Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Azeotropic mixture of HCl and water has

Question 2

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

Question 3

3. Electricity in voltaic cell is produced due to

Answer

Neutralization

Question 4

4. 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 10³

Answer

1.06 x 10⁴

Question 5

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

Question 6

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

Question 7

7. 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 8

8. 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 9

9. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 10

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

Question 11

11. 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 12

12. 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 13

13. 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 14

14. The unit of specific conductivity is

Answer

Ohm cm¯¹

Answer

Ohm cm¯²

Answer

Ohm¯¹ cm

Answer

Ohm¯¹ cm¯¹

Question 15

15. Pick out the wrong statement. In electrochemical cell

Answer

Electrons are released at anode

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

Question 16

16. 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 17

17. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

Answer

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

Answer

Hg is more inert than Pt

Answer

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

Answer

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

Question 18

18. Cathode provides electrons to

Answer

Neutral atom

Answer

Does not provide any electron

Question 19

19. 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

Weak acid and its salt of weak base

Answer

A strong acid and its salt of a strong base

Question 20

20. Decrease in oxidation number is called

Answer

All of these

Question 21

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

Answer

Both oxidation and reduction

Answer

Neither oxidation and reduction

Question 22

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

Question 23

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

Answer

Distribution law

Answer

Ostwald’s dilution law

Answer

Henry’s law

Answer

Raoult’s law

Question 24

24. Metals usually conduct electricity because

Answer

In metals the ions are free to more

Answer

They are mobile electrons in the metallic structure

Answer

Metals have high resistance

Answer

Metals are decomposed by current

Question 25

25. Potential of Zn is called

Answer

It has not potential

Question 26

26. Choose the best reducing agent among the following

Question 27

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

Question 28

28. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

Answer

None of these

Answer

Slightly more than the total volume of the components

Answer

Equal to the total volume of the components

Answer

Slightly less than the total volume of the components

Question 29

29. A certain current liberate 0.5 g of hydrogen in 2 h. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

Question 30

30. 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 31

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

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. 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. The depression of freezing point is directly proportional to

Answer

Molarity of the solvent

Answer

Molality of the solution

Answer

Mole fraction of the solution

Answer

Molarity of the solution

Question 35

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

Question 36

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

Answer

Manufacture of bleach

Answer

Electroplating

Answer

Rust removal

Answer

Making leather

Question 37

37. Alkaline battery has a voltage of

Question 38

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

Answer

2Br– → Br₂ + 2e –

Answer

Na → Na⁺ + e–

Answer

Na⁺ + e– → Na

Answer

Br₂ + 2e – → 2Br –

Question 39

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

Question 40

40. Which of the following is the strongest oxidizing agent?

Question 41

41. 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 42

42. When the solute is present in trace quantities the following expression is used?

Answer

Microgram percent

Answer

Milligram percent

Answer

Gram per million

Answer

Parts per million

Question 43

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

Question 44

44. 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

S² m² mol¯²

Answer

S m² mol¯¹

Question 45

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

Answer

Heat energy

Answer

Magnetic energy

Answer

Electrical energy

Answer

Sound energy

Question 46

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

Answer

Ionization potential

Answer

Standard reduction potential

Answer

Cell voltage

Answer

Standard oxidation potential

Question 47

47. Secondary cell is

Answer

Daniel cell

Answer

Electrolytic cell

Answer

Non rechargeable

Answer

Rechargeable

Question 48

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

Answer

Not particular

Question 49

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

Answer

Create potential difference between two electrodes

Answer

Remove adsorbed oxygen from electrode surfaces

Answer

Produce high purity water

Answer

Generate heat

Question 50

50. 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

Very high positive value of reduction potential

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Question 51

51. 96500 C of electricity liberates from CuSO₄ solution

Answer

96500 g of CU

Answer

31.75 g of Cu

Answer

100 g of Cu

Answer

63.5 g of Cu

Question 52

52. 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 53

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

Answer

– 0.35 V

Answer

– 1.17 V

Question 54

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

Answer

Li is smaller in size as compared to Cu

Answer

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

Answer

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

Answer

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

Question 55

55. Density of H₂SO₄ in lead accumulator is

Question 56

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

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. Which has maximum oxidation number

Question 59

59. 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 enthalpy of mixing is zero

