Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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

Equal to the total volume of the components

Answer

None of these

Answer

Slightly less than the total volume of the components

Question 2

2. Wen quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

Answer

Electrochemical equivalent

Answer

None of these

Answer

One gm. Equivalent weight

Answer

One gm. atomic weight

Question 3

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

Answer

Standard reduction potential

Answer

Standard oxidation potential

Answer

Cell voltage

Answer

Ionization potential

Question 4

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

Question 5

5. Corrosion reactions are

Answer

Spontaneous acid–base reactions

Answer

None of these

Answer

Non-spontaneous redox reactions

Answer

Spontaneous redox reactions

Question 6

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

Question 7

7. Maximum freezing point falls in

Answer

Naphthalene

Question 8

8. 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 9

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

Answer

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

Answer

Boiling point of pure water decreases by the addition of ethanol

Answer

Boiling point of pure benzene increases by the addition of toluene

Answer

Vapour pressure of pure benzene decreases by the addition of naphthalene

Question 10

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

Answer

278 S cm² mol¯¹

Answer

176 S cm² mol¯¹

Answer

128 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Question 11

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

Answer

Na₂SO₄

Answer

CH₃ CooNH₄

Question 12

12. 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

1.0 x 10²

Answer

2.0 x 10¹¹

Answer

1.0 x 10¹⁰

Answer

4.0 x 10¹²

Question 13

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

Answer

None of these

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

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

Answer

Electrons flow from cathode to anode through the external battery

Question 14

14. Reduction always occurs

Answer

Both A and B

Answer

At cathode

Answer

None of these

Question 15

15. In a Galvanic cell

Answer

Chemical energy is converted into electricity

Answer

Electrical energy is converted into heat

Answer

Electrical energy is converted into chemical energy

Answer

Chemical energy is converted into heat

Question 16

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

Answer

Unsaturated

Answer

Supersaturated

Question 17

17. 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 18

18. 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 weak base

Answer

Weak acid and its salt of strong base

Answer

A strong acid and its salt of a strong base

Question 19

19. 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 20

20. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 21

21. Stronger the oxidizing agent, greater is the

Answer

Reduction potential

Answer

e.m.f of cell

Answer

Oxidation potential

Answer

Redox potential

Question 22

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

Answer

Electrorefining

Answer

Electroplating

Answer

Both A and B

Answer

None of these

Question 23

23. Pure water does not conduct electricity because it

Answer

Has low boiling point

Answer

Is neutral

Answer

Is readily decomposed

Answer

Is almost unionized

Question 24

24. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 25

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

Answer

Equal to that of water

Answer

Equal to that of ethanol

Answer

More than that of H₂O

Answer

Less than that of water

Question 26

26. The art of electroplating was given by

Answer

Thomas Gradam

Question 27

27. In alkaline battery anode is made up of

Question 28

28. Cathode provides electrons to

Answer

Neutral atom

Answer

Does not provide any electron

Question 29

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

Answer

Osmotic pressure

Answer

Surface tension

Answer

Refractive index

Question 30

30. 50 mL of 10 N H₂SO₄. 25 mL of 12 N HCl and 40 mL of 5N HNO₃ are mixed and the volume of the mixture is made 1000 mL by adding water. The normality of resulting solution will be

