Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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 2

2. Units of molarity are

Answer

None of these

Question 3

3. The reference electrode is made by using

Answer

Hg₂Cl₂

Question 4

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

Answer

– 1.17 V

Answer

– 0.35 V

Question 5

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

Answer

Iron rusts

Answer

Gold is denser

Answer

Gold has lower reduction potential then iron

Answer

Gold has higher reduction potential then iron

Question 6

6. Best way to prevent rusting iron is by

Answer

Making iron cathode

Answer

Both of these

Answer

None of these

Answer

Putting it in saline water

Question 7

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

Answer

None of these

Answer

Both Na⁺ and CI¯

Question 8

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

Answer

Gains electrons

Answer

Acts as a catalyst

Answer

Loses electrons

Answer

pH is changed

Question 9

9. A redox reaction involves

Answer

Ion combination reaction

Answer

Electron transfer

Answer

A reaction in a solution

Answer

Proton transfer

Question 10

10. Voltaic cell can be recharged by

Answer

By addition of fresh solution

Answer

By removal of solution

Answer

By heating it

Answer

By replacing external circuit with external source of electricity

Question 11

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

Question 12

12. 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 13

13. Which substances are mixed to form a buffer solution?

Answer

A strong acid and its salt of a strong base

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

Question 14

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

Answer

Increases gradually

Answer

Drops to zero

Answer

Does not change

Answer

Increases rapidly

Question 15

15. Half cells are interconnected through

Answer

No connection exists

Answer

Salt Bridge

Answer

Electric circuit

Question 16

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

Question 17

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

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

None of these

Answer

Electrons flow from cathode to anode through the external battery

Question 18

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

Question 19

19. 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 20

20. Secondary cell is

Answer

Non rechargeable

Answer

Rechargeable

Answer

Electrolytic cell

Answer

Daniel cell

Question 21

21. 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 22

22. The art of electroplating was given by

Answer

Thomas Gradam

Question 23

23. Oxidation number of carbon in NaHCO₃ is

Question 24

24. 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 25

25. In alkaline battery anode is made up of

Question 26

26. Alkaline battery has a voltage of

Question 27

27. 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 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

S² m² mol¯²

Answer

S² m² mol

Answer

S m² mol¯¹

Answer

S m mol¯¹

Question 29

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

Answer

Unsaturated

Answer

Supersaturated

Question 30

30. In an electrolytic cell current flows

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

Answer

From cathode to anode in outer circuit

Question 31

31. Electrode potential of Zn is

Answer

Oxidation-reduction

Answer

Depends on the nature of the coupled electrode

Question 32

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

Question 33

33. 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)₄Cl₂]Cl₂

Answer

[Pt(NH₃)₄Cl₃]Cl

Answer

[Pt(NH₃)₄Cl₄]

