Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Which of the following (IM) conducts more electricity?

Answer

Boric acid

Answer

Sulphuric acid

Answer

Phosphorus acid

Answer

Nitric acid

Question 2

2. Choose the best reducing agent among the following

Question 3

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

Answer

Making leather

Answer

Manufacture of bleach

Answer

Electroplating

Answer

Rust removal

Question 4

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

Answer

Strong acid and its salt of weak base

Answer

Weak acid and its salt of strong base

Answer

A strong acid and its salt of a strong base

Answer

Weak acid and its salt of weak base

Question 5

5. 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 6

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

Question 7

7. 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 8

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

Answer

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

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⁺

Question 9

9. Azeotropic mixture of HCl and water has

Question 10

10. 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 11

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

Answer

Na, Pt and graphite

Answer

Na and S only

Answer

Pt and graphite only

Question 12

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

Answer

Both Na⁺ and CI¯

Answer

None of these

Question 13

13. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 14

14. 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 15

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

Answer

Equal to that of ethanol

Answer

Equal to that of water

Answer

Less than that of water

Answer

More than that of H₂O

Question 16

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 17

17. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 18

18. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

Answer

Na → Na⁺ + e–

Answer

Br₂ + 2e – → 2Br –

Answer

2Br– → Br₂ + 2e –

Answer

Na⁺ + e– → Na

Question 19

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

Question 20

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

Question 21

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

Question 22

22. 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

1.0 x 10²

Answer

2.0 x 10¹¹

Question 23

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

Answer

Gold has lower reduction potential then iron

Answer

Iron rusts

Answer

Gold is denser

Answer

Gold has higher reduction potential then iron

Question 24

24. 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 25

25. When common salt is dissolved in water

Answer

B.P of water remain constant

Answer

Any possibility

Answer

B.P of water increase

Answer

B.P of water decrease

Question 26

26. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

Answer

0.918 cm¯¹

Answer

1.12 cm¯¹

Answer

0.66 cm¯¹

Answer

0.142 cm¯¹

Question 27

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

Answer

0.1 N NaCl

Question 28

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

Answer

Ionization potential

Answer

Cell voltage

Answer

Standard oxidation potential

Answer

Standard reduction potential

Question 29

29. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 30

30. 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

Boiling point of pure water decreases by the addition of ethanol

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

Question 31

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

Question 32

32. Stronger the oxidizing agent, greater is the

Answer

Oxidation potential

Answer

e.m.f of cell

Answer

Reduction potential

Answer

Redox potential

Question 33

33. 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 34

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

Answer

CH₃ CooNH₄

Answer

Na₂SO₄

Question 35

35. Cathode provides electrons to

Answer

Does not provide any electron

Answer

Neutral atom

Question 36

36. Temperature for standard electrode potential is

Question 37

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

Question 38

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

Answer

Henry’s law

Answer

Ostwald’s dilution law

Answer

Raoult’s law

Answer

Distribution law

Question 39

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

Answer

Electrical energy

Answer

None of these

Answer

Chemical energy

Answer

Heat energy

Question 40

40. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

Answer

128 S cm² mol¯¹

Answer

278 S cm² mol¯¹

Answer

176 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Question 41

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

Answer

Daniel cell

Answer

Electrolytic cell

Answer

Galvanic cell

Question 42

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

Question 43

43. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 44

44. In alkaline battery anode is made up of

Question 45

45. 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 46

46. 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 47

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

Question 48

48. During a redox reaction, an oxidizing agent

Answer

Is oxidized

Answer

Is hydrolysed

Answer

Loses electrons

Answer

Gains electrons

Question 49

49. What will be the density of H₂SO₄ when lead accumulator is recharged?

Answer

1.15 cm¯³

Answer

1.25 cm¯³

Answer

1.81 cm¯³

Answer

2.15 cm¯³

Question 50

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

Answer

None of these

Answer

Both A and B

Answer

Electrorefining

Answer

Electroplating

Question 51

51. When electricity is passed through molten electrolyte consisting of alumina and cryolite, 13.5 g of Al are deposited. The number of faradays of electricity passed must be

Question 52

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

Question 53

53. In the conversion of Br2 to BrO₃¯¹ the oxidation state of bromine changes from

Question 54

54. 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 55

55. Alkaline battery has a voltage of

Question 56

56. Oxidation number of carbon in NaHCO₃ is

Question 57

57. 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

Question 58

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

Answer

Chloroform

Answer

Molten NaCl

Answer

Pure distilled water

Answer

Dilute solution of glucose

Question 59

59. 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 60

60. 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

Answer

S m² mol¯¹

Answer

S² m² mol¯²

Question 61

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

Answer

0.1 M Glucose

Answer

0.1 M Sucrose

Answer

0.1 M BaCl₂

Answer

0.1 M NaCl

Question 62

62. 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 63

63. Secondary cell is

Answer

Non rechargeable

Answer

Daniel cell

Answer

Rechargeable

Answer

Electrolytic cell

Question 64

64. Units of molarity are

Answer

None of these

Answer 122

Electroplating

Answer 123

Ionization potential

Answer 124

Electric change

Answer 125

Standard electrode potential

Answer 126

Decreases on dilution

Answer 127

Depends on density of electrolyte itself.

