Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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 2

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

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 3

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

Answer

Magnetic energy

Answer

Sound energy

Answer

Electrical energy

Answer

Heat energy

Question 4

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

Answer

Chloroform

Answer

Molten NaCl

Answer

Dilute solution of glucose

Answer

Pure distilled water

Question 5

5. Mole fraction of pure water is

Answer

Exactly equal to one

Answer

Slightly less than one

Answer

None of these

Answer

Slightly greater than one

Question 6

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

Answer

Equal to that of water

Answer

Less than that of water

Answer

More than that of H₂O

Answer

Equal to that of ethanol

Question 7

7. An electrolyte

Answer

Possesses ions even in solid state

Answer

Forms complex ions in solution

Answer

Gives ions only when dissolved in water

Answer

Gives ions only when electricity is passed

Question 8

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

Question 9

9. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 10

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

Question 11

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

Answer

Hg₂Cl₂

Question 12

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

Question 13

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

Answer

Neither oxidation and reduction

Answer

Both oxidation and reduction

Question 14

14. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 15

15. In a chemical reaction, oxidation process involves

Answer

Decrease in oxidation number of element

Answer

Increase in oxidation number of element

Answer

Increase in oxidation number of the elements in reactants

Answer

Oxidation number neither increases nor decreases

Question 16

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

Answer

Vacuum distillation

Answer

Fractional distillation

Answer

Distillation

Answer

None of these

Question 17

17. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 18

18. Specific conductivity of a solution

Answer

Remains unchanged with dilution

Answer

Increases with dilution

Answer

Decreases with dilution

Answer

Depends on mass of electrolyte

Question 19

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

Answer

Electrolytic cell

Answer

Galvanic cell

Answer

Daniel cell

Question 20

20. A device which converts electrical energy into chemical energy is called

Answer

A galvanic cell

Answer

A voltaic cell

Answer

An electrolytic cell

Answer

A chemical cell

Question 21

21. Molarity of water is

Question 22

22. A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If Kf for water is 1.80, the correct formulation for the above molecule is

Answer

[Pt(NH₃)₄Cl₃]Cl

Answer

[Pt(NH₃)₄Cl₂]Cl₂

Answer

[Pt(NH₃)₄Cl]Cl₃

Answer

[Pt(NH₃)₄Cl₄]

Question 23

23. Temperature for standard electrode potential is

Question 24

24. Decrease in oxidation number is called

Answer

All of these

Question 25

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

Question 26

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

Question 27

27. Salt bridge transfers

Answer

Solvent particles

Question 28

28. 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

4.0 x 10¹²

Answer

2.0 x 10¹¹

Answer

1.0 x 10¹⁰

Question 29

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

Question 30

30. Anode electrode element always have _________ position in electrochemical series

Answer

Not particular

Question 31

31. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 32

32. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

Question 33

33. Density of H₂SO₄ in lead accumulator is

Answer

1.15 g/Cm³

Answer

1.25g/Cm³

Answer

1.2 g/Cm³

Answer

120 g Cm³

Question 34

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

Answer

One gm. atomic weight

Answer

Electrochemical equivalent

Answer

One gm. Equivalent weight

Answer

None of these

Question 35

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

Question 36

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

Question 37

37. Potential of Zn is called

Answer

It has not potential

Question 38

38. 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 high positive value of reduction potential

