ G = 0, ∆E = 0

Question 17

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

Answer

Electric change

Answer

Ionization potential

Answer

Standard electrode potential

Answer

Electroplating

Question 18

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

Question 19

19. 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¯²

Answer

S² m² mol

Answer

S m mol¯¹

Answer

S m² mol¯¹

Question 20

20. Chemical used in salt bridge is

Question 21

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

Question 22

22. Salt bridge transfers

Answer

Solvent particles

Question 23

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

Question 24

24. The unit of specific conductivity is

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯¹

Answer

Ohm cm¯²

Answer

Ohm¯¹ cm

Question 25

25. Stronger the oxidizing agent, greater is the

Answer

Reduction potential

Answer

Redox potential

Answer

Oxidation potential

Answer

e.m.f of cell

Question 26

26. Corrosion is basically a

Answer

Electrochemical phenomenon

Answer

Interaction

Answer

Union between two light metals and a heavy metal

Answer

Altered reaction in presence of H₂O

Question 27

27. Salt bridge transfers

Question 28

28. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 29

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

Question 30

30. 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 31

31. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 32

32. Camphor is often used in molecular mass determination because

Answer

It has a very high cryoscopic constant

Answer

It is volatile

Answer

It is solvent for organic substances

Answer

It is readily available

Question 33

33. Which of the following statements is FALSE?

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

Answer

Reduction occurs at cathode

Question 34

34. Best way to prevent rusting iron is by

Answer

None of these

Answer

Both of these

Answer

Making iron cathode

Answer

Putting it in saline water

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

Answer

Decrease rapidly

Answer

Decreases slowly

Answer

Drops to zero

Answer

Does not change

Question 37

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

Question 38

38. Strong reducing agents have

Answer

None of these

Answer

Greater positive value of standard reduction potential

Answer

Lesser positive value of standard reduction potential

Answer

Greater negative value of standard reduction potential

Question 39

39. Molarity of water is

Question 40

40. When common salt is dissolved in water

Answer

Any possibility

Answer

B.P of water decrease

Answer

B.P of water remain constant

Answer

B.P of water increase

Question 41

41. Pick out the wrong statement. In electrochemical cell

Answer

Salt bridge maintains the electrical neutrality of the solution

Answer

Electrons are released at anode

Answer

Chemical energy is converted into electrical energy

Answer

Cathode is regarded as negative electrode

Question 42

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

Question 43

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

Answer

Rust removal

Answer

Manufacture of bleach

Answer

Making leather

Answer

Electroplating

Question 44

44. Pure water does not conduct electricity because it

Answer

Is readily decomposed

Answer

Has low boiling point

Answer

Is almost unionized

Answer

Is neutral

Question 45

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

Answer

Refractive index

Answer

Osmotic pressure

Answer

Surface tension

Question 46

46. Temperature for standard electrode potential is

Question 47

47. When electricity is passed through molten Al₂O₃ + Na₃AIF₆ and 13.5 gms of Al are deposited, the number of faraday must be

