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

None of these

Answer

Equal to the total volume of the components

Answer

Slightly less than the total volume of the components

Question 2

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

Answer

0.1 N NaCl

Question 3

3. Best way to prevent rusting iron is by

Answer

Making iron cathode

Answer

None of these

Answer

Putting it in saline water

Answer

Both of these

Question 4

4. 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 5

5. The unit of specific conductivity is

Answer

Ohm¯¹ cm

Answer

Ohm cm¯¹

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯²

Question 6

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

Answer

Rust removal

Answer

Electroplating

Answer

Manufacture of bleach

Answer

Making leather

Question 7

7. The specific conductance of 0.1 M NaCl solution is 1.06 x 10¯² ohm¯¹mol¯¹. Its molar conductance in ohm¯¹ cm² mol¯¹ is

Answer

1.06 x 10²

Answer

1.06 x 10⁴

Answer

1.06 x 10³

Question 8

8. What are the ions present in water?

Answer

H+ and OH-

Question 9

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

Question 10

10. 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 11

11. 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 12

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 13

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

Question 14

14. Half cells are interconnected through

Answer

Salt Bridge

Answer

No connection exists

Answer

Electric circuit

Question 15

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

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 16

16. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 17

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

Answer

20g NaCl/100ml

Answer

58.5g NaCl/100ml

Answer

10.0g NaCl/100ml

Answer

5.58g NaCl/100m

Question 18

18. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 19

19. By means of fuel cells, chemical energy may be converted into

Answer

Magnetic energy

Answer

Electrical energy

Answer

Heat energy

Answer

Sound energy

Question 20

20. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 21

21. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

Question 22

22. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 23

23. Salt bridge transfers

Question 24

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

Answer

Both Na⁺ and CI¯

Answer

None of these

Question 25

25. 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

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer

Boiling point of pure water decreases by the addition of ethanol

Answer

Boiling point of pure benzene increases by the addition of toluene

Question 26

26. 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 27

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

Question 28

28. 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

S m² mol¯¹

Answer

S² m² mol

Answer

S² m² mol¯²

Question 29

29. Standard hydrogen electrode has an arbitrarily fixed potential

Answer

None of these

Question 30

30. Temperature for standard electrode potential is

Question 31

31. Chemical used in salt bridge is

Question 32

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

Answer

Nitric acid

Answer

Phosphorus acid

Answer

Sulphuric acid

Answer

Boric acid

Question 33

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

Question 34

34. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

Answer

None of these

Question 35

35. Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Kf of water 1.86 K mol¯¹ kg and specific gravity of ethylene glycol is 1.11)

Question 36

36. 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 37

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

Answer

Raoult’s law

Answer

Distribution law

Answer

Henry’s law

Answer

Ostwald’s dilution law

Question 38

38. In alkaline battery the anode is made up of

Question 39

39. 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

0.66 cm¯¹

Answer

0.918 cm¯¹

Answer

1.12 cm¯¹

Answer

0.142 cm¯¹

Question 40

40. 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 41

41. The process of electrical coating of one metal on another to protect, decorate or to have a greater resistance to corrosion is called