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Answer

Very low ionization potential values

Question 39

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

Answer

1.25 cm¯³

Answer

1.15 cm¯³

Answer

2.15 cm¯³

Answer

1.81 cm¯³

Question 40

40. A dry alkaline cell has porous Zn anode & MnO₂ as cathode the electrolyte used is

Question 41

41. If liquids A and B form an ideal solution

Answer

The entropy of mixing is zero

Answer

The free energy of mixing is zero

Answer

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

Answer

The enthalpy of mixing is zero

Question 42

42. Pick out the wrong statement. In electrochemical cell

Answer

Electrons are released at anode

Answer

Cathode is regarded as negative electrode

Answer

Chemical energy is converted into electrical energy

Answer

Salt bridge maintains the electrical neutrality of the solution

Question 43

43. Chemical used in salt bridge is

Question 44

44. The depression of freezing point is directly proportional to

Answer

Molarity of the solution

Answer

Mole fraction of the solution

Answer

Molality of the solution

Answer

Molarity of the solvent

Question 45

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

Answer

Create potential difference between two electrodes

Answer

Produce high purity water

Answer

Generate heat

Answer

Remove adsorbed oxygen from electrode surfaces

Question 46

46. Electrode potential of Zn is

Answer

Depends on the nature of the coupled electrode

Answer

Oxidation-reduction

Question 47

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

Question 48

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

Answer

None of these

Question 49

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

Question 50

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

Answer

Supersaturated

Answer

Unsaturated

Question 51

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

Question 52

52. 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 53

53. Camphor is often used in molecular mass determination because

Answer

It is volatile

Answer

It has a very high cryoscopic constant

Answer

It is solvent for organic substances

Answer

It is readily available

Question 54

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

Answer

CH₃ CooNH₄

Answer

Na₂SO₄

Question 55

55. Oxidation state of hydrogen in CaH₂ is

Question 56

56. 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 57

57. The Vant Hoff factor (i) accounts for

Answer

The extent of dissolution of solute

Answer

The extent of dissociation of solute

Answer

Degree of solubilization of solute

Answer

The degree of decomposition of solution

Question 58

58. Salt bridge transfers

Question 59

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

Answer

Electrical energy

Answer

None of these

Answer

Heat energy

Answer

Chemical energy

Question 60

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 61

61. Units of molarity are

Answer

None of these

Question 62

62. Colligative properties are the properties of

Answer

Both a and b

Answer

Concentration solutions behave as nearly non – ideal solutions

Answer

Neither a nor b

Answer

Dilute solution which behave as nearly ideal solution

Question 63

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

Answer

Acts as a catalyst

Answer

Gains electrons

Answer

Loses electrons

Answer

pH is changed

Question 64

64. 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

Answer 122

Equal to the total volume of the components

Answer 123

Slightly more than the total volume of the components

Answer 124

None of these

Answer 125

Slightly less than the total volume of the components

Answer 126

Boiling point of pure water decreases by the addition of ethanol

Answer 127

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 128

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

Answer 129

Boiling point of pure benzene increases by the addition of toluene

Answer 130

12157.48 sec

Answer 131

Sufficient date not given

