Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. Oxidation number of carbon in NaHCO₃ is

Question 2

2. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

Question 3

3. The solubility of a gas in water depends upon

Answer

Temperature

Answer

Nature of the gas

Answer

All of these

Answer

Pressure of the gas

Question 4

4. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

Answer

Electric change

Answer

Electroplating

Answer

Ionization potential

Answer

Standard electrode potential

Question 5

5. Reaction takes place at anode is

Answer

Hydrolysis

Answer

Ionization

Question 6

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

Question 7

7. Salt bridge transfers

Answer

Solvent particles

Question 8

8. 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 9

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

Answer

Loses electrons

Answer

Gains electrons

Answer

Acts as a catalyst

Answer

pH is changed

Question 10

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

Question 11

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

Question 12

12. When common salt is dissolved in water

Answer

B.P of water decrease

Answer

B.P of water remain constant

Answer

B.P of water increase

Answer

Any possibility

Question 13

13. In alkaline battery the anode is made up of

Question 14

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

Question 15

15. Which has maximum oxidation number

Question 16

16. Reduction always occurs

Answer

None of these

Answer

At cathode

Answer

Both A and B

Question 17

17. H₂ gas in SHE is filled at a pressure of

Answer

750 mm of Hg

Answer

760 mm of Hg

Answer

780 mm of Hg

Answer

800 mm of Hg

Question 18

18. The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

Answer

Melting point

Answer

Sublimation point

Answer

Inversion point

Answer

Boiling point

Question 19

19. 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 reduction potential of Li⁺/Li is lower than that of Cu²+/Cu

Answer

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

Question 20

20. The unit of specific conductivity is

Answer

Ohm cm¯²

Answer

Ohm¯¹ cm

Answer

Ohm¯¹ cm¯¹

Answer

Ohm cm¯¹

Question 21

21. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

Question 22

22. In alkaline battery anode is made up of

Question 23

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

Answer

Both Na⁺ and CI¯

Answer

None of these

Question 24

24. If the salt bridge is not used between two half cells, then the voltage

Answer

Decreases slowly

Answer

Decrease rapidly

Answer

Drops to zero

Answer

Does not change

Question 25

25. Temperature for standard electrode potential is

Question 26

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

Question 27

27. 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 28

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

Question 29

29. The degree of dissociation of weak electrolyte increases as

Answer

Dilution increases

Answer

Dilution decreases

Answer

Pressure increases

Question 30

30. Which of the following statements is FALSE?

Answer

Reduction occurs at cathode

Answer

All electrochemical reactions involve the transfer of electrons

Answer

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

Answer

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

Question 31

31. 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 32

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

Answer

Not particular

Question 33

33. Solution with same osmotic pressures are called

Answer

Hypertonic

Question 34

34. 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 35

35. Secondary cell is

Answer

Electrolytic cell

Answer

Non rechargeable

Answer

Daniel cell

Answer

Rechargeable

Question 36

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

Answer

∆ G = 0, ∆E = 0

Answer

∆ G = +ve, ∆ E = 0

Answer

∆ G = -ve, ∆ E = 0

Answer

∆ G = -ve

Question 37

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

Answer

None of these

Question 38

38. 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

0.142 cm¯¹

Answer

1.12 cm¯¹

Answer

0.918 cm¯¹

Answer

0.66 cm¯¹

Question 39

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

Question 40

40. Density of H₂SO₄ in lead accumulator is

Answer

120 g Cm³

Answer

1.2 g/Cm³

Answer

1.15 g/Cm³

Answer

1.25g/Cm³

Question 41

41. Half cells are interconnected through

Answer

Electric circuit

Answer

Salt Bridge

Answer

No connection exists

Question 42

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

Question 43

43. The amount of electricity that can deposit 108 g of silver from silver nitrate solution is

Question 44

44. 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 negative values reduction potential