Answer

Electroplating

Answer

Conduction

Answer

Electrolysis

Question 42

42. Molarity of water is

Question 43

43. Metals usually conduct electricity because

Answer

Metals have high resistance

Answer

In metals the ions are free to more

Answer

They are mobile electrons in the metallic structure

Answer

Metals are decomposed by current

Question 44

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

Answer

Standard oxidation potential

Answer

Standard reduction potential

Answer

Ionization potential

Answer

Cell voltage

Question 45

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

Question 46

46. In an electrolytic cell current flows

Answer

From cathode to anode in outer circuit

Answer

From anode to cathode in an outer circuit

Answer

From cathode to anode inside the cell

Answer

From anode to cathode inside the cell

Question 47

47. In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

Answer

Create potential difference between two electrodes

Answer

Produce high purity water

Answer

Remove adsorbed oxygen from electrode surfaces

Answer

Generate heat

Question 48

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

Question 49

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

Answer

Unsaturated

Answer

Supersaturated

Question 50

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

Question 51

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

Question 52

52. 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 53

53. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 54

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

Answer

Less than that of water

Answer

Equal to that of water

Answer

More than that of H₂O

Answer

Equal to that of ethanol

Question 55

55. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 56

56. 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 57

57. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

Answer

22400 cm³

Question 58

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

Answer

Na⁺ + e– → Na

Answer

Br₂ + 2e – → 2Br –

Answer

2Br– → Br₂ + 2e –

Answer

Na → Na⁺ + e–

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

Answer

Electrons flow from cathode to anode through the external battery

Answer

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

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

None of these

Question 61

61. Maximum freezing point falls in

Answer

Naphthalene

Question 62

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

Question 63

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

Answer

Na₂SO₄

Answer

CH₃ CooNH₄

Question 64

64. Specific conductivity of a solution

Answer

Increases with dilution

Answer

Depends on mass of electrolyte

Answer

Remains unchanged with dilution

Answer

Decreases with dilution

Answer 114

0.1 M NaCl

Answer 115

0.1 M BaCl₂

Answer 116

0.1 M Sucrose

Answer 117

0.1 M Glucose

Answer 118

Both are possible

Answer 119

Increase in oxidation number of all the elements on reactant side

Answer 120

Increase in oxidation number

Answer 121

Decrease in oxidation number

Answer 122

All of these

Answer 123

Electrochemical equivalent

Answer 124

One gm. atomic weight

Answer 125

None of these

Answer 126

One gm. Equivalent weight

Answer 127

B.P of water remain constant

Answer 128

B.P of water increase

Answer 129

Any possibility

Answer 130

B.P of water decrease

Answer 131

Gold has higher reduction potential then iron

Answer 132

Iron rusts

Answer 133

Gold has lower reduction potential then iron

Answer 134

Gold is denser

Answer 135

800 mm of Hg

Answer 136

760 mm of Hg

Answer 137

750 mm of Hg

Answer 138

780 mm of Hg

Answer 139

Chemical energy is converted into heat

Answer 140

Electrical energy is converted into heat

Answer 141

Chemical energy is converted into electricity

Answer 142

Electrical energy is converted into chemical energy

Answer 143

Ca(NO₃)₂

Answer 144

4.0 x 10¹²

Answer 145

1.0 x 10¹⁰

Answer 146

1.0 x 10²

Answer 147

2.0 x 10¹¹

Answer 148

Galvanization

Answer 149

Electrolysis

Answer 150

Photo electrolysis

Answer 151

Cathodic protection

Answer 152

Surface tension

Answer 153

Refractive index

Answer 154

Osmotic pressure

Answer 155

Increase in oxidation number of element

Answer 156

Increase in oxidation number of the elements in reactants

Answer 157

Decrease in oxidation number of element

Answer 158

Oxidation number neither increases nor decreases

Answer 159

Cathode to anode through the external circuit

Answer 160

Anode to cathode through the external circuit

Answer 161

Anode to cathode through the solution

Answer 162

Cathode to anode through the solution

Answer 163

Chemical energy

Answer 164

None of these

Answer 165

Electrical energy

Answer 166

Heat energy

Answer 167

Electrolytic cell

Answer 168

Galvanic cell

Answer 169

Not particular

Answer 170

Slightly less than one

Answer 171

Exactly equal to one

Answer 172

None of these

Answer 173

Slightly greater than one

Answer 174

Depends on the nature of the coupled electrode

Answer 175

Oxidation-reduction

Answer 176

Dilute solution of glucose

Answer 177

Molten NaCl

Answer 178

Chloroform

Answer 179

Pure distilled water

Answer 180

By removal of solution

Answer 181

By heating it

Answer 182

By addition of fresh solution

Answer 183

By replacing external circuit with external source of electricity

Answer 184

Hydrolyzed

Answer 185

Precipitated

Answer 186

Possesses ions even in solid state

Answer 187

Gives ions only when electricity is passed

Answer 188

Forms complex ions in solution

Answer 189

Gives ions only when dissolved in water

Answer 190

[Pt(NH₃)₄Cl₂]Cl₂

Answer 191

[Pt(NH₃)₄Cl]Cl₃

Answer 192

[Pt(NH₃)₄Cl₄]