Answer 132

Interaction

Answer 133

Union between two light metals and a heavy metal

Answer 134

Electrochemical phenomenon

Answer 135

Altered reaction in presence of H₂O

Answer 136

None of these

Answer 137

O₂, SO₂

Answer 138

None of these

Answer 139

Both are possible

Answer 140

Decrease in oxidation number

Answer 141

Increase in oxidation number

Answer 142

Increase in oxidation number of all the elements on reactant side

Answer 143

Parts per million

Answer 144

Gram per million

Answer 145

Microgram percent

Answer 146

Milligram percent

Answer 147

Chemical energy is converted into heat

Answer 148

Chemical energy is converted into electricity

Answer 149

Electrical energy is converted into chemical energy

Answer 150

Electrical energy is converted into heat

Answer 151

Hydrolyzed

Answer 152

Precipitated

Answer 153

Sum of reduction and oxidation potentials

Answer 154

Refractive index

Answer 155

Osmotic pressure

Answer 156

Surface tension

Answer 157

Does not change

Answer 158

Decrease rapidly

Answer 159

Drops to zero

Answer 160

Decreases slowly

Answer 161

Does not provide any electron

Answer 162

Neutral atom

Answer 163

Increases gradually

Answer 164

Does not change

Answer 165

Drops to zero

Answer 166

Increases rapidly

Answer 167

Cathode to anode through the solution

Answer 168

Anode to cathode through the solution

Answer 169

Cathode to anode through the external circuit

Answer 170

Anode to cathode through the external circuit

Answer 171

Ohm¯¹ cm

Answer 172

Ohm cm¯¹

Answer 173

Ohm¯¹ cm¯¹

Answer 174

Ohm cm¯²

Answer 175

Electrolysis

Answer 176

Galvanization

Answer 177

Cathodic protection

Answer 178

Photo electrolysis

Answer 179

Conduction

Answer 180

Electrolysis

Answer 181

Electroplating

Answer 182

Br₂ + 2e – → 2Br –

Answer 183

2Br– → Br₂ + 2e –

Answer 184

Na → Na⁺ + e–

Answer 185

Na⁺ + e– → Na

Answer 186

Pressure increases

Answer 187

Dilution increases

Answer 188

Dilution decreases

Answer 189

Henry’s law

Answer 190

Distribution law

Answer 191

Ostwald’s dilution law

Answer 192

Raoult’s law

Answer 193

Lesser positive value of standard reduction potential

Answer 194

Greater positive value of standard reduction potential

Answer 195

Greater negative value of standard reduction potential

Answer 196

None of these

Answer 197

None of these

Answer 198

Spontaneous redox reactions

Answer 199

Non-spontaneous redox reactions

Answer 200

Spontaneous acid–base reactions

Answer 201

Nature of the gas

Answer 202

Pressure of the gas

Answer 203

All of these

Answer 204

Temperature

Answer 205

Non-spontaneous reaction

Answer 206

Spontaneous reaction

Answer 207

Neutralization

Answer 208

Is almost unionized

Answer 209

Is readily decomposed

Answer 210

Has low boiling point

Answer 211

Is neutral

Answer 212

None of these

Answer 213

Electroplating

Answer 214

Both A and B

Answer 215

Electrorefining

Answer 216

Thomas Gradam

Answer 217

Boric acid

Answer 218

Sulphuric acid

Answer 219

Phosphorus acid

Answer 220

Nitric acid

Answer 221

176 S cm² mol¯¹

Answer 222

302 S cm² mol¯¹

Answer 223

128 S cm² mol¯¹

Answer 224

278 S cm² mol¯¹

Answer 225

By addition of fresh solution

Answer 226

By replacing external circuit with external source of electricity

Answer 227

By heating it

Answer 228

By removal of solution

Answer 229

Metals are decomposed by current

Answer 230

In metals the ions are free to more

Answer 231

Metals have high resistance

Answer 232

They are mobile electrons in the metallic structure

Answer 233

Weak acid and its salt of weak base

Answer 234

Weak acid and its salt of strong base

Answer 235

Strong acid and its salt of weak base

Answer 236

A strong acid and its salt of a strong base

Answer 237

Electrolytic cell

Answer 238

Rechargeable

Answer 239

Daniel cell

Answer 240

Non rechargeable

Answer 241

Decreases on dilution

Answer 242

Does not change on dilution

Answer 243

Depends on density of electrolyte itself.

