Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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 2

2. 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

Reduction potentials are negative

Answer

Very high negative values reduction potential

Answer

Very high positive value of reduction potential

Question 3

3. 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 solution

Answer

Anode to cathode through the external circuit

Question 4

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

Question 5

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 6

6. Prevention of corrosion of iron by Zn coating is called

Answer

Photo electrolysis

Answer

Electrolysis

Answer

Galvanization

Answer

Cathodic protection

Question 7

7. 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 8

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

Answer

Electrical energy

Answer

Magnetic energy

Answer

Sound energy

Answer

Heat energy

Question 9

9. In a chemical reaction, oxidation process involves

Answer

Oxidation number neither increases nor decreases

Answer

Increase in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Answer

Decrease in oxidation number of element

Question 10

10. 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 11

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

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 12

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

Question 13

13. Alkaline battery has a voltage of

Question 14

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

Question 15

15. Temperature for standard electrode potential is

Question 16

16. Pick out the wrong statement. In electrochemical cell

Answer

Cathode is regarded as negative electrode

Answer

Salt bridge maintains the electrical neutrality of the solution

Answer

Chemical energy is converted into electrical energy

Answer

Electrons are released at anode

Question 17

17. Vant Hoff’s factor of Ca(NO₃)₂ is

Question 18

18. The unit of specific conductivity is

Answer

Ohm¯¹ cm

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯¹

Answer

Ohm cm¯²

Question 19

19. Reduction always occurs

Answer

At cathode

Answer

Both A and B

Answer

None of these

Question 20

20. Maximum freezing point falls in

Answer

Naphthalene

Question 21

21. The degree of dissociation of weak electrolyte increases as

Answer

Dilution decreases

Answer

Pressure increases

Answer

Dilution increases

Question 22

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

Answer

∆ G = -ve, ∆ E = 0

Answer

∆ G = 0, ∆E = 0

Answer

∆ G = -ve

Answer

∆ G = +ve, ∆ E = 0

Question 23

23. A redox reaction involves

Answer

Ion combination reaction

Answer

Proton transfer

Answer

Electron transfer

Answer

A reaction in a solution

Question 24

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

Answer

None of these

Answer

Electrons flow from cathode to anode through the external battery

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

Question 25

25. In alkaline battery anode is made up of

Question 26

26. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 27

27. Which of the following statements is FALSE?

Answer

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

Answer

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

Answer

Reduction occurs at cathode

Answer

All electrochemical reactions involve the transfer of electrons

Question 28

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

Question 29

29. If liquids A and B form an ideal solution

Answer

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

Answer

The free energy of mixing is zero

Answer

The entropy of mixing is zero

Answer

The enthalpy of mixing is zero

Question 30

30. The molality of 2% NaCl. W/W solution is approximately

Question 31

31. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

Question 32

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

Question 33

33. 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 34

34. What are the ions present in water?

Answer

H+ and OH-

Question 35

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

Question 36

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

Question 37

37. The number of coulombs required for the deposition of 107.870 g of silver is

Question 38

38. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 39

39. Which has maximum oxidation number

Question 40

40. Decrease in oxidation number is called

Answer

All of these

Question 41

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

Question 42

42. 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 43

43. The reference calomel electrode is made from which of the following?

Answer

Hg₂Cl₂

Question 44

44. The standard EMF of Daniel cell is 1.10 volt. The maximum electrical work obtained from the Daniel cell is

Question 45

45. The strength of solution an element whose electrode potential is to be measured

Question 46

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

Answer

Refractive index

Answer

Surface tension

Answer

Osmotic pressure

Question 47

47. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 48

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

Answer

Electroplating

Answer

Making leather

Answer

Manufacture of bleach

Answer

Rust removal

Question 49

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

Question 50

50. The solubility of a gas in water depends upon

Answer

Temperature

Answer

All of these

Answer

Nature of the gas

Answer

Pressure of the gas

Question 51

51. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

Question 52

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

Answer

O₂, SO₂

Answer

None of these

Question 53

53. Pure water does not conduct electricity because it

Answer

Has low boiling point

Answer

Is almost unionized

Answer

Is readily decomposed

Answer