Answer

Reduction potentials are negative

Answer

Very high positive value of reduction potential

Answer

Very low ionization potential values

Question 45

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

Question 46

46. 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 is denser

Answer

Gold has higher reduction potential then iron

Question 47

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

Question 48

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

Answer

Less than that of water

Answer

Equal to that of water

Answer

Equal to that of ethanol

Answer

More than that of H₂O

Question 49

49. Colligative properties are the properties of

Answer

Dilute solution which behave as nearly ideal solution

Answer

Neither a nor b

Answer

Concentration solutions behave as nearly non – ideal solutions

Answer

Both a and b

Question 50

50. 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

2.0 x 10¹¹

Answer

1.0 x 10¹⁰

Answer

4.0 x 10¹²

Question 51

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

Question 52

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

Answer

2Br– → Br₂ + 2e –

Answer

Br₂ + 2e – → 2Br –

Answer

Na⁺ + e– → Na

Answer

Na → Na⁺ + e–

Question 53

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

Question 54

54. Which of the following will have the highest boiling point at 1 atm pressure?

Answer

0.1 M Sucrose

Answer

0.1 M NaCl

Answer

0.1 M BaCl₂

Answer

0.1 M Glucose

Question 55

55. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 56

56. 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 57

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

Question 58

58. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

Answer

176 S cm² mol¯¹

Answer

128 S cm² mol¯¹

Answer

302 S cm² mol¯¹

Answer

278 S cm² mol¯¹

Question 59

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

Question 60

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

Answer

Surface tension

Answer

Refractive index

Answer

Osmotic pressure

Question 61

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

Answer

Ostwald’s dilution law

Answer

Raoult’s law

Answer

Distribution law

Answer

Henry’s law

Question 62

62. 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 63

63. Strong reducing agents have

Answer

None of these

Answer

Greater positive value of standard reduction potential

Answer

Greater negative value of standard reduction potential

Answer

Lesser positive value of standard reduction potential

Question 64

64. Specific conductivity of a solution

Answer

Increases with dilution

Answer

Decreases with dilution

Answer

Remains unchanged with dilution

Answer

Depends on mass of electrolyte

Answer 127

Both of these

Answer 128

Putting it in saline water

Answer 129

None of these

Answer 130

Making iron cathode

Answer 131

Spontaneous reaction

Answer 132

Non-spontaneous reaction

Answer 133

Neutralization

Answer 134

Electrical energy is converted into heat

Answer 135

Electrical energy is converted into chemical energy

Answer 136

Chemical energy is converted into electricity

Answer 137

Chemical energy is converted into heat

Answer 138

Free electrons

Answer 139

Free molecules

Answer 140

Atoms of Na and Cl.