Answer 193

[Pt(NH₃)₄Cl₃]Cl

Answer 194

Galvanic cell

Answer 195

Daniel cell

Answer 196

Electrolytic cell

Answer 197

Electrorefining

Answer 198

Both A and B

Answer 199

None of these

Answer 200

Electroplating

Answer 201

The enthalpy of mixing is zero

Answer 202

The entropy of mixing is zero

Answer 203

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

Answer 204

The free energy of mixing is zero

Answer 205

Hg₂Cl₂

Answer 206

Neutral atom

Answer 207

Does not provide any electron

Answer 208

Hypertonic

Answer 209

Strong acid and its salt of weak base

Answer 210

A strong acid and its salt of a strong base

Answer 211

Weak acid and its salt of weak base

Answer 212

Weak acid and its salt of strong base

Answer 213

e.m.f of cell

Answer 214

Reduction potential

Answer 215

Oxidation potential

Answer 216

Redox potential

Answer 217

At cathode

Answer 218

Both A and B

Answer 219

None of these

Answer 220

Parts per million

Answer 221

Milligram percent

Answer 222

Microgram percent

Answer 223

Gram per million

Answer 224

Very high negative values reduction potential

Answer 225

Reduction potentials are negative

Answer 226

Very low ionization potential values

Answer 227

Very high positive value of reduction potential

Answer 228

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

Answer 229

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

Answer 230

Hg is more inert than Pt

Answer 231

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

Answer 232

Union between two light metals and a heavy metal

Answer 233

Altered reaction in presence of H₂O

Answer 234

Electrochemical phenomenon

Answer 235

Interaction

Answer 236

Decrease rapidly

Answer 237

Drops to zero

Answer 238

Decreases slowly

Answer 239

Does not change

Answer 240

Neutralization

Answer 241

Daniel cell

Answer 242

Rechargeable

Answer 243

Electrolytic cell

Answer 244

Non rechargeable

Answer 245

Na and S only

Answer 246

Na, Pt and graphite

Answer 247

Pt and graphite only

Answer 248

None of these

Answer 249

Vacuum distillation

Answer 250

Distillation

Answer 251

Fractional distillation

Answer 252

It has not potential

Answer 253

Molarity of the solvent

Answer 254

Molarity of the solution

Answer 255

Molality of the solution

Answer 256

Mole fraction of the solution

Answer 257

Both a and b

Answer 258

Dilute solution which behave as nearly ideal solution

Answer 259

Neither a nor b

Answer 260

Concentration solutions behave as nearly non – ideal solutions

Answer 261

Free electrons

Answer 262

Free molecules

Answer 263

Atoms of Na and Cl.

Answer 264

Standard electrode potential

Answer 265

Electric change

Answer 266

Ionization potential

Answer 267

Electroplating

Answer 268

The degree of decomposition of solution

Answer 269

Degree of solubilization of solute

Answer 270

The extent of dissolution of solute

Answer 271

The extent of dissociation of solute

Answer 272

None of these

Answer 273

Non-spontaneous redox reactions

Answer 274

Spontaneous acid–base reactions

Answer 275

Spontaneous redox reactions

Answer 276

Increases rapidly

Answer 277

Increases gradually

Answer 278

Drops to zero

Answer 279

Does not change

Answer 280

Nature of the gas

Answer 281

All of these

Answer 282

Temperature

Answer 283

Pressure of the gas

Answer 284

120 g Cm³

Answer 285

1.25g/Cm³

Answer 286

1.2 g/Cm³

Answer 287

1.15 g/Cm³

Answer 288

Does not change on dilution

Answer 289

Decreases on dilution

Answer 290

Increases on dilution slightly

Answer 291

Depends on density of electrolyte itself.

Answer 292

Thomas Gradam

Answer 293

None of these

Answer 294

Greater negative value of standard reduction potential

Answer 295

Greater positive value of standard reduction potential

Answer 296

Lesser positive value of standard reduction potential

Answer 297

None of these

Answer 298

O₂, SO₂

Answer 299

A reaction in a solution

Answer 300

Proton transfer

Answer 301

Electron transfer

Answer 302

Ion combination reaction

Answer 303

302 S cm² mol¯¹

Answer 304

278 S cm² mol¯¹

Answer 305

176 S cm² mol¯¹

Answer 306

128 S cm² mol¯¹

Answer 307

Sum of reduction and oxidation potentials

Answer 308

Neutralization

Answer 309

Non-spontaneous reaction

Answer 310

Spontaneous reaction

Answer 311

1 – 2 α

Answer 312

Arrhenius law

Answer 313

Raoult’s law

Answer 314

Henry’s law

Answer 315

Ostwald’s law

Answer 316

Solvent particles

Answer 317

Gains electrons

Answer 318

Loses electrons

Answer 319

Is oxidized

Answer 320

Is hydrolysed

Answer 321

Li is smaller in size as compared to Cu

Answer 322

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

Answer 323

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

Answer 324

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

Answer 325

1.25 cm¯³

Answer 326

1.15 cm¯³

Answer 327

1.81 cm¯³

Answer 328

2.15 cm¯³

Answer 329

Loses electrons

Answer 330

Gains electrons

Answer 331

pH is changed

Answer 332

Acts as a catalyst

Answer 333

100 g of Cu

Answer 334

96500 g of CU

Answer 335

63.5 g of Cu

Answer 336

31.75 g of Cu

Answer 337

It is solvent for organic substances

Answer 338

It is readily available

Answer 339

It has a very high cryoscopic constant

Answer 340

It is volatile

Answer 341

Salt bridge maintains the electrical neutrality of the solution

Answer 342

Chemical energy is converted into electrical energy

Answer 343

Electrons are released at anode

Answer 344

Cathode is regarded as negative electrode

Answer 345

H₄P₃O₇

Answer 346

A chemical cell

Answer 347

A galvanic cell

Answer 348

An electrolytic cell

Answer 349

A voltaic cell

Answer 350

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

Answer 351

Reduction occurs at cathode

Answer 352

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

Answer 353

All electrochemical reactions involve the transfer of electrons

Answer 354

Neither oxidation and reduction

Answer 355

Both oxidation and reduction

Answer 356

Diffusion rate of the solute

Answer 357

Ionic concentration

Answer 358

Elevation in boiling point

Answer 359

Flow of solvent from a concentrated to a dilute solution

Answer 360

12157.48 sec

Answer 361

None of these

Answer 362

Inversion point

Answer 363

Boiling point

Answer 364

Melting point

Answer 365

Sublimation point

Answer 366

None of these

Answer 367

Pressure increases

Answer 368

Dilution increases

Answer 369

Dilution decreases

Total Questions:	192
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Total Marks:	192
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