Question 31

31. Colligative properties are the properties of

Answer

Neither a nor b

Answer

Concentration solutions behave as nearly non – ideal solutions

Answer

Dilute solution which behave as nearly ideal solution

Answer

Both a and b

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

Answer

Electrolytic cell

Answer

Galvanic cell

Question 34

34. Which has maximum oxidation number

Question 35

35. 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 36

36. Chemical used in salt bridge is

Question 37

37. Calculate the percentage by weight if NaCl, if 2.0 g of NaCl is dissolved in 20g of water

Question 38

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

Question 39

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

Answer

Chemical energy

Answer

Heat energy

Answer

None of these

Answer

Electrical energy

Question 40

40. Oxidation state of hydrogen in CaH₂ is

Question 41

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

Question 42

42. 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 m² mol¯¹

Answer

S² m² mol

Answer

S² m² mol¯²

Answer

S m mol¯¹

Question 43

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

Question 44

44. 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 45

45. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 46

46. The solubility of a gas in water depends upon

Answer

Pressure of the gas

Answer

All of these

Answer

Nature of the gas

Answer

Temperature

Question 47

47. Molarity of water is

Question 48

48. Half cells are interconnected through

Answer

No connection exists

Answer

Salt Bridge

Answer

Electric circuit

Question 49

49. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 50

50. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 51

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

Answer

Both oxidation and reduction

Answer

Neither oxidation and reduction

Question 52

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

Question 53

53. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 54

54. Specific conductivity of a solution

Answer

Depends on mass of electrolyte

Answer

Decreases with dilution

Answer

Increases with dilution

Answer

Remains unchanged with dilution

Question 55

55. 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

Pt and graphite only

Answer

Na and S only

Question 56

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

Question 57

57. In a Galvanic cell, the electrons flow from

Answer

Cathode to anode through the external circuit

Answer

Cathode to anode through the solution

Answer

Anode to cathode through the external circuit

Answer

Anode to cathode through the solution

Question 58

58. Alkaline battery has a voltage of

Question 59

59. 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 60

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

Question 61

61. In electrolytic cell, electricity in carried out by

Answer

Spontaneous reaction

Answer

Non-spontaneous reaction

Answer

Neutralization

Question 62

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

Question 63

63. In alkaline battery the anode is made up of

Question 64

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

Answer

Increases gradually

Answer

Increases rapidly

Answer

Drops to zero

Answer

Does not change

Answer 120

B.P of water remain constant

Answer 121

B.P of water increase

Answer 122

Any possibility

Answer 123

B.P of water decrease

Answer 124

Union between two light metals and a heavy metal

Answer 125

Electrochemical phenomenon

Answer 126

Interaction

Answer 127

Altered reaction in presence of H₂O

Answer 128

Melting point

Answer 129

Inversion point

Answer 130

Boiling point

Answer 131

Sublimation point

Answer 132

0.1 N NaCl

Answer 133

None of these

Answer 134

760 mm of Hg

Answer 135

Slightly more than 1 atom

Answer 136

Neutralization

Answer 137

Rechargeable

Answer 138

Non rechargeable

Answer 139

Electrolytic cell

Answer 140

Daniel cell

Answer 141

Electrolysis

Answer 142

Electroplating

Answer 143

Conduction

Answer 144

They are mobile electrons in the metallic structure

Answer 145

Metals are decomposed by current

Answer 146

Metals have high resistance

Answer 147

In metals the ions are free to more

Answer 148

None of these

Answer 149

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

Answer 150

Reduction occurs at cathode

Answer 151

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

Answer 152

All electrochemical reactions involve the transfer of electrons

Answer 153

Cathodic protection

Answer 154

Photo electrolysis

Answer 155

Galvanization

Answer 156

Electrolysis

Answer 157

Hg₂Cl₂

Answer 158

Gold has higher reduction potential then iron

Answer 159

Iron rusts

Answer 160

Gold is denser

Answer 161

Gold has lower reduction potential then iron

Answer 162

From cathode to anode inside the cell

Answer 163

From cathode to anode in outer circuit

Answer 164

From anode to cathode in an outer circuit

Answer 165

From anode to cathode inside the cell

Answer 166

Br₂ + 2e – → 2Br –

Answer 167

Na → Na⁺ + e–

Answer 168

Na⁺ + e– → Na

Answer 169

2Br– → Br₂ + 2e –

Answer 170

22400 cm³

Answer 171

Exactly equal to one

Answer 172

None of these

Answer 173

Slightly greater than one

Answer 174

Slightly less than one

Answer 175

Precipitated

Answer 176

Hydrolyzed

Answer 177

Molality of the solution

Answer 178

Molarity of the solution

Answer 179

Mole fraction of the solution

Answer 180

Molarity of the solvent

Answer 181

O₂, SO₂

Answer 182

None of these

Answer 183

Hydrolysis

Answer 184

Ionization

Answer 185

None of these

Answer 186

Distillation

Answer 187

Fractional distillation

Answer 188

Vacuum distillation

Answer 189

Raoult’s law

Answer 190

Henry’s law

Answer 191

Ostwald’s law

Answer 192

Arrhenius law

Answer 193

Sound energy

Answer 194

Heat energy

Answer 195

Electrical energy

Answer 196

Magnetic energy

Answer 197

Greater positive value of standard reduction potential

Answer 198

None of these

Answer 199

Greater negative value of standard reduction potential

Answer 200

Lesser positive value of standard reduction potential

Answer 201

Molten NaCl

Answer 202

Pure distilled water

Answer 203

Chloroform

Answer 204

Dilute solution of glucose

Answer 205

All of these

Answer 206

Microgram percent

Answer 207

Gram per million

Answer 208

Milligram percent

Answer 209

Parts per million

Answer 210

– 0.35 V

Answer 211

– 1.17 V

Answer 212

Increases on dilution slightly

Answer 213

Depends on density of electrolyte itself.

Answer 214

Does not change on dilution

Answer 215

Decreases on dilution

Answer 216

It has a very high cryoscopic constant

Answer 217

It is volatile

Answer 218

It is solvent for organic substances

Answer 219

It is readily available

Answer 220

Generate heat

Answer 221

Remove adsorbed oxygen from electrode surfaces

Answer 222

Produce high purity water

Answer 223

Create potential difference between two electrodes

Answer 224

Free molecules

Answer 225

Atoms of Na and Cl.