Answer 141

Anode to cathode through the external circuit

Answer 142

Anode to cathode through the solution

Answer 143

Cathode to anode through the solution

Answer 144

Cathode to anode through the external circuit

Answer 145

Electroplating

Answer 146

Electrorefining

Answer 147

Both A and B

Answer 148

None of these

Answer 149

1.25 cm¯³

Answer 150

1.15 cm¯³

Answer 151

2.15 cm¯³

Answer 152

1.81 cm¯³

Answer 153

Neutralization

Answer 154

Unsaturated

Answer 155

Supersaturated

Answer 156

A galvanic cell

Answer 157

A voltaic cell

Answer 158

A chemical cell

Answer 159

An electrolytic cell

Answer 160

Electrolysis

Answer 161

Conduction

Answer 162

Electroplating

Answer 163

Na and S only

Answer 164

Na, Pt and graphite

Answer 165

Pt and graphite only

Answer 166

Slightly more than 1 atom

Answer 167

760 mm of Hg

Answer 168

Increase in oxidation number of the elements in reactants

Answer 169

Decrease in oxidation number of element

Answer 170

Increase in oxidation number of element

Answer 171

Oxidation number neither increases nor decreases

Answer 172

– 0.35 V

Answer 173

– 1.17 V

Answer 174

The free energy of mixing is zero

Answer 175

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

Answer 176

The entropy of mixing is zero

Answer 177

The enthalpy of mixing is zero

Answer 178

By replacing external circuit with external source of electricity

Answer 179

By heating it

Answer 180

By removal of solution

Answer 181

By addition of fresh solution

Answer 182

20g NaCl/100ml

Answer 183

10.0g NaCl/100ml

Answer 184

58.5g NaCl/100ml

Answer 185

5.58g NaCl/100m

Answer 186

Cell voltage

Answer 187

Ionization potential

Answer 188

Standard oxidation potential

Answer 189

Standard reduction potential

Answer 190

Reduction potential

Answer 191

e.m.f of cell

Answer 192

Oxidation potential

Answer 193

Redox potential

Answer 194

Depends on the nature of the coupled electrode

Answer 195

Oxidation-reduction

Answer 196

The extent of dissociation of solute

Answer 197

The extent of dissolution of solute

Answer 198

Degree of solubilization of solute

Answer 199

The degree of decomposition of solution

Answer 200

Galvanic cell

Answer 201

Daniel cell

Answer 202

Electrolytic cell

Answer 203

None of these

Answer 204

Electrons flow cathode to anode within the electrolytic solution

Answer 205

Electrons flow from cathode to anode through the external battery

Answer 206

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

Answer 207

Slightly less than one

Answer 208

Slightly greater than one

Answer 209

None of these

Answer 210

Exactly equal to one

Answer 211

Electrical energy

Answer 212

Heat energy

Answer 213

Chemical energy

Answer 214

None of these

Answer 215

Metals are decomposed by current

Answer 216

In metals the ions are free to more

Answer 217

Metals have high resistance

Answer 218

They are mobile electrons in the metallic structure

Answer 219

H+ and OH-

Answer 220

Neither oxidation and reduction

Answer 221

Both oxidation and reduction

Answer 222

Hg₂Cl₂

Answer 223

All of these

Answer 224

1 – 2 α

Answer 225

Forms complex ions in solution

Answer 226

Gives ions only when electricity is passed

Answer 227

Possesses ions even in solid state

Answer 228

Gives ions only when dissolved in water

Answer 229

S m mol¯¹

Answer 230

S² m² mol

Answer 231

S m² mol¯¹

Answer 232

S² m² mol¯²

Answer 233

One gm. atomic weight

Answer 234

Electrochemical equivalent

Answer 235

One gm. Equivalent weight

Answer 236

None of these

Answer 237

Is almost unionized

Answer 238

Is readily decomposed

Answer 239

Has low boiling point

Answer 240

Is neutral

Answer 241

Boiling point of pure water decreases by the addition of ethanol

Answer 242

Boiling point of pure benzene increases by the addition of toluene

Answer 243

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 244

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

Answer 245

Thomas Gradam

Answer 246

Electrochemical phenomenon

Answer 247

Altered reaction in presence of H₂O

Answer 248

Interaction

Answer 249

Union between two light metals and a heavy metal

Answer 250

0.1 N NaCl

Answer 251

A reaction in a solution