Is neutral

Question 54

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

Question 55

55. Salt bridge transfers

Question 56

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

Question 57

57. Potential of Zn is called

Answer

It has not potential

Question 58

58. 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 59

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

Question 60

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

Answer

pH is changed

Answer

Loses electrons

Answer

Gains electrons

Answer

Acts as a catalyst

Question 61

61. In a Galvanic cell

Answer

Chemical energy is converted into heat

Answer

Electrical energy is converted into chemical energy

Answer

Electrical energy is converted into heat

Answer

Chemical energy is converted into electricity

Question 62

62. 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

Slightly less than the total volume of the components

Answer

None of these

Answer

Equal to the total volume of the components

Question 63

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

Answer

H₄P₃O₇

Question 64

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

Answer

Drops to zero

Answer

Increases rapidly

Answer

Does not change

Answer

Increases gradually

Answer 105

1.06 x 10⁴

Answer 106

1.06 x 10²

Answer 107

1.06 x 10³

Answer 108

Greater negative value of standard reduction potential

Answer 109

Greater positive value of standard reduction potential

Answer 110

Lesser positive value of standard reduction potential

Answer 111

None of these

Answer 112

Gold has lower reduction potential then iron

Answer 113

Iron rusts

Answer 114

Gold has higher reduction potential then iron

Answer 115

Gold is denser

Answer 116

Equal to that of ethanol

Answer 117

Equal to that of water

Answer 118

More than that of H₂O

Answer 119

Less than that of water

Answer 120

Reduction potential

Answer 121

e.m.f of cell

Answer 122

Redox potential

Answer 123

Oxidation potential

Answer 124

Neither a nor b

Answer 125

Concentration solutions behave as nearly non – ideal solutions

Answer 126

Dilute solution which behave as nearly ideal solution

Answer 127

Both a and b

Answer 128

Spontaneous redox reactions

Answer 129

Spontaneous acid–base reactions

Answer 130

Non-spontaneous redox reactions

Answer 131

None of these

Answer 132

Conduction

Answer 133

Electrolysis

Answer 134

Electroplating

Answer 135

Gives ions only when dissolved in water

Answer 136

Possesses ions even in solid state

Answer 137

Gives ions only when electricity is passed

Answer 138

Forms complex ions in solution

Answer 139

Not particular

Answer 140

Gains electrons

Answer 141

Loses electrons

Answer 142

Is oxidized

Answer 143

Is hydrolysed

Answer 144

Molarity of the solvent

Answer 145

Mole fraction of the solution

Answer 146

Molarity of the solution

Answer 147

Molality of the solution

Answer 148

Precipitated

Answer 149

Hydrolyzed

Answer 150

780 mm of Hg

Answer 151

800 mm of Hg

Answer 152

750 mm of Hg

Answer 153

760 mm of Hg

Answer 154

Diffusion rate of the solute

Answer 155

Ionic concentration

Answer 156

Elevation in boiling point

Answer 157

Flow of solvent from a concentrated to a dilute solution

Answer 158

20g NaCl/100ml

Answer 159

58.5g NaCl/100ml

Answer 160

10.0g NaCl/100ml

Answer 161

5.58g NaCl/100m

Answer 162

Increase in oxidation number of all the elements on reactant side

Answer 163

Both are possible

Answer 164

Decrease in oxidation number

Answer 165

Increase in oxidation number

Answer 166

Na₂SO₄

Answer 167

CH₃ CooNH₄

Answer 168

None of these

Answer 169

None of these

Answer 170

Both Na⁺ and CI¯

Answer 171

Metals are decomposed by current

Answer 172

They are mobile electrons in the metallic structure

Answer 173

Metals have high resistance

Answer 174

In metals the ions are free to more

Answer 175

0.1 M NaCl

Answer 176

0.1 M BaCl₂

Answer 177

0.1 M Glucose

Answer 178

0.1 M Sucrose

Answer 179

Thomas Gradam

Answer 180

Heat energy

Answer 181

Chemical energy

Answer 182

Electrical energy

Answer 183

None of these

Answer 184

Create potential difference between two electrodes

Answer 185

Generate heat

Answer 186

Remove adsorbed oxygen from electrode surfaces

Answer 187

Produce high purity water

Answer 188

None of these

Answer 189

A voltaic cell

Answer 190

A chemical cell

Answer 191

An electrolytic cell

Answer 192

A galvanic cell

Answer 193

Neither oxidation and reduction

Answer 194

Both oxidation and reduction

Answer 195

12157.48 sec

Answer 196

Free electrons

Answer 197

Atoms of Na and Cl.

Answer 198

Free molecules

Answer 199

The extent of dissociation of solute

Answer 200

Degree of solubilization of solute

Answer 201

The degree of decomposition of solution

Answer 202

The extent of dissolution of solute

Answer 203

Solvent particles

Answer 204

Slightly greater than one

Answer 205

Exactly equal to one

Answer 206

None of these

Answer 207

Slightly less than one

Answer 208

Neutral atom

Answer 209

Does not provide any electron

Answer 210

Daniel cell

Answer 211

Non rechargeable

Answer 212

Rechargeable

Answer 213

Electrolytic cell

Answer 214

Drops to zero

Answer 215

Does not change

Answer 216

Decrease rapidly

Answer 217

Decreases slowly

Answer 218

S m mol¯¹

Answer 219

S m² mol¯¹

Answer 220

S² m² mol¯²

Answer 221

S² m² mol

Answer 222

Unsaturated

Answer 223

Supersaturated

Answer 224

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

Answer 225

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

Answer 226

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

Answer 227

Li is smaller in size as compared to Cu

Answer 228

1 – 2 α

Answer 229

176 S cm² mol¯¹

Answer 230

128 S cm² mol¯¹

Answer 231

278 S cm² mol¯¹

Answer 232

302 S cm² mol¯¹

Answer 233

Depends on density of electrolyte itself.