Answer

[Pt(NH₃)₄Cl]Cl₃

Question 34

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

Question 35

35. Which of the following is a strong electrolyte?

Answer

Ca(NO₃)₂

Question 36

36. Strong reducing agents have

Answer

Lesser positive value of standard reduction potential

Answer

None of these

Answer

Greater positive value of standard reduction potential

Answer

Greater negative value of standard reduction potential

Question 37

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

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 38

38. 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 39

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

Answer

Osmotic pressure

Answer

Refractive index

Answer

Surface tension

Question 40

40. Camphor is often used in molecular mass determination because

Answer

It is readily available

Answer

It is volatile

Answer

It has a very high cryoscopic constant

Answer

It is solvent for organic substances

Question 41

41. In alkaline battery the anode is made up of

Question 42

42. Salt bridge transfers

Answer

Solvent particles

Question 43

43. Corrosion reactions are

Answer

Non-spontaneous redox reactions

Answer

Spontaneous acid–base reactions

Answer

None of these

Answer

Spontaneous redox reactions

Question 44

44. 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 45

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

Question 46

46. Maximum freezing point falls in

Answer

Naphthalene

Question 47

47. Temperature for standard electrode potential is

Question 48

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

Question 49

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

Question 50

50. Choose the best reducing agent among the following

Question 51

51. Corrosion is basically a

Answer

Union between two light metals and a heavy metal

Answer

Interaction

Answer

Electrochemical phenomenon

Answer

Altered reaction in presence of H₂O

Question 52

52. Density of H₂SO₄ in lead accumulator is

Question 53

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

Answer

Na⁺ + e– → Na

Answer

2Br– → Br₂ + 2e –

Answer

Br₂ + 2e – → 2Br –

Answer

Na → Na⁺ + e–

Question 54

54. Which has maximum oxidation number

Question 55

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

Answer

5.58g NaCl/100m

Answer

20g NaCl/100ml

Answer

10.0g NaCl/100ml

Answer

58.5g NaCl/100ml

Question 56

56. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 57

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

Answer

1.81 cm¯³

Answer

1.15 cm¯³

Answer

2.15 cm¯³

Answer

1.25 cm¯³

Question 58

58. Stronger the oxidizing agent, greater is the

Answer

Redox potential

Answer

e.m.f of cell

Answer

Oxidation potential

Answer

Reduction potential

Question 59

59. 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 60

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

Question 61

61. Reduction always occurs

Answer

Both A and B

Answer

None of these

Answer

At cathode

Question 62

62. Reaction takes place at anode is

Answer

Ionization

Answer

Hydrolysis

Question 63

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

Answer

More than that of H₂O

Answer

Equal to that of ethanol

Answer

Equal to that of water

Answer

Less than that of water

Question 64

64. During a redox reaction, an oxidizing agent

Answer

Gains electrons

Answer

Loses electrons

Answer

Is oxidized

Answer

Is hydrolysed

Answer 130

Dilution decreases

Answer 131

Pressure increases

Answer 132

Dilution increases

Answer 133

Atoms of Na and Cl.

