Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Choose the best reducing agent among the following

Question 2

2. Chemical used in salt bridge is

Question 3

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

Answer

H₄P₃O₇

Question 4

4. 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 5

5. 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 6

6. The relative lowering of vapour pressure is equal to mole fraction of the solute. This law is called:

Answer

Arrhenius law

Answer

Raoult’s law

Answer

Ostwald’s law

Answer

Henry’s law

Question 7

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

Answer

Supersaturated

Answer

Unsaturated

Question 8

8. Decrease in oxidation number is called

Answer

All of these

Question 9

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

Answer

5.58g NaCl/100m

Answer

20g NaCl/100ml

Answer

10.0g NaCl/100ml

Answer

58.5g NaCl/100ml

Question 10

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

Answer

Hydrolyzed

Answer

Precipitated

Question 11

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

Question 12

12. In an electrolytic cell current flows

Answer

From cathode to anode inside the cell

Answer

From anode to cathode in an outer circuit

Answer

From cathode to anode in outer circuit

Answer

From anode to cathode inside the cell

Question 13

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

Question 14

14. The unit of specific conductivity is

Answer

Ohm¯¹ cm

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯²

Answer

Ohm cm¯¹

Question 15

15. 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 16

16. In a Galvanic cell, the electrons flow from

Answer

Anode to cathode through the solution

Answer

Cathode to anode through the external circuit

Answer

Cathode to anode through the solution

Answer

Anode to cathode through the external circuit

Question 17

17. 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 18

18. In a Galvanic cell

Answer

Electrical energy is converted into heat

Answer

Chemical energy is converted into heat

Answer

Electrical energy is converted into chemical energy

Answer

Chemical energy is converted into electricity

Question 19

19. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 20

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

Question 21

21. The depression of freezing point is directly proportional to

Answer

Mole fraction of the solution

Answer

Molality of the solution

Answer

Molarity of the solution

Answer

Molarity of the solvent

Question 22

22. 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 23

23. 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 24

24. During a redox reaction, an oxidizing agent

Answer

Loses electrons

Answer

Is hydrolysed

Answer

Gains electrons

Answer

Is oxidized

Question 25

25. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 26

26. Which of the statements given below concerning properties of solution, describe a colligaive effect?

Answer

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer

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

Answer

Boiling point of pure benzene increases by the addition of toluene

Answer

Boiling point of pure water decreases by the addition of ethanol

Question 27

27. 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 28

28. Oxidation number of carbon in NaHCO₃ is

Question 29

29. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 30

30. A redox reaction involves

Answer

A reaction in a solution

Answer

Proton transfer

Answer

Electron transfer

Answer

Ion combination reaction

Question 31

31. 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

Weak acid and its salt of weak base

Answer

A strong acid and its salt of a strong base

Question 32

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

Answer

Distillation

Answer

None of these

Answer

Vacuum distillation

Answer

Fractional distillation

Question 33

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

Answer

Equal to that of ethanol

Answer

More than that of H₂O

Answer

Less than that of water

Answer

Equal to that of water

Question 34

34. Molarity of water is

Question 35

35. Electrochemical series is a list of elements arranged into increasing order to either

Answer

Cell voltage

Answer

Standard reduction potential

Answer

Standard oxidation potential

Answer

Ionization potential

Question 36

36. The electrode with more negative value of reduction potential acts as

Answer

None of these

Question 37

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

Answer

– 0.35 V

Answer

– 1.17 V

Question 38

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

Question 39

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

Question 40

40. Molton NaCl conducts electricity due to the presence of

Answer

Free electrons

Answer

Free molecules

Answer

Atoms of Na and Cl.

Question 41

41. 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 42

42. Azeotropic mixture of HCl and water has

Question 43

43. Best way to prevent rusting iron is by

Answer

Both of these

Answer

None of these

Answer

Making iron cathode

Answer

Putting it in saline water

Question 44

44. If 18 g of glucose (C₆H₁₂C₆) is present in 1000 g of an aqueous solution of glucose it is said to be

Question 45

45. 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 46

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

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

Answer

Gains electrons

Answer

pH is changed

Answer

Loses electrons

Answer

Acts as a catalyst

Question 49

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

Answer

Elevation in boiling point

Answer

Diffusion rate of the solute

Answer

Ionic concentration

Answer

Flow of solvent from a concentrated to a dilute solution

Question 50

50. Stronger the oxidizing agent, greater is the

Answer

Reduction potential

Answer

Redox potential

Answer

Oxidation potential

Answer

e.m.f of cell

Question 51

51. Potential of Zn is called

Answer

It has not potential

Question 52

52. In a chemical reaction, oxidation process involves

Answer

Oxidation number neither increases nor decreases

Answer

Decrease in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Answer

Increase in oxidation number of element

Question 53

53. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 54

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

Question 55

55. 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 low ionization potential values

Answer

Very high negative values reduction potential

Answer

Very high positive value of reduction potential

Answer

Reduction potentials are negative

Question 56

56. 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 57

57. Which of the following statement is correct for electrolytic cell?

Answer

Electrons flow from cathode to anode through the external battery

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

None of these

Answer

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

Question 58

58. The conductivity of strong electrolyte

Answer

Depends on density of electrolyte itself.