Answer 128

Does not change on dilution

Answer 129

Increases on dilution slightly

Answer 130

Nature of the gas

Answer 131

All of these

Answer 132

Pressure of the gas

Answer 133

Temperature

Answer 134

Increase in oxidation number of element

Answer 135

Increase in oxidation number of the elements in reactants

Answer 136

Oxidation number neither increases nor decreases

Answer 137

Decrease in oxidation number of element

Answer 138

12157.48 sec

Answer 139

Diffusion rate of the solute

Answer 140

Flow of solvent from a concentrated to a dilute solution

Answer 141

Ionic concentration

Answer 142

Elevation in boiling point

Answer 143

[Pt(NH₃)₄Cl₃]Cl

Answer 144

[Pt(NH₃)₄Cl]Cl₃

Answer 145

[Pt(NH₃)₄Cl₄]

Answer 146

[Pt(NH₃)₄Cl₂]Cl₂

Answer 147

Hg₂Cl₂

Answer 148

– 1.17 V

Answer 149

– 0.35 V

Answer 150

Spontaneous reaction

Answer 151

Neutralization

Answer 152

Non-spontaneous reaction

Answer 153

22400 cm³

Answer 154

All of these

Answer 155

None of these

Answer 156

Slightly more than the total volume of the components

Answer 157

Equal to the total volume of the components

Answer 158

Slightly less than the total volume of the components

Answer 159

Naphthalene

Answer 160

From cathode to anode inside the cell

Answer 161

From cathode to anode in outer circuit

Answer 162

From anode to cathode inside the cell

Answer 163

From anode to cathode in an outer circuit

Answer 164

∆ G = +ve, ∆ E = 0

Answer 165

∆ G = -ve

Answer 166

∆ G = -ve, ∆ E = 0

Answer 167

∆ G = 0, ∆E = 0

Answer 168

None of these

Answer 169

O₂, SO₂

Answer 170

Generate heat

Answer 171

Remove adsorbed oxygen from electrode surfaces

Answer 172

Produce high purity water

Answer 173

Create potential difference between two electrodes

Answer 174

Loses electrons

Answer 175

Acts as a catalyst

Answer 176

pH is changed

Answer 177

Gains electrons

Answer 178

Solvent particles

Answer 179

Increase in oxidation number of all the elements on reactant side

Answer 180

Both are possible

Answer 181

Increase in oxidation number

Answer 182

Decrease in oxidation number

Answer 183

None of these

Answer 184

Non-spontaneous redox reactions

Answer 185

Spontaneous redox reactions

Answer 186

Spontaneous acid–base reactions

Answer 187

Inversion point

Answer 188

Boiling point

Answer 189

Melting point

Answer 190

Sublimation point

Answer 191

Drops to zero

Answer 192

Does not change

Answer 193

Increases gradually

Answer 194

Increases rapidly

Answer 195

Thomas Gradam

Answer 196

A voltaic cell

Answer 197

A chemical cell

Answer 198

A galvanic cell

Answer 199

An electrolytic cell

Answer 200

760 mm of Hg

Answer 201

Slightly more than 1 atom

Answer 202

Very low ionization potential values

Answer 203

Very high positive value of reduction potential

Answer 204

Very high negative values reduction potential

Answer 205

Reduction potentials are negative

Answer 206

Ohm cm¯¹

Answer 207

Ohm¯¹ cm

Answer 208

Ohm¯¹ cm¯¹

Answer 209

Ohm cm¯²

Answer 210

The entropy of mixing is zero

Answer 211

The free energy of mixing is zero

Answer 212

The enthalpy of mixing is zero

Answer 213

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

Answer 214

31.75 g of Cu

Answer 215

63.5 g of Cu

Answer 216

96500 g of CU

Answer 217

100 g of Cu

Answer 218

58.5g NaCl/100ml

Answer 219

20g NaCl/100ml

Answer 220

10.0g NaCl/100ml

Answer 221

5.58g NaCl/100m

Answer 222

Magnetic energy

Answer 223

Electrical energy

Answer 224

Heat energy

Answer 225

Sound energy

Answer 226

Atoms of Na and Cl.

