Chemistry Electro Chemistry Online Mcqs Test

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Question 1

1. 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 2

2. 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 3

3. 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 4

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

Answer

Equal to that of water

Answer

More than that of H₂O

Answer

Less than that of water

Answer

Equal to that of ethanol

Question 5

5. 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 6

6. The substance having highest conductivity at room temperature among the following is

Answer

0.1 N NaCl

Question 7

7. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

Question 8

8. 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

Very low ionization potential values

Answer

Reduction potentials are negative

Answer

Very high negative values reduction potential

Question 9

9. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

Question 10

10. Electrode potential of Zn is

Answer

Oxidation-reduction

Answer

Depends on the nature of the coupled electrode

Question 11

11. 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 12

12. 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 13

13. 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 14

14. Density of H₂SO₄ in lead accumulator is

Answer

1.2 g/Cm³

Answer

1.15 g/Cm³

Answer

1.25g/Cm³

Answer

120 g Cm³

Question 15

15. Oxidation state of hydrogen in CaH₂ is

Question 16

16. 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 17

17. 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

1.0 x 10¹⁰

Answer

4.0 x 10¹²

Answer

2.0 x 10¹¹

Question 18

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

Answer

A chemical cell

Answer

An electrolytic cell

Answer

A galvanic cell

Answer

A voltaic cell

Question 19

19. Which of the substances Na, Hg, S Pt and graphite can be used as electrodes in electrolytic cells having aqueous solution?

Answer

Pt and graphite only

Answer

Na, Pt and graphite

Answer

Na and S only

Question 20

20. What are the ions present in water?

Answer

H+ and OH-

Question 21

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

Question 22

22. Best way to prevent rusting iron is by

Answer

Both of these

Answer

Putting it in saline water

Answer

Making iron cathode

Answer

None of these

Question 23

23. In a Galvanic cell

Answer

Electrical energy is converted into chemical energy

Answer

Chemical energy is converted into electricity

Answer

Electrical energy is converted into heat

Answer

Chemical energy is converted into heat

Question 24

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

Answer

760 mm of Hg

Answer

Slightly more than 1 atom

Question 25

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

Question 26

26. The cryoscopic constant of water is 1.86. The elevation of B.P for a 0.1m solution of a solute in water is

Answer

Sufficient date not given

Question 27

27. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

Question 28

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

Answer

302 S cm² mol¯¹

Answer

278 S cm² mol¯¹

Answer

128 S cm² mol¯¹

Answer

176 S cm² mol¯¹

Question 29

29. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

Question 30

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

Question 31

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

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

Answer

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

Question 32

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

Question 33

33. Azeotropic mixture of HCl and water has

Question 34

34. 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 35

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

Answer

Iron rusts

Answer

Gold has higher reduction potential then iron

Answer

Gold has lower reduction potential then iron

Answer

Gold is denser

Question 36

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

Question 37

37. 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 38

38. 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 39

39. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

Question 40

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

Question 41

41. Units of molarity are

Answer

None of these

Question 42

42. 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 43

43. 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

S m² mol¯¹

Answer

S² m² mol

Answer

S² m² mol¯²

Question 44

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

Answer

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

Answer

Electrons flow from cathode to anode through the external battery

Answer

Electrons flow cathode to anode within the electrolytic solution

Answer

None of these

Question 45

45. Oxidation number of carbon in NaHCO₃ is

Question 46

46. In electrolytic cell, electricity in carried out by

Answer

Spontaneous reaction

Answer

Neutralization

Answer

Non-spontaneous reaction

Question 47

47. Potential of Zn is called

Answer

It has not potential

Question 48

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

Question 49

49. Molton NaCl conducts electricity due to the presence of

Answer

Free electrons

Answer

Atoms of Na and Cl.