Answer

Increases on dilution slightly

Answer

Decreases on dilution

Answer

Does not change on dilution

Question 59

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

Answer

∆ G = -ve, ∆ E = 0

Answer

∆ G = +ve, ∆ E = 0

Answer

∆ G = 0, ∆E = 0

Answer

∆ G = -ve

Question 60

60. 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 61

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

Question 62

62. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 63

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

Question 64

64. In alkaline battery the anode is made up of

Answer 117

Dilute solution of glucose

Answer 118

Chloroform

Answer 119

Pure distilled water

Answer 120

Molten NaCl

Answer 121

Boric acid

Answer 122

Sulphuric acid

Answer 123

Nitric acid

Answer 124

Phosphorus acid

Answer 125

100 g of Cu

Answer 126

63.5 g of Cu

Answer 127

31.75 g of Cu

Answer 128

96500 g of CU

Answer 129

Dilution increases

Answer 130

Dilution decreases

Answer 131

Pressure increases

Answer 132

Solvent particles

Answer 133

Osmotic pressure

Answer 134

Surface tension

Answer 135

Refractive index

Answer 136

Chemical energy is converted into electrical energy

Answer 137

Electrons are released at anode

Answer 138

Cathode is regarded as negative electrode

Answer 139

Salt bridge maintains the electrical neutrality of the solution

Answer 140

1.25g/Cm³

Answer 141

1.15 g/Cm³

Answer 142

120 g Cm³

Answer 143

1.2 g/Cm³

Answer 144

Hypertonic

Answer 145

Decrease in oxidation number

Answer 146

Both are possible

Answer 147

Increase in oxidation number

Answer 148

Increase in oxidation number of all the elements on reactant side

Answer 149

Ionization potential

Answer 150

Electroplating

Answer 151

Standard electrode potential

Answer 152

Electric change

Answer 153

The enthalpy of mixing is zero

Answer 154

The entropy of mixing is zero

Answer 155

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

Answer 156

The free energy of mixing is zero

Answer 157

None of these

Answer 158

Greater negative value of standard reduction potential

Answer 159

Lesser positive value of standard reduction potential

Answer 160

Greater positive value of standard reduction potential

Answer 161

Equal to the total volume of the components

Answer 162

Slightly less than the total volume of the components

Answer 163

Slightly more than the total volume of the components

Answer 164

None of these

Answer 165

None of these

Answer 166

Both Na⁺ and CI¯

Answer 167

Drops to zero

Answer 168

Decreases slowly

Answer 169

Decrease rapidly

Answer 170

Does not change

Answer 171

One gm. atomic weight

Answer 172

None of these

Answer 173

Electrochemical equivalent

Answer 174

One gm. Equivalent weight

Answer 175

Spontaneous acid–base reactions

Answer 176

None of these

Answer 177

Spontaneous redox reactions

Answer 178

Non-spontaneous redox reactions

Answer 179

Salt Bridge

Answer 180

Electric circuit

Answer 181

No connection exists

Answer 182

Na and S only

Answer 183

Pt and graphite only

Answer 184

Na, Pt and graphite

Answer 185

22400 cm³

Answer 186

None of these

Answer 187

1.06 x 10³

Answer 188

1.06 x 10²

Answer 189

1.06 x 10⁴

Answer 190

Spontaneous reaction

Answer 191

Neutralization

Answer 192

Non-spontaneous reaction

Answer 193

Decreases with dilution

Answer 194

Depends on mass of electrolyte

Answer 195

Remains unchanged with dilution

Answer 196

Increases with dilution

Answer 197

750 mm of Hg

Answer 198

800 mm of Hg

Answer 199

760 mm of Hg

Answer 200

780 mm of Hg

Answer 201

1.12 cm¯¹

Answer 202

0.66 cm¯¹

Answer 203

0.142 cm¯¹

Answer 204

0.918 cm¯¹

Answer 205

Possesses ions even in solid state

Answer 206

Gives ions only when electricity is passed

Answer 207

Gives ions only when dissolved in water

Answer 208

Forms complex ions in solution

Answer 209

Dilute solution which behave as nearly ideal solution

Answer 210

Both a and b

Answer 211

Concentration solutions behave as nearly non – ideal solutions

Answer 212

Neither a nor b

Answer 213

Oxidation-reduction

Answer 214

Depends on the nature of the coupled electrode

Answer 215

Rechargeable

Answer 216

Electrolytic cell

Answer 217

Daniel cell

Answer 218

Non rechargeable

Answer 219

None of these

Answer 220

Produce high purity water

Answer 221

Remove adsorbed oxygen from electrode surfaces

Answer 222

Create potential difference between two electrodes

Answer 223

Generate heat

Answer 224

Milligram percent

Answer 225

Microgram percent

Answer 226

Parts per million

Answer 227

Gram per million

Answer 228

Thomas Gradam

Answer 229

An electrolytic cell

Answer 230

A galvanic cell

Answer 231

A voltaic cell