Question 48

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

Answer

Precipitated

Answer

Hydrolyzed

Question 49

49. The Vant Hoff factor (i) accounts for

Answer

The degree of decomposition of solution

Answer

The extent of dissociation of solute

Answer

Degree of solubilization of solute

Answer

The extent of dissolution of solute

Question 50

50. Cathodic reaction in the electrolysis of dil. H₂SO₄ is always

Question 51

51. Which has maximum oxidation number

Question 52

52. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 53

53. Potential of Zn is called

Answer

It has not potential

Question 54

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

Answer

Gold has higher reduction potential then iron

Answer

Iron rusts

Answer

Gold is denser

Answer

Gold has lower reduction potential then iron

Question 55

55. 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 56

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

Answer

Supersaturated

Answer

Unsaturated

Question 57

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

Answer

Galvanic cell

Answer

Electrolytic cell

Question 58

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

Answer

Does not change

Answer

Drops to zero

Answer

Increases rapidly

Answer

Increases gradually

Question 59

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

Answer

None of these

Answer

O₂, SO₂

Question 60

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

Answer

Vacuum distillation

Answer

Fractional distillation

Answer

None of these

Answer

Distillation

Question 61

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

Answer

Acts as a catalyst

Answer

Loses electrons

Answer

pH is changed

Answer

Gains electrons

Question 62

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

Question 63

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

Answer

Galvanic cell

Answer

Daniel cell

Answer

Electrolytic cell

Question 64

64. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Answer 128

Does not provide any electron

Answer 129

Neutral atom

Answer 130

Metals have high resistance

Answer 131

In metals the ions are free to more

Answer 132

Metals are decomposed by current

Answer 133

They are mobile electrons in the metallic structure

Answer 134

Equal to the total volume of the components

Answer 135

Slightly more than the total volume of the components

Answer 136

None of these

Answer 137

Slightly less than the total volume of the components

Answer 138

Concentration solutions behave as nearly non – ideal solutions

Answer 139

Both a and b

Answer 140

Neither a nor b

Answer 141

Dilute solution which behave as nearly ideal solution

Answer 142

1.0 x 10¹⁰

Answer 143

4.0 x 10¹²

Answer 144

1.0 x 10²

Answer 145

2.0 x 10¹¹

Answer 146

278 S cm² mol¯¹

Answer 147

128 S cm² mol¯¹

Answer 148

302 S cm² mol¯¹

Answer 149

176 S cm² mol¯¹

Answer 150

120 g Cm³

Answer 151

1.25g/Cm³

Answer 152

1.2 g/Cm³

Answer 153

1.15 g/Cm³

Answer 154

Ionization

Answer 155

Hydrolysis

Answer 156

Hypertonic

Answer 157

Thomas Gradam

Answer 158

Sound energy

Answer 159

Magnetic energy

Answer 160

Electrical energy

Answer 161

Heat energy

Answer 162

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

Answer 163

Li is smaller in size as compared to Cu

Answer 164

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

Answer 165

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

Answer 166

No connection exists

Answer 167

Electric circuit

Answer 168

Salt Bridge

Answer 169

H₄P₃O₇

Answer 170

Increase in oxidation number of all the elements on reactant side

Answer 171

Decrease in oxidation number

Answer 172

Increase in oxidation number

Answer 173

Both are possible

Answer 174

Non-spontaneous reaction

Answer 175

Spontaneous reaction

Answer 176

Neutralization

Answer 177

Anode to cathode through the external circuit

Answer 178

Cathode to anode through the external circuit

Answer 179

Anode to cathode through the solution

Answer 180

Cathode to anode through the solution

Answer 181

Na and S only

Answer 182

Pt and graphite only

Answer 183

Na, Pt and graphite

Answer 184

Electron transfer

Answer 185

Proton transfer

Answer 186

Ion combination reaction

Answer 187

A reaction in a solution

Answer 188

Sufficient date not given

Answer 189

Molarity of the solution

Answer 190

Molarity of the solvent

Answer 191

Mole fraction of the solution

Answer 192

Molality of the solution

Answer 193

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

Answer 194

None of these

Answer 195

Electrons flow cathode to anode within the electrolytic solution

Answer 196

Electrons flow from cathode to anode through the external battery

Answer 197

0.1 M Sucrose

Answer 198

0.1 M NaCl

Answer 199

0.1 M BaCl₂

Answer 200

0.1 M Glucose

Answer 201

None of these

Answer 202

Atoms of Na and Cl.

Answer 203

Free electrons

Answer 204

Free molecules

Answer 205

The enthalpy of mixing is zero

Answer 206

The free energy of mixing is zero

Answer 207

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

Answer 208

The entropy of mixing is zero

Answer 209

One gm. atomic weight

Answer 210

Electrochemical equivalent

Answer 211

One gm. Equivalent weight

Answer 212

None of these

Answer 213

0.66 cm¯¹

Answer 214

0.918 cm¯¹

Answer 215

0.142 cm¯¹

Answer 216

1.12 cm¯¹

Answer 217

Ca(NO₃)₂

Answer 218

96500 g of CU

Answer 219

100 g of Cu

Answer 220

63.5 g of Cu

Answer 221

31.75 g of Cu

Answer 222

– 1.17 V

Answer 223

– 0.35 V

Answer 224

[Pt(NH₃)₄Cl₄]

Answer 225

[Pt(NH₃)₄Cl₃]Cl

Answer 226

[Pt(NH₃)₄Cl₂]Cl₂

Answer 227

[Pt(NH₃)₄Cl]Cl₃

Answer 228

All of these

Answer 229

Pressure of the gas

Answer 230

Nature of the gas

Answer 231

Temperature

Answer 232

Electrolysis

Answer 233

Electroplating

Answer 234

Conduction

Answer 235

Decreases on dilution

Answer 236

Increases on dilution slightly

Answer 237

Does not change on dilution

Answer 238

Depends on density of electrolyte itself.