Answer 234

Decreases on dilution

Answer 235

Increases on dilution slightly

Answer 236

Does not change on dilution

Answer 237

By replacing external circuit with external source of electricity

Answer 238

By heating it

Answer 239

By addition of fresh solution

Answer 240

By removal of solution

Answer 241

0.1 N NaCl

Answer 242

Boiling point of pure benzene increases by the addition of toluene

Answer 243

Boiling point of pure water decreases by the addition of ethanol

Answer 244

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 245

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

Answer 246

Na → Na⁺ + e–

Answer 247

Na⁺ + e– → Na

Answer 248

Br₂ + 2e – → 2Br –

Answer 249

2Br– → Br₂ + 2e –

Answer 250

None of these

Answer 251

Microgram percent

Answer 252

Milligram percent

Answer 253

Gram per million

Answer 254

Parts per million

Answer 255

From anode to cathode in an outer circuit

Answer 256

From anode to cathode inside the cell

Answer 257

From cathode to anode in outer circuit

Answer 258

From cathode to anode inside the cell

Answer 259

63.5 g of Cu

Answer 260

100 g of Cu

Answer 261

31.75 g of Cu

Answer 262

96500 g of CU

Answer 263

1.2 g/Cm³

Answer 264

120 g Cm³

Answer 265

1.15 g/Cm³

Answer 266

1.25g/Cm³

Answer 267

None of these

Answer 268

Both A and B

Answer 269

Electrorefining

Answer 270

Electroplating

Answer 271

Pure distilled water

Answer 272

Dilute solution of glucose

Answer 273

Chloroform

Answer 274

Molten NaCl

Answer 275

Neutralization

Answer 276

Interaction

Answer 277

Union between two light metals and a heavy metal

Answer 278

Electrochemical phenomenon

Answer 279

Altered reaction in presence of H₂O

Answer 280

Hydrolysis

Answer 281

Ionization

Answer 282

1.12 cm¯¹

Answer 283

0.66 cm¯¹

Answer 284

0.918 cm¯¹

Answer 285

0.142 cm¯¹

Answer 286

No connection exists

Answer 287

Electric circuit

Answer 288

Salt Bridge

Answer 289

Oxidation-reduction

Answer 290

Depends on the nature of the coupled electrode

Answer 291

Electrochemical equivalent

Answer 292

One gm. Equivalent weight

Answer 293

None of these

Answer 294

One gm. atomic weight

Answer 295

It is solvent for organic substances

Answer 296

It is volatile

Answer 297

It has a very high cryoscopic constant

Answer 298

It is readily available

Answer 299

Increases with dilution

Answer 300

Remains unchanged with dilution

Answer 301

Depends on mass of electrolyte

Answer 302

Decreases with dilution

Answer 303

None of these

Answer 304

Fractional distillation

Answer 305

Distillation

Answer 306

Vacuum distillation

Answer 307

Weak acid and its salt of weak base

Answer 308

A strong acid and its salt of a strong base

Answer 309

Weak acid and its salt of strong base

Answer 310

Strong acid and its salt of weak base

Answer 311

Hg is more inert than Pt

Answer 312

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

Answer 313

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

Answer 314

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

Answer 315

Standard oxidation potential

Answer 316

Ionization potential

Answer 317

Standard reduction potential

Answer 318

Cell voltage

Answer 319

Putting it in saline water

Answer 320

Making iron cathode

Answer 321

None of these

Answer 322

Both of these

Answer 323

None of these

Answer 324

Inversion point

Answer 325

Sublimation point

Answer 326

Melting point

Answer 327

Boiling point

Answer 328

Ionization potential

Answer 329

Electroplating

Answer 330

Electric change

Answer 331

Standard electrode potential

Answer 332

Boric acid

Answer 333

Sulphuric acid

Answer 334

Phosphorus acid

Answer 335

Nitric acid

Answer 336

Galvanic cell

Answer 337

Electrolytic cell

Answer 338

Daniel cell

Answer 339

[Pt(NH₃)₄Cl₂]Cl₂

Answer 340

[Pt(NH₃)₄Cl]Cl₃

Answer 341

[Pt(NH₃)₄Cl₄]

Answer 342

[Pt(NH₃)₄Cl₃]Cl

Answer 343

B.P of water increase

Answer 344

Any possibility

Answer 345

B.P of water remain constant

Answer 346

B.P of water decrease

Answer 347

Raoult’s law

Answer 348

Henry’s law

Answer 349

Arrhenius law

Answer 350

Ostwald’s law

Answer 351

Sufficient date not given

Answer 352

Non-spontaneous reaction

Answer 353

Neutralization

Answer 354

Spontaneous reaction

Answer 355

Henry’s law

Answer 356

Distribution law

Answer 357

Raoult’s law

Answer 358

Ostwald’s dilution law

Answer 359

Electrolytic cell

Answer 360

Galvanic cell

Answer 361

Hg₂Cl₂

Answer 362

1.25 cm¯³

Answer 363

1.81 cm¯³

Answer 364

2.15 cm¯³

Answer 365

1.15 cm¯³

Answer 366

2.0 x 10¹¹

Answer 367

1.0 x 10¹⁰

Answer 368

4.0 x 10¹²

Answer 369

1.0 x 10²

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