Answer

Free molecules

Question 50

50. Decrease in oxidation number is called

Answer

All of these

Question 51

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

Question 52

52. Metals usually conduct electricity because

Answer

They are mobile electrons in the metallic structure

Answer

Metals are decomposed by current

Answer

In metals the ions are free to more

Answer

Metals have high resistance

Question 53

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

Answer

Sublimation point

Answer

Boiling point

Answer

Inversion point

Answer

Melting point

Question 54

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

Answer

H₄P₃O₇

Question 55

55. Density of H₂SO₄ in lead accumulator is

Question 56

56. 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 57

57. An aqueous solution freezes at -0.186°C. (Kf = 1.86, Kb = 0.512). What is the elevation in boiling point?

Question 58

58. 96500 C of electricity liberates from CuSO₄ solution

Answer

100 g of Cu

Answer

31.75 g of Cu

Answer

96500 g of CU

Answer

63.5 g of Cu

Question 59

59. 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 60

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

Question 61

61. Camphor is often used in molecular mass determination because

Answer

It is readily available

Answer

It is volatile

Answer

It is solvent for organic substances

Answer

It has a very high cryoscopic constant

Question 62

62. Specific conductivity of a solution

Answer

Increases with dilution

Answer

Remains unchanged with dilution

Answer

Depends on mass of electrolyte

Answer

Decreases with dilution

Question 63

63. A cell in which chemical energy is converted into electrical energy is called

Answer

Galvanic cell

Answer

Electrolytic cell

Question 64

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

Answer

Osmotic pressure

Answer

Surface tension

Answer

Refractive index

Answer 101

None of these

Answer 102

Spontaneous acid–base reactions

Answer 103

Non-spontaneous redox reactions

Answer 104

Spontaneous redox reactions

Answer 105

From anode to cathode inside the cell

Answer 106

From cathode to anode in outer circuit

Answer 107

From anode to cathode in an outer circuit

Answer 108

From cathode to anode inside the cell

Answer 109

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

Answer 110

Reduction occurs at cathode

Answer 111

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

Answer 112

All electrochemical reactions involve the transfer of electrons

Answer 113

Not particular

Answer 114

B.P of water increase

Answer 115

B.P of water remain constant

Answer 116

B.P of water decrease

Answer 117

Any possibility

Answer 118

Both A and B

Answer 119

At cathode

Answer 120

None of these

Answer 121

None of these

Answer 122

Heat energy

Answer 123

Chemical energy

Answer 124

Electrical energy

Answer 125

Anode to cathode through the external circuit

Answer 126

Cathode to anode through the external circuit

Answer 127

Cathode to anode through the solution

Answer 128

Anode to cathode through the solution

Answer 129

Ionization

Answer 130

Hydrolysis

Answer 131

Galvanic cell

Answer 132

Electrolytic cell

Answer 133

Daniel cell

Answer 134

Increase in oxidation number

Answer 135

Decrease in oxidation number

Answer 136

Increase in oxidation number of all the elements on reactant side

Answer 137

Both are possible

Answer 138

Chemical energy is converted into electrical energy

Answer 139

Salt bridge maintains the electrical neutrality of the solution

Answer 140

Cathode is regarded as negative electrode

Answer 141

Electrons are released at anode

Answer 142

0.1 M Glucose

Answer 143

0.1 M NaCl

Answer 144

0.1 M Sucrose

Answer 145

0.1 M BaCl₂

Answer 146

No connection exists

Answer 147

Electric circuit

Answer 148

Salt Bridge

Answer 149

Sulphuric acid

Answer 150

Boric acid

Answer 151

Phosphorus acid

Answer 152

Nitric acid

Answer 153

Exactly equal to one

Answer 154

None of these

Answer 155

Slightly less than one

Answer 156

Slightly greater than one

Answer 157

Boiling point of pure water decreases by the addition of ethanol

Answer 158

Vapour pressure of pure benzene decreases by the addition of naphthalene

Answer 159

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

Answer 160

Boiling point of pure benzene increases by the addition of toluene

Answer 161

1.06 x 10³

Answer 162

1.06 x 10⁴

Answer 163

1.06 x 10²

Answer 164

By heating it

Answer 165

By replacing external circuit with external source of electricity

Answer 166

By removal of solution

Answer 167

By addition of fresh solution

Answer 168

Electron transfer

Answer 169

A reaction in a solution

Answer 170

Ion combination reaction

Answer 171

Proton transfer

Answer 172

Distillation

Answer 173

None of these

Answer 174

Vacuum distillation

Answer 175

Fractional distillation

Answer 176

12157.48 sec

Answer 177

Dilution increases

Answer 178

Pressure increases

Answer 179

Dilution decreases

Answer 180

None of these

Answer 181

e.m.f of cell

Answer 182

Oxidation potential

Answer 183

Reduction potential

Answer 184

Redox potential

Answer 185

Parts per million

Answer 186

Gram per million

Answer 187

Milligram percent

Answer 188

Microgram percent

Answer 189

∆ G = -ve

Answer 190

∆ G = +ve, ∆ E = 0

Answer 191

∆ G = -ve, ∆ E = 0

Answer 192

∆ G = 0, ∆E = 0

Answer 193

[Pt(NH₃)₄Cl₂]Cl₂

Answer 194

[Pt(NH₃)₄Cl₄]