Answer 226

Free electrons

Answer 227

Electrolytic cell

Answer 228

Daniel cell

Answer 229

Galvanic cell

Answer 230

10.0g NaCl/100ml

Answer 231

5.58g NaCl/100m

Answer 232

20g NaCl/100ml

Answer 233

58.5g NaCl/100ml

Answer 234

The entropy of mixing is zero

Answer 235

The enthalpy of mixing is zero

Answer 236

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

Answer 237

The free energy of mixing is zero

Answer 238

Is oxidized

Answer 239

Gains electrons

Answer 240

Loses electrons

Answer 241

Is hydrolysed

Answer 242

It has not potential

Answer 243

By addition of fresh solution

Answer 244

By replacing external circuit with external source of electricity

Answer 245

By heating it

Answer 246

By removal of solution

Answer 247

Does not change

Answer 248

Drops to zero

Answer 249

Decrease rapidly

Answer 250

Decreases slowly

Answer 251

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

Answer 252

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

Answer 253

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

Answer 254

Li is smaller in size as compared to Cu

Answer 255

H+ and OH-

Answer 256

[Pt(NH₃)₄Cl₃]Cl

Answer 257

[Pt(NH₃)₄Cl]Cl₃

Answer 258

[Pt(NH₃)₄Cl₂]Cl₂

Answer 259

[Pt(NH₃)₄Cl₄]

Answer 260

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

Answer 261

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

Answer 262

Hg is more inert than Pt

Answer 263

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

Answer 264

1.25 cm¯³

Answer 265

1.15 cm¯³

Answer 266

2.15 cm¯³

Answer 267

1.81 cm¯³

Answer 268

A chemical cell

Answer 269

A voltaic cell

Answer 270

An electrolytic cell

Answer 271

A galvanic cell

Answer 272

Degree of solubilization of solute

Answer 273

The extent of dissolution of solute

Answer 274

The degree of decomposition of solution

Answer 275

The extent of dissociation of solute

Answer 276

Ion combination reaction

Answer 277

Proton transfer

Answer 278

Electron transfer

Answer 279

A reaction in a solution

Answer 280

Decrease in oxidation number of element

Answer 281

Increase in oxidation number of the elements in reactants

Answer 282

Increase in oxidation number of element

Answer 283

Oxidation number neither increases nor decreases

Answer 284

Sulphuric acid

Answer 285

Phosphorus acid

Answer 286

Boric acid

Answer 287

Nitric acid

Answer 288

Very low ionization potential values

Answer 289

Reduction potentials are negative

Answer 290

Very high negative values reduction potential

Answer 291

Very high positive value of reduction potential

Answer 292

Not particular

Answer 293

0.142 cm¯¹

Answer 294

0.918 cm¯¹

Answer 295

0.66 cm¯¹

Answer 296

1.12 cm¯¹

Answer 297

Pressure increases

Answer 298

Dilution increases

Answer 299

Dilution decreases

Answer 300

Salt bridge maintains the electrical neutrality of the solution

Answer 301

Cathode is regarded as negative electrode

Answer 302

Electrons are released at anode

Answer 303

Chemical energy is converted into electrical energy

Answer 304

Sum of reduction and oxidation potentials

Answer 305

None of these

Answer 306

Making iron cathode

Answer 307

Putting it in saline water

Answer 308

Both of these

Answer 309

None of these

Answer 310

Electroplating

Answer 311

Rust removal

Answer 312

Manufacture of bleach

Answer 313

Making leather

Answer 314

Acts as a catalyst

Answer 315

Loses electrons

Answer 316

Gains electrons

Answer 317

pH is changed

Answer 318

12157.48 sec

Answer 319

Electric change

Answer 320

Electroplating

Answer 321

Ionization potential

Answer 322

Standard electrode potential

Answer 323

Solvent particles

Answer 324

Both Na⁺ and CI¯

Answer 325

None of these

Answer 326

Depends on the nature of the coupled electrode

Answer 327

Oxidation-reduction

Answer 328

Increase in oxidation number

Answer 329

Both are possible

Answer 330

Increase in oxidation number of all the elements on reactant side

Answer 331

Decrease in oxidation number

Answer 332

Ohm cm¯¹

Answer 333

Ohm cm¯²

Answer 334

Ohm¯¹ cm¯¹

Answer 335

Ohm¯¹ cm

Answer 336

Gives ions only when electricity is passed

Answer 337

Gives ions only when dissolved in water

Answer 338

Possesses ions even in solid state

Answer 339

Forms complex ions in solution

Answer 340

Distribution law

Answer 341

Raoult’s law

Answer 342

Ostwald’s dilution law

Answer 343

Henry’s law

Answer 344

96500 g of CU

Answer 345

100 g of Cu

Answer 346

63.5 g of Cu

Answer 347

31.75 g of Cu

Answer 348

120 g Cm³

Answer 349

1.25g/Cm³

Answer 350

1.15 g/Cm³

Answer 351

1.2 g/Cm³

Answer 352

750 mm of Hg

Answer 353

780 mm of Hg

Answer 354

800 mm of Hg

Answer 355

760 mm of Hg

Answer 356

Elevation in boiling point

Answer 357

Flow of solvent from a concentrated to a dilute solution

Answer 358

Ionic concentration

Answer 359

Diffusion rate of the solute

Answer 360

H₄P₃O₇

Answer 361

0.1 M Glucose

Answer 362

0.1 M BaCl₂

Answer 363

0.1 M Sucrose

Answer 364

0.1 M NaCl

Answer 365

1 – 2 α

Answer 366

1.06 x 10²

Answer 367

1.06 x 10⁴

Answer 368

1.06 x 10³

Answer 369

None of these

Total Questions:	192
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Total Marks:	192
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