Answer 244

Increases on dilution slightly

Answer 245

Ca(NO₃)₂

Answer 246

Both A and B

Answer 247

At cathode

Answer 248

None of these

Answer 249

S m mol¯¹

Answer 250

S m² mol¯¹

Answer 251

S² m² mol

Answer 252

S² m² mol¯²

Answer 253

0.1 N NaCl

Answer 254

Electric change

Answer 255

Ionization potential

Answer 256

Electroplating

Answer 257

Standard electrode potential

Answer 258

Rust removal

Answer 259

Making leather

Answer 260

Electroplating

Answer 261

Manufacture of bleach

Answer 262

Na and S only

Answer 263

Na, Pt and graphite

Answer 264

Pt and graphite only

Answer 265

760 mm of Hg

Answer 266

800 mm of Hg

Answer 267

750 mm of Hg

Answer 268

780 mm of Hg

Answer 269

Hg₂Cl₂

Answer 270

H₄P₃O₇

Answer 271

5.58g NaCl/100m

Answer 272

58.5g NaCl/100ml

Answer 273

10.0g NaCl/100ml

Answer 274

20g NaCl/100ml

Answer 275

B.P of water remain constant

Answer 276

B.P of water increase

Answer 277

B.P of water decrease

Answer 278

Any possibility

Answer 279

Salt Bridge

Answer 280

Electric circuit

Answer 281

No connection exists

Answer 282

Naphthalene

Answer 283

Cell voltage

Answer 284

Standard oxidation potential

Answer 285

Ionization potential

Answer 286

Standard reduction potential

Answer 287

Both of these

Answer 288

None of these

Answer 289

Putting it in saline water

Answer 290

Making iron cathode

Answer 291

Is hydrolysed

Answer 292

Is oxidized

Answer 293

Gains electrons

Answer 294

Loses electrons

Answer 295

Gold has higher reduction potential then iron

Answer 296

Gold is denser

Answer 297

Gold has lower reduction potential then iron

Answer 298

Iron rusts

Answer 299

H+ and OH-

Answer 300

1 – 2 α

Answer 301

100 g of Cu

Answer 302

63.5 g of Cu

Answer 303

31.75 g of Cu

Answer 304

96500 g of CU

Answer 305

From anode to cathode inside the cell

Answer 306

From cathode to anode in outer circuit

Answer 307

From anode to cathode in an outer circuit

Answer 308

From cathode to anode inside the cell

Answer 309

∆ G = 0, ∆E = 0

Answer 310

∆ G = -ve, ∆ E = 0

Answer 311

∆ G = +ve, ∆ E = 0

Answer 312

∆ G = -ve

Answer 313

A reaction in a solution

Answer 314

Ion combination reaction

Answer 315

Electron transfer

Answer 316

Proton transfer

Answer 317

Sublimation point

Answer 318

Boiling point

Answer 319

Inversion point

Answer 320

Melting point

Answer 321

1.12 cm¯¹

Answer 322

0.66 cm¯¹

Answer 323

0.918 cm¯¹

Answer 324

0.142 cm¯¹

Answer 325

0.1 M Sucrose

Answer 326

0.1 M BaCl₂

Answer 327

0.1 M Glucose

Answer 328

0.1 M NaCl

Answer 329

Ionization

Answer 330

Hydrolysis

Answer 331

All electrochemical reactions involve the transfer of electrons

Answer 332

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

Answer 333

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

Answer 334

Reduction occurs at cathode

Answer 335

None of these

Answer 336

Electrons flow cathode to anode within the electrolytic solution

Answer 337

Electrons flow from cathode to anode through the external battery

Answer 338

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

Answer 339

Redox potential

Answer 340

Reduction potential

Answer 341

e.m.f of cell

Answer 342

Oxidation potential

Answer 343

Galvanic cell

Answer 344

Electrolytic cell

Answer 345

Henry’s law

Answer 346

Ostwald’s law

Answer 347

Arrhenius law

Answer 348

Raoult’s law

Answer 349

1.06 x 10²

Answer 350

1.06 x 10³

Answer 351

1.06 x 10⁴

Answer 352

Both Na⁺ and CI¯

Answer 353

None of these

Answer 354

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

Answer 355

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

Answer 356

Hg is more inert than Pt

Answer 357

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

Answer 358

Free molecules

Answer 359

Free electrons

Answer 360

Atoms of Na and Cl.

Answer 361

Ionic concentration

Answer 362

Diffusion rate of the solute

Answer 363

Elevation in boiling point

Answer 364

Flow of solvent from a concentrated to a dilute solution

Answer 365

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

Answer 366

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

Answer 367

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

Answer 368

Li is smaller in size as compared to Cu

Answer 369

None of these

Total Questions:	192
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Total Marks:	192
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