Answer 227

Free electrons

Answer 228

Free molecules

Answer 229

Chemical energy is converted into heat

Answer 230

Chemical energy is converted into electricity

Answer 231

Electrical energy is converted into chemical energy

Answer 232

Electrical energy is converted into heat

Answer 233

Interaction

Answer 234

Union between two light metals and a heavy metal

Answer 235

Electrochemical phenomenon

Answer 236

Altered reaction in presence of H₂O

Answer 237

The extent of dissolution of solute

Answer 238

The extent of dissociation of solute

Answer 239

The degree of decomposition of solution

Answer 240

Degree of solubilization of solute

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

Electrons flow cathode to anode within the electrolytic solution

Answer 245

1.06 x 10²

Answer 246

1.06 x 10⁴

Answer 247

1.06 x 10³

Answer 248

In metals the ions are free to more

Answer 249

Metals have high resistance

Answer 250

Metals are decomposed by current

Answer 251

They are mobile electrons in the metallic structure

Answer 252

Ionization

Answer 253

Hydrolysis

Answer 254

Supersaturated

Answer 255

Unsaturated

Answer 256

Milligram percent

Answer 257

Gram per million

Answer 258

Microgram percent

Answer 259

Parts per million

Answer 260

Gives ions only when dissolved in water

Answer 261

Gives ions only when electricity is passed

Answer 262

Possesses ions even in solid state

Answer 263

Forms complex ions in solution

Answer 264

Electrolytic cell

Answer 265

Galvanic cell

Answer 266

At cathode

Answer 267

Both A and B

Answer 268

None of these

Answer 269

Decreases with dilution

Answer 270

Depends on mass of electrolyte

Answer 271

Increases with dilution

Answer 272

Remains unchanged with dilution

Answer 273

Drops to zero

Answer 274

Does not change

Answer 275

Decrease rapidly

Answer 276

Decreases slowly

Answer 277

Raoult’s law

Answer 278

Ostwald’s law

Answer 279

Henry’s law

Answer 280

Arrhenius law

Answer 281

Anode to cathode through the external circuit

Answer 282

Cathode to anode through the solution

Answer 283

Anode to cathode through the solution

Answer 284

Cathode to anode through the external circuit

Answer 285

H+ and OH-

Answer 286

Slightly less than one

Answer 287

Slightly greater than one

Answer 288

None of these

Answer 289

Exactly equal to one

Answer 290

Electrochemical equivalent

Answer 291

One gm. atomic weight

Answer 292

None of these

Answer 293

One gm. Equivalent weight

Answer 294

1 – 2 α

Answer 295

None of these

Answer 296

H₄P₃O₇

Answer 297

Electroplating

Answer 298

Conduction

Answer 299

Electrolysis

Answer 300

Hg₂Cl₂

Answer 301

Surface tension

Answer 302

Refractive index

Answer 303

Osmotic pressure

Answer 304

None of these

Answer 305

Both of these

Answer 306

Making iron cathode

Answer 307

Putting it in saline water

Answer 308

Oxidation-reduction

Answer 309

Depends on the nature of the coupled electrode

Answer 310

A reaction in a solution

Answer 311

Electron transfer

Answer 312

Ion combination reaction

Answer 313

Proton transfer

Answer 314

Dilution increases

Answer 315

Pressure increases

Answer 316

Dilution decreases

Answer 317

It has not potential

Answer 318

Distillation

Answer 319

Fractional distillation

Answer 320

Vacuum distillation

Answer 321

None of these

Answer 322

None of these

Answer 323

Molality of the solution

Answer 324

Molarity of the solution

Answer 325

Molarity of the solvent

Answer 326

Mole fraction of the solution

Answer 327

Concentration solutions behave as nearly non – ideal solutions

Answer 328

Neither a nor b

Answer 329

Both a and b

Answer 330

Dilute solution which behave as nearly ideal solution

Answer 331

Salt Bridge

Answer 332

Electric circuit

Answer 333

No connection exists

Answer 334

750 mm of Hg

Answer 335

800 mm of Hg

Answer 336

760 mm of Hg

Answer 337

780 mm of Hg

Answer 338

By removal of solution

Answer 339

By replacing external circuit with external source of electricity

Answer 340

By addition of fresh solution

Answer 341

By heating it

Answer 342

None of these

Answer 343

Hydrolyzed

Answer 344

Precipitated

Answer 345

1.15 g/Cm³

Answer 346

1.2 g/Cm³

Answer 347

1.25g/Cm³

Answer 348

120 g Cm³

Answer 349

None of these

Answer 350

Greater positive value of standard reduction potential

Answer 351

Greater negative value of standard reduction potential

Answer 352

Lesser positive value of standard reduction potential

Answer 353

Hg is more inert than Pt

Answer 354

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

Answer 355

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

Answer 356

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

Answer 357

Not particular

Answer 358

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

Answer 359

All electrochemical reactions involve the transfer of electrons

Answer 360

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

Answer 361

Reduction occurs at cathode

Answer 362

Photo electrolysis

Answer 363

Electrolysis

Answer 364

Cathodic protection

Answer 365

Galvanization

Answer 366

It is readily available

Answer 367

It is volatile

Answer 368

It has a very high cryoscopic constant

Answer 369

It is solvent for organic substances

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