Answer

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

Question 60

60. 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

None of these

Answer

One gm. Equivalent weight

Question 61

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

Answer

Iron rusts

Answer

Gold has lower reduction potential then iron

Answer

Gold has higher reduction potential then iron

Answer

Gold is denser

Question 62

62. Maximum freezing point falls in

Answer

Naphthalene

Question 63

63. 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 64

64. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Answer 114

None of these

Answer 115

Forms complex ions in solution

Answer 116

Gives ions only when electricity is passed

Answer 117

Gives ions only when dissolved in water

Answer 118

Possesses ions even in solid state

Answer 119

0.1 M Glucose

Answer 120

0.1 M NaCl

Answer 121

0.1 M BaCl₂

Answer 122

0.1 M Sucrose

Answer 123

1.15 cm¯³

Answer 124

1.81 cm¯³

Answer 125

2.15 cm¯³

Answer 126

1.25 cm¯³

Answer 127

Electric circuit

Answer 128

No connection exists

Answer 129

Salt Bridge

Answer 130

Solvent particles

Answer 131

∆ G = 0, ∆E = 0

Answer 132

∆ G = -ve, ∆ E = 0

Answer 133

∆ G = +ve, ∆ E = 0

Answer 134

∆ G = -ve

Answer 135

The degree of decomposition of solution

Answer 136

The extent of dissolution of solute

Answer 137

Degree of solubilization of solute

Answer 138

The extent of dissociation of solute

Answer 139

1.12 cm¯¹

Answer 140

0.66 cm¯¹

Answer 141

0.142 cm¯¹

Answer 142

0.918 cm¯¹

Answer 143

A galvanic cell

Answer 144

An electrolytic cell

Answer 145

A chemical cell

Answer 146

A voltaic cell

Answer 147

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

Answer 148

None of these

Answer 149

Electrons flow cathode to anode within the electrolytic solution

Answer 150

Electrons flow from cathode to anode through the external battery

Answer 151

B.P of water remain constant

Answer 152

B.P of water decrease

Answer 153

Any possibility

Answer 154

B.P of water increase

Answer 155

None of these

Answer 156

Thomas Gradam

Answer 157

Acts as a catalyst

Answer 158

Gains electrons

Answer 159

Loses electrons

Answer 160

pH is changed

Answer 161

Increase in oxidation number

Answer 162

Both are possible

Answer 163

Increase in oxidation number of all the elements on reactant side

Answer 164

Decrease in oxidation number

Answer 165

Decrease rapidly

Answer 166

Drops to zero

Answer 167

Does not change

Answer 168

Decreases slowly

Answer 169

Cathode to anode through the solution

Answer 170

Anode to cathode through the external circuit

Answer 171

Cathode to anode through the external circuit

Answer 172

Anode to cathode through the solution

Answer 173

1 – 2 α

Answer 174

Na₂SO₄

Answer 175

CH₃ CooNH₄

Answer 176

Gains electrons

Answer 177

Is oxidized

Answer 178

Loses electrons

Answer 179

Is hydrolysed

Answer 180

Equal to that of water

Answer 181

Less than that of water

Answer 182

More than that of H₂O

Answer 183

Equal to that of ethanol

Answer 184

Precipitated

Answer 185

Hydrolyzed

Answer 186

Decrease in oxidation number of element

Answer 187

Oxidation number neither increases nor decreases

Answer 188

Increase in oxidation number of the elements in reactants

Answer 189

Increase in oxidation number of element

Answer 190

1.15 g/Cm³

Answer 191

1.25g/Cm³

Answer 192

1.2 g/Cm³

Answer 193

120 g Cm³

Answer 194

Dilute solution of glucose

Answer 195

Chloroform

Answer 196

Pure distilled water

Answer 197

Molten NaCl

Answer 198

Reduction occurs at cathode

Answer 199

All electrochemical reactions involve the transfer of electrons

Answer 200

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

Answer 201

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

Answer 202

Dilute solution which behave as nearly ideal solution

Answer 203

Neither a nor b

Answer 204

Concentration solutions behave as nearly non – ideal solutions

Answer 205

Both a and b

Answer 206

Chemical energy is converted into heat

Answer 207

Chemical energy is converted into electricity

Answer 208

Electrical energy is converted into chemical energy

Answer 209

Electrical energy is converted into heat

Answer 210

Refractive index

Answer 211

Osmotic pressure

Answer 212

Surface tension

Answer 213

Decreases on dilution

Answer 214

Depends on density of electrolyte itself.

Answer 215

Increases on dilution slightly

Answer 216

Does not change on dilution

Answer 217

It has a very high cryoscopic constant

Answer 218

It is readily available

Answer 219

It is volatile

Answer 220

It is solvent for organic substances

Answer 221

0.1 N NaCl

Answer 222

Free molecules

Answer 223

Free electrons

Answer 224

Atoms of Na and Cl.