Answer 232

A chemical cell

Answer 233

None of these

Answer 234

Electrical energy

Answer 235

Heat energy

Answer 236

Chemical energy

Answer 237

At cathode

Answer 238

None of these

Answer 239

Both A and B

Answer 240

Na₂SO₄

Answer 241

CH₃ CooNH₄

Answer 242

Electroplating

Answer 243

Manufacture of bleach

Answer 244

Rust removal

Answer 245

Making leather

Answer 246

1.0 x 10²

Answer 247

1.0 x 10¹⁰

Answer 248

4.0 x 10¹²

Answer 249

2.0 x 10¹¹

Answer 250

Has low boiling point

Answer 251

Is almost unionized

Answer 252

Is neutral

Answer 253

Is readily decomposed

Answer 254

Ca(NO₃)₂

Answer 255

The extent of dissociation of solute

Answer 256

The degree of decomposition of solution

Answer 257

The extent of dissolution of solute

Answer 258

Degree of solubilization of solute

Answer 259

Galvanic cell

Answer 260

Electrolytic cell

Answer 261

Neutral atom

Answer 262

Does not provide any electron

Answer 263

None of these

Answer 264

O₂, SO₂

Answer 265

Slightly greater than one

Answer 266

Exactly equal to one

Answer 267

None of these

Answer 268

Slightly less than one

Answer 269

[Pt(NH₃)₄Cl]Cl₃

Answer 270

[Pt(NH₃)₄Cl₄]

Answer 271

[Pt(NH₃)₄Cl₃]Cl

Answer 272

[Pt(NH₃)₄Cl₂]Cl₂

Answer 273

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

Answer 274

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

Answer 275

Li is smaller in size as compared to Cu

Answer 276

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

Answer 277

S m² mol¯¹

Answer 278

S² m² mol

Answer 279

S m mol¯¹

Answer 280

S² m² mol¯²

Answer 281

Not particular

Answer 282

Electrical energy

Answer 283

Heat energy

Answer 284

Sound energy

Answer 285

Magnetic energy

Answer 286

B.P of water increase

Answer 287

B.P of water decrease

Answer 288

Any possibility

Answer 289

B.P of water remain constant

Answer 290

Gold has higher reduction potential then iron

Answer 291

Gold is denser

Answer 292

Gold has lower reduction potential then iron

Answer 293

Iron rusts

Answer 294

By removal of solution

Answer 295

By addition of fresh solution

Answer 296

By heating it

Answer 297

By replacing external circuit with external source of electricity

Answer 298

Melting point

Answer 299

Boiling point

Answer 300

Inversion point

Answer 301

Sublimation point

Answer 302

Conduction

Answer 303

Electroplating

Answer 304

Electrolysis

Answer 305

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

Answer 306

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

Answer 307

Hg is more inert than Pt

Answer 308

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

Answer 309

Both A and B

Answer 310

None of these

Answer 311

Electrorefining

Answer 312

Electroplating

Answer 313

Hg₂Cl₂

Answer 314

2Br– → Br₂ + 2e –

Answer 315

Br₂ + 2e – → 2Br –

Answer 316

Na → Na⁺ + e–

Answer 317

Na⁺ + e– → Na

Answer 318

0.1 N NaCl

Answer 319

Does not change

Answer 320

Increases rapidly

Answer 321

Drops to zero

Answer 322

Increases gradually

Answer 323

Pressure of the gas

Answer 324

Temperature

Answer 325

Nature of the gas

Answer 326

All of these

Answer 327

In metals the ions are free to more

Answer 328

Metals are decomposed by current

Answer 329

They are mobile electrons in the metallic structure

Answer 330

Metals have high resistance

Answer 331

760 mm of Hg

Answer 332

Slightly more than 1 atom

Answer 333

Naphthalene

Answer 334

Altered reaction in presence of H₂O

Answer 335

Electrochemical phenomenon

Answer 336

Interaction

Answer 337

Union between two light metals and a heavy metal

Answer 338

1.81 cm¯³

Answer 339

2.15 cm¯³

Answer 340

1.15 cm¯³

Answer 341

1.25 cm¯³

Answer 342

Both oxidation and reduction

Answer 343

Neither oxidation and reduction

Answer 344

0.1 M NaCl

Answer 345

0.1 M Glucose

Answer 346

0.1 M BaCl₂

Answer 347

0.1 M Sucrose

Answer 348

Cathodic protection

Answer 349

Electrolysis

Answer 350

Galvanization

Answer 351

Photo electrolysis

Answer 352

H+ and OH-

Answer 353

1 – 2 α

Answer 354

It is readily available

Answer 355

It is solvent for organic substances

Answer 356

It is volatile

Answer 357

It has a very high cryoscopic constant

Answer 358

128 S cm² mol¯¹

Answer 359

278 S cm² mol¯¹

Answer 360

176 S cm² mol¯¹

Answer 361

302 S cm² mol¯¹

Answer 362

Ostwald’s dilution law

Answer 363

Henry’s law

Answer 364

Raoult’s law

Answer 365

Distribution law

Answer 366

Reduction occurs at cathode

Answer 367

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

Answer 368

All electrochemical reactions involve the transfer of electrons

Answer 369

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

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