Answer 134

Free molecules

Answer 135

Free electrons

Answer 136

Hydrolyzed

Answer 137

Precipitated

Answer 138

O₂, SO₂

Answer 139

None of these

Answer 140

Ostwald’s dilution law

Answer 141

Distribution law

Answer 142

Raoult’s law

Answer 143

Henry’s law

Answer 144

800 mm of Hg

Answer 145

750 mm of Hg

Answer 146

760 mm of Hg

Answer 147

780 mm of Hg

Answer 148

Na₂SO₄

Answer 149

CH₃ CooNH₄

Answer 150

Very low ionization potential values

Answer 151

Very high negative values reduction potential

Answer 152

Reduction potentials are negative

Answer 153

Very high positive value of reduction potential

Answer 154

Electroplating

Answer 155

Both A and B

Answer 156

None of these

Answer 157

Electrorefining

Answer 158

0.1 N NaCl

Answer 159

Slightly less than the total volume of the components

Answer 160

Equal to the total volume of the components

Answer 161

Slightly more than the total volume of the components

Answer 162

None of these

Answer 163

Phosphorus acid

Answer 164

Nitric acid

Answer 165

Boric acid

Answer 166

Sulphuric acid

Answer 167

Sufficient date not given

Answer 168

Electrons are released at anode

Answer 169

Salt bridge maintains the electrical neutrality of the solution

Answer 170

Cathode is regarded as negative electrode

Answer 171

Chemical energy is converted into electrical energy

Answer 172

0.1 M BaCl₂

Answer 173

0.1 M NaCl

Answer 174

0.1 M Glucose

Answer 175

0.1 M Sucrose

Answer 176

12157.48 sec

Answer 177

Making leather

Answer 178

Rust removal

Answer 179

Manufacture of bleach

Answer 180

Electroplating

Answer 181

H₄P₃O₇

Answer 182

All of these

Answer 183

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

Answer 184

Hg is more inert than Pt

Answer 185

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

Answer 186

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

Answer 187

1 – 2 α

Answer 188

Ionization potential

Answer 189

Electroplating

Answer 190

Standard electrode potential

Answer 191

Electric change

Answer 192

Inversion point

Answer 193

Boiling point

Answer 194

Sublimation point

Answer 195

Melting point

Answer 196

0.66 cm¯¹

Answer 197

0.918 cm¯¹

Answer 198

1.12 cm¯¹

Answer 199

0.142 cm¯¹

Answer 200

It has not potential

Answer 201

Degree of solubilization of solute

Answer 202

The degree of decomposition of solution

Answer 203

The extent of dissolution of solute

Answer 204

The extent of dissociation of solute

Answer 205

Heat energy

Answer 206

Magnetic energy

Answer 207

Sound energy

Answer 208

Electrical energy

Answer 209

302 S cm² mol¯¹

Answer 210

278 S cm² mol¯¹

Answer 211

128 S cm² mol¯¹

Answer 212

176 S cm² mol¯¹

Answer 213

Electrolytic cell

Answer 214

Daniel cell

Answer 215

Galvanic cell

Answer 216

None of these

Answer 217

Distillation

Answer 218

Vacuum distillation

Answer 219

Fractional distillation

Answer 220

Neutralization

Answer 221

Spontaneous reaction

Answer 222

Non-spontaneous reaction

Answer 223

4.0 x 10¹²

Answer 224

1.0 x 10¹⁰

Answer 225

2.0 x 10¹¹

Answer 226

1.0 x 10²

Answer 227

Any possibility

Answer 228

B.P of water decrease

Answer 229

B.P of water remain constant

Answer 230

B.P of water increase

Answer 231

Molarity of the solution

Answer 232

Molarity of the solvent

Answer 233

Molality of the solution

Answer 234

Mole fraction of the solution

Answer 235

Galvanic cell

Answer 236

Electrolytic cell

Answer 237

Both oxidation and reduction

Answer 238

Neither oxidation and reduction

Answer 239

Ohm cm¯¹

Answer 240

Ohm¯¹ cm

Answer 241

Ohm cm¯²

Answer 242

Ohm¯¹ cm¯¹

Answer 243

Hg₂Cl₂

Answer 244

Create potential difference between two electrodes

Answer 245

Produce high purity water

Answer 246

Generate heat

Answer 247

Remove adsorbed oxygen from electrode surfaces

Answer 248

Electrolysis

Answer 249

Electroplating

Answer 250

Conduction

Answer 251

Pt and graphite only

Answer 252

Na, Pt and graphite

Answer 253

Na and S only

Answer 254

∆ G = -ve

Answer 255

∆ G = -ve, ∆ E = 0

Answer 256

∆ G = +ve, ∆ E = 0

Answer 257

∆ G = 0, ∆E = 0

Answer 258

Is readily decomposed

Answer 259

Is neutral

Answer 260

Has low boiling point

Answer 261

Is almost unionized

Answer 262

Neutralization

Answer 263

Sum of reduction and oxidation potentials

Answer 264

None of these

Answer 265

Slightly greater than one

Answer 266

None of these

Answer 267

Exactly equal to one

Answer 268

Slightly less than one

Answer 269

H+ and OH-

Answer 270

Not particular

Answer 271

Parts per million

Answer 272

Milligram percent

Answer 273

Microgram percent

Answer 274

Gram per million

Answer 275

1.06 x 10²

Answer 276

1.06 x 10⁴

Answer 277

1.06 x 10³

Answer 278

Arrhenius law

Answer 279

Ostwald’s law

Answer 280

Raoult’s law

Answer 281

Henry’s law

Answer 282

Boiling point of pure benzene increases by the addition of toluene

Answer 283

Boiling point of pure water decreases by the addition of ethanol

Answer 284

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

Answer 285

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 286

Depends on density of electrolyte itself.

Answer 287

Decreases on dilution

Answer 288

Increases on dilution slightly

Answer 289

Does not change on dilution

Answer 290

Elevation in boiling point

Answer 291

Diffusion rate of the solute

Answer 292

Ionic concentration

Answer 293

Flow of solvent from a concentrated to a dilute solution

Answer 294

A chemical cell

Answer 295

A voltaic cell

Answer 296

An electrolytic cell

Answer 297

A galvanic cell

Answer 298

Neither a nor b

Answer 299

Concentration solutions behave as nearly non – ideal solutions

Answer 300

Dilute solution which behave as nearly ideal solution

Answer 301

Both a and b

Answer 302

Heat energy

Answer 303

Electrical energy

Answer 304

None of these

Answer 305

Chemical energy

Answer 306

Anode to cathode through the external circuit

Answer 307

Cathode to anode through the external circuit

Answer 308

Cathode to anode through the solution

Answer 309

Anode to cathode through the solution

Answer 310

Reduction occurs at cathode

Answer 311

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

Answer 312

All electrochemical reactions involve the transfer of electrons

Answer 313

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

Answer 314

Remains unchanged with dilution

Answer 315

Increases with dilution

Answer 316

Depends on mass of electrolyte

Answer 317

Decreases with dilution

Answer 318

Chemical energy is converted into electricity

Answer 319

Electrical energy is converted into chemical energy

Answer 320

Electrical energy is converted into heat

Answer 321

Chemical energy is converted into heat

Answer 322

100 g of Cu

Answer 323

31.75 g of Cu

Answer 324

63.5 g of Cu

Answer 325

96500 g of CU

Answer 326

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

Answer 327

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

Answer 328

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

Answer 329

Li is smaller in size as compared to Cu

Answer 330

Neutral atom

Answer 331

Does not provide any electron

Answer 332

120 g Cm³

Answer 333

1.2 g/Cm³

Answer 334

1.15 g/Cm³

Answer 335

1.25g/Cm³

Answer 336

Increase in oxidation number of all the elements on reactant side

Answer 337

Decrease in oxidation number

Answer 338

Both are possible

Answer 339

Increase in oxidation number

Answer 340

Decreases slowly

Answer 341

Decrease rapidly

Answer 342

Does not change

Answer 343

Drops to zero

Answer 344

They are mobile electrons in the metallic structure

Answer 345

In metals the ions are free to more

Answer 346

Metals have high resistance

Answer 347

Metals are decomposed by current

Answer 348

Gives ions only when electricity is passed

Answer 349

Forms complex ions in solution

Answer 350

Gives ions only when dissolved in water

Answer 351

Possesses ions even in solid state

Answer 352

None of these

Answer 353

All of these

Answer 354

Temperature

Answer 355

Nature of the gas

Answer 356

Pressure of the gas

Answer 357

22400 cm³

Answer 358

Pure distilled water

Answer 359

Chloroform

Answer 360

Dilute solution of glucose

Answer 361

Molten NaCl

Answer 362

Standard oxidation potential

Answer 363

Cell voltage

Answer 364

Standard reduction potential

Answer 365

Ionization potential

Answer 366

Cathodic protection

Answer 367

Galvanization

Answer 368

Photo electrolysis

Answer 369

Electrolysis

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