Answer 252

Proton transfer

Answer 253

Electron transfer

Answer 254

Ion combination reaction

Answer 255

63.5 g of Cu

Answer 256

100 g of Cu

Answer 257

31.75 g of Cu

Answer 258

96500 g of CU

Answer 259

Gram per million

Answer 260

Parts per million

Answer 261

Milligram percent

Answer 262

Microgram percent

Answer 263

From anode to cathode inside the cell

Answer 264

From cathode to anode in outer circuit

Answer 265

From cathode to anode inside the cell

Answer 266

From anode to cathode in an outer circuit

Answer 267

It has not potential

Answer 268

Precipitated

Answer 269

Hydrolyzed

Answer 270

Electroplating

Answer 271

Manufacture of bleach

Answer 272

Making leather

Answer 273

Rust removal

Answer 274

Sufficient date not given

Answer 275

None of these

Answer 276

Gains electrons

Answer 277

Is hydrolysed

Answer 278

Loses electrons

Answer 279

Is oxidized

Answer 280

None of these

Answer 281

Sum of reduction and oxidation potentials

Answer 282

Electrolysis

Answer 283

Photo electrolysis

Answer 284

Galvanization

Answer 285

Cathodic protection

Answer 286

[Pt(NH₃)₄Cl₂]Cl₂

Answer 287

[Pt(NH₃)₄Cl₃]Cl

Answer 288

[Pt(NH₃)₄Cl₄]

Answer 289

[Pt(NH₃)₄Cl]Cl₃

Answer 290

1.06 x 10²

Answer 291

1.06 x 10³

Answer 292

1.06 x 10⁴

Answer 293

22400 cm³

Answer 294

Ostwald’s law

Answer 295

Raoult’s law

Answer 296

Arrhenius law

Answer 297

Henry’s law

Answer 298

Magnetic energy

Answer 299

Sound energy

Answer 300

Electrical energy

Answer 301

Heat energy

Answer 302

Flow of solvent from a concentrated to a dilute solution

Answer 303

Ionic concentration

Answer 304

Elevation in boiling point

Answer 305

Diffusion rate of the solute

Answer 306

None of these

Answer 307

None of these

Answer 308

Slightly less than the total volume of the components

Answer 309

Equal to the total volume of the components

Answer 310

Slightly more than the total volume of the components

Answer 311

H₄P₃O₇

Answer 312

Increase in oxidation number of all the elements on reactant side

Answer 313

Increase in oxidation number

Answer 314

Decrease in oxidation number

Answer 315

Both are possible

Answer 316

Naphthalene

Answer 317

Neutral atom

Answer 318

Does not provide any electron

Answer 319

Ca(NO₃)₂

Answer 320

Molten NaCl

Answer 321

Chloroform

Answer 322

Pure distilled water

Answer 323

Dilute solution of glucose

Answer 324

Hg is more inert than Pt

Answer 325

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

Answer 326

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

Answer 327

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

Answer 328

None of these

Answer 329

Spontaneous redox reactions

Answer 330

Non-spontaneous redox reactions

Answer 331

Spontaneous acid–base reactions

Answer 332

Weak acid and its salt of strong base

Answer 333

Strong acid and its salt of weak base

Answer 334

Weak acid and its salt of weak base

Answer 335

A strong acid and its salt of a strong base

Answer 336

Electrolytic cell

Answer 337

Galvanic cell

Answer 338

Hg₂Cl₂

Answer 339

Depends on density of electrolyte itself.

Answer 340

Does not change on dilution

Answer 341

Increases on dilution slightly

Answer 342

Decreases on dilution

Answer 343

Create potential difference between two electrodes

Answer 344

Produce high purity water

Answer 345

Generate heat

Answer 346

Remove adsorbed oxygen from electrode surfaces

Answer 347

Vacuum distillation

Answer 348

Fractional distillation

Answer 349

None of these

Answer 350

Distillation

Answer 351

Increases gradually

Answer 352

Increases rapidly

Answer 353

Does not change

Answer 354

Drops to zero

Answer 355

It is readily available

Answer 356

It is volatile

Answer 357

It has a very high cryoscopic constant

Answer 358

It is solvent for organic substances

Answer 359

Na₂SO₄

Answer 360

CH₃ CooNH₄

Answer 361

Molality of the solution

Answer 362

Molarity of the solution

Answer 363

Mole fraction of the solution

Answer 364

Molarity of the solvent

Answer 365

12157.48 sec

Answer 366

Phosphorus acid

Answer 367

Sulphuric acid

Answer 368

Boric acid

Answer 369

Nitric acid

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