Answer 239

Not particular

Answer 240

Dilution decreases

Answer 241

Pressure increases

Answer 242

Dilution increases

Answer 243

A chemical cell

Answer 244

An electrolytic cell

Answer 245

A voltaic cell

Answer 246

A galvanic cell

Answer 247

Na⁺ + e– → Na

Answer 248

Na → Na⁺ + e–

Answer 249

Br₂ + 2e – → 2Br –

Answer 250

2Br– → Br₂ + 2e –

Answer 251

Galvanization

Answer 252

Photo electrolysis

Answer 253

Electrolysis

Answer 254

Cathodic protection

Answer 255

Neutralization

Answer 256

Naphthalene

Answer 257

Equal to that of ethanol

Answer 258

More than that of H₂O

Answer 259

Equal to that of water

Answer 260

Less than that of water

Answer 261

Pure distilled water

Answer 262

Dilute solution of glucose

Answer 263

Molten NaCl

Answer 264

Chloroform

Answer 265

1.06 x 10³

Answer 266

1.06 x 10²

Answer 267

1.06 x 10⁴

Answer 268

H+ and OH-

Answer 269

At cathode

Answer 270

None of these

Answer 271

Both A and B

Answer 272

12157.48 sec

Answer 273

22400 cm³

Answer 274

Inversion point

Answer 275

Melting point

Answer 276

Sublimation point

Answer 277

Boiling point

Answer 278

Slightly greater than one

Answer 279

None of these

Answer 280

Exactly equal to one

Answer 281

Slightly less than one

Answer 282

Non rechargeable

Answer 283

Electrolytic cell

Answer 284

Daniel cell

Answer 285

Rechargeable

Answer 286

Ionization potential

Answer 287

Standard reduction potential

Answer 288

Standard oxidation potential

Answer 289

Cell voltage

Answer 290

A strong acid and its salt of a strong base

Answer 291

Strong acid and its salt of weak base

Answer 292

Weak acid and its salt of strong base

Answer 293

Weak acid and its salt of weak base

Answer 294

Depends on mass of electrolyte

Answer 295

Remains unchanged with dilution

Answer 296

Increases with dilution

Answer 297

Decreases with dilution

Answer 298

Very low ionization potential values

Answer 299

Reduction potentials are negative

Answer 300

Very high positive value of reduction potential

Answer 301

Very high negative values reduction potential

Answer 302

Hg₂Cl₂

Answer 303

Henry’s law

Answer 304

Raoult’s law

Answer 305

Arrhenius law

Answer 306

Ostwald’s law

Answer 307

58.5g NaCl/100ml

Answer 308

5.58g NaCl/100m

Answer 309

10.0g NaCl/100ml

Answer 310

20g NaCl/100ml

Answer 311

Possesses ions even in solid state

Answer 312

Forms complex ions in solution

Answer 313

Gives ions only when electricity is passed

Answer 314

Gives ions only when dissolved in water

Answer 315

Hg₂Cl₂

Answer 316

Depends on the nature of the coupled electrode

Answer 317

Oxidation-reduction

Answer 318

Slightly more than 1 atom

Answer 319

760 mm of Hg

Answer 320

None of these

Answer 321

Sum of reduction and oxidation potentials

Answer 322

Elevation in boiling point

Answer 323

Flow of solvent from a concentrated to a dilute solution

Answer 324

Ionic concentration

Answer 325

Diffusion rate of the solute

Answer 326

Both Na⁺ and CI¯

Answer 327

None of these

Answer 328

By heating it

Answer 329

By replacing external circuit with external source of electricity

Answer 330

By addition of fresh solution

Answer 331

By removal of solution

Answer 332

1 – 2 α

Answer 333

Electrical energy is converted into chemical energy

Answer 334

Chemical energy is converted into heat

Answer 335

Electrical energy is converted into heat

Answer 336

Chemical energy is converted into electricity

Answer 337

None of these

Answer 338

From cathode to anode in outer circuit

Answer 339

From anode to cathode inside the cell

Answer 340

From cathode to anode inside the cell

Answer 341

From anode to cathode in an outer circuit

Answer 342

1.81 cm¯³

Answer 343

2.15 cm¯³

Answer 344

1.15 cm¯³

Answer 345

1.25 cm¯³

Answer 346

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

Answer 347

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

Answer 348

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

Answer 349

Hg is more inert than Pt

Answer 350

Ostwald’s dilution law

Answer 351

Henry’s law

Answer 352

Raoult’s law

Answer 353

Distribution law

Answer 354

Remove adsorbed oxygen from electrode surfaces

Answer 355

Generate heat

Answer 356

Produce high purity water

Answer 357

Create potential difference between two electrodes

Answer 358

Chemical energy

Answer 359

None of these

Answer 360

Electrical energy

Answer 361

Heat energy

Answer 362

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 363

Boiling point of pure water decreases by the addition of ethanol

Answer 364

Boiling point of pure benzene increases by the addition of toluene

Answer 365

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

Answer 366

Phosphorus acid

Answer 367

Nitric acid

Answer 368

Boric acid

Answer 369

Sulphuric acid

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