Answer 225

Pressure of the gas

Answer 226

All of these

Answer 227

Nature of the gas

Answer 228

Temperature

Answer 229

760 mm of Hg

Answer 230

Slightly more than 1 atom

Answer 231

Slightly greater than one

Answer 232

Exactly equal to one

Answer 233

Slightly less than one

Answer 234

None of these

Answer 235

Hypertonic

Answer 236

Increases with dilution

Answer 237

Remains unchanged with dilution

Answer 238

Depends on mass of electrolyte

Answer 239

Decreases with dilution

Answer 240

Greater negative value of standard reduction potential

Answer 241

Lesser positive value of standard reduction potential

Answer 242

Greater positive value of standard reduction potential

Answer 243

None of these

Answer 244

Galvanization

Answer 245

Cathodic protection

Answer 246

Photo electrolysis

Answer 247

Electrolysis

Answer 248

Vacuum distillation

Answer 249

Fractional distillation

Answer 250

Distillation

Answer 251

None of these

Answer 252

Phosphorus acid

Answer 253

Boric acid

Answer 254

Nitric acid

Answer 255

Sulphuric acid

Answer 256

Electrolytic cell

Answer 257

Galvanic cell

Answer 258

Drops to zero

Answer 259

Increases gradually

Answer 260

Does not change

Answer 261

Increases rapidly

Answer 262

None of these

Answer 263

Both A and B

Answer 264

At cathode

Answer 265

12157.48 sec

Answer 266

Ionization potential

Answer 267

Electric change

Answer 268

Electroplating

Answer 269

Standard electrode potential

Answer 270

None of these

Answer 271

Pressure increases

Answer 272

Dilution increases

Answer 273

Dilution decreases

Answer 274

Diffusion rate of the solute

Answer 275

Ionic concentration

Answer 276

Elevation in boiling point

Answer 277

Flow of solvent from a concentrated to a dilute solution

Answer 278

Depends on the nature of the coupled electrode

Answer 279

Oxidation-reduction

Answer 280

H₄P₃O₇

Answer 281

Ostwald’s law

Answer 282

Henry’s law

Answer 283

Arrhenius law

Answer 284

Raoult’s law

Answer 285

Melting point

Answer 286

Inversion point

Answer 287

Boiling point

Answer 288

Sublimation point

Answer 289

Non-spontaneous redox reactions

Answer 290

Spontaneous redox reactions

Answer 291

Spontaneous acid–base reactions

Answer 292

None of these

Answer 293

Is neutral

Answer 294

Has low boiling point

Answer 295

Is readily decomposed

Answer 296

Is almost unionized

Answer 297

[Pt(NH₃)₄Cl]Cl₃

Answer 298

[Pt(NH₃)₄Cl₄]

Answer 299

[Pt(NH₃)₄Cl₂]Cl₂

Answer 300

[Pt(NH₃)₄Cl₃]Cl

Answer 301

None of these

Answer 302

Making iron cathode

Answer 303

Both of these

Answer 304

Putting it in saline water

Answer 305

Hg₂Cl₂

Answer 306

176 S cm² mol¯¹

Answer 307

302 S cm² mol¯¹

Answer 308

278 S cm² mol¯¹

Answer 309

128 S cm² mol¯¹

Answer 310

2.0 x 10¹¹

Answer 311

1.0 x 10²

Answer 312

1.0 x 10¹⁰

Answer 313

4.0 x 10¹²

Answer 314

O₂, SO₂

Answer 315

None of these

Answer 316

Non-spontaneous reaction

Answer 317

Spontaneous reaction

Answer 318

Neutralization

Answer 319

Supersaturated

Answer 320

Unsaturated

Answer 321

Ca(NO₃)₂

Answer 322

Daniel cell

Answer 323

Electrolytic cell

Answer 324

Galvanic cell

Answer 325

800 mm of Hg

Answer 326

750 mm of Hg

Answer 327

760 mm of Hg

Answer 328

780 mm of Hg

Answer 329

From cathode to anode inside the cell

Answer 330

From cathode to anode in outer circuit

Answer 331

From anode to cathode inside the cell

Answer 332

From anode to cathode in an outer circuit

Answer 333

None of these

Answer 334

Electrorefining

Answer 335

Electroplating

Answer 336

Both A and B

Answer 337

Ionization

Answer 338

Hydrolysis

Answer 339

By replacing external circuit with external source of electricity

Answer 340

By heating it

Answer 341

By addition of fresh solution

Answer 342

By removal of solution

Answer 343

Boiling point of pure benzene increases by the addition of toluene

Answer 344

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

Answer 345

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 346

Boiling point of pure water decreases by the addition of ethanol

Answer 347

Na, Pt and graphite

Answer 348

Pt and graphite only

Answer 349

Na and S only

Answer 350

Sufficient date not given

Answer 351

Altered reaction in presence of H₂O

Answer 352

Electrochemical phenomenon

Answer 353

Union between two light metals and a heavy metal

Answer 354

Interaction

Answer 355

Oxidation potential

Answer 356

Redox potential

Answer 357

Reduction potential

Answer 358

e.m.f of cell

Answer 359

None of these

Answer 360

Both Na⁺ and CI¯

Answer 361

H+ and OH-

Answer 362

58.5g NaCl/100ml

Answer 363

10.0g NaCl/100ml

Answer 364

20g NaCl/100ml

Answer 365

5.58g NaCl/100m

Answer 366

A reaction in a solution

Answer 367

Electron transfer

Answer 368

Ion combination reaction

Answer 369

Proton transfer

Total Questions:	192
Time Allowed:	60 Minutes
Total Marks:	192
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Chemistry Electro Chemistry Online Mcqs Test

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