Answer 195

[Pt(NH₃)₄Cl]Cl₃

Answer 196

[Pt(NH₃)₄Cl₃]Cl

Answer 197

Strong acid and its salt of weak base

Answer 198

Weak acid and its salt of strong base

Answer 199

A strong acid and its salt of a strong base

Answer 200

Weak acid and its salt of weak base

Answer 201

Precipitated

Answer 202

Hydrolyzed

Answer 203

Unsaturated

Answer 204

Supersaturated

Answer 205

1.25 cm¯³

Answer 206

1.81 cm¯³

Answer 207

1.15 cm¯³

Answer 208

2.15 cm¯³

Answer 209

CH₃ CooNH₄

Answer 210

Na₂SO₄

Answer 211

Rechargeable

Answer 212

Electrolytic cell

Answer 213

Daniel cell

Answer 214

Non rechargeable

Answer 215

Both oxidation and reduction

Answer 216

Neither oxidation and reduction

Answer 217

Solvent particles

Answer 218

0.918 cm¯¹

Answer 219

0.142 cm¯¹

Answer 220

1.12 cm¯¹

Answer 221

0.66 cm¯¹

Answer 222

Loses electrons

Answer 223

Acts as a catalyst

Answer 224

pH is changed

Answer 225

Gains electrons

Answer 226

Depends on density of electrolyte itself.

Answer 227

Does not change on dilution

Answer 228

Decreases on dilution

Answer 229

Increases on dilution slightly

Answer 230

Ca(NO₃)₂

Answer 231

Thomas Gradam

Answer 232

Is almost unionized

Answer 233

Has low boiling point

Answer 234

Is neutral

Answer 235

Is readily decomposed

Answer 236

Drops to zero

Answer 237

Increases rapidly

Answer 238

Does not change

Answer 239

Increases gradually

Answer 240

Na → Na⁺ + e–

Answer 241

Na⁺ + e– → Na

Answer 242

2Br– → Br₂ + 2e –

Answer 243

Br₂ + 2e – → 2Br –

Answer 244

– 0.35 V

Answer 245

– 1.17 V

Answer 246

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

Answer 247

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

Answer 248

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

Answer 249

Li is smaller in size as compared to Cu

Answer 250

Neutralization

Answer 251

750 mm of Hg

Answer 252

760 mm of Hg

Answer 253

780 mm of Hg

Answer 254

800 mm of Hg

Answer 255

The free energy of mixing is zero

Answer 256

The enthalpy of mixing is zero

Answer 257

The entropy of mixing is zero

Answer 258

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

Answer 259

Molarity of the solvent

Answer 260

Mole fraction of the solution

Answer 261

Molarity of the solution

Answer 262

Molality of the solution

Answer 263

Heat energy

Answer 264

Sound energy

Answer 265

Electrical energy

Answer 266

Magnetic energy

Answer 267

Both A and B

Answer 268

None of these

Answer 269

Electroplating

Answer 270

Electrorefining

Answer 271

All of these

Answer 272

Temperature

Answer 273

Pressure of the gas

Answer 274

Nature of the gas

Answer 275

Arrhenius law

Answer 276

Raoult’s law

Answer 277

Ostwald’s law

Answer 278

Henry’s law

Answer 279

Ostwald’s dilution law

Answer 280

Raoult’s law

Answer 281

Distribution law

Answer 282

Henry’s law

Answer 283

Chloroform

Answer 284

Molten NaCl

Answer 285

Dilute solution of glucose

Answer 286

Pure distilled water

Answer 287

Is hydrolysed

Answer 288

Is oxidized

Answer 289

Loses electrons

Answer 290

Gains electrons

Answer 291

Naphthalene

Answer 292

Does not provide any electron

Answer 293

Neutral atom

Answer 294

Hypertonic

Answer 295

Electroplating

Answer 296

Rust removal

Answer 297

Manufacture of bleach

Answer 298

Making leather

Answer 299

The extent of dissolution of solute

Answer 300

Degree of solubilization of solute

Answer 301

The degree of decomposition of solution

Answer 302

The extent of dissociation of solute

Answer 303

One gm. atomic weight

Answer 304

None of these

Answer 305

One gm. Equivalent weight

Answer 306

Electrochemical equivalent

Answer 307

Gives ions only when electricity is passed

Answer 308

Possesses ions even in solid state

Answer 309

Forms complex ions in solution

Answer 310

Gives ions only when dissolved in water

Answer 311

None of these

Answer 312

Slightly more than the total volume of the components

Answer 313

Slightly less than the total volume of the components

Answer 314

None of these

Answer 315

Equal to the total volume of the components

Answer 316

Concentration solutions behave as nearly non – ideal solutions

Answer 317

Both a and b

Answer 318

Dilute solution which behave as nearly ideal solution

Answer 319

Neither a nor b

Answer 320

Galvanization

Answer 321

Cathodic protection

Answer 322

Electrolysis

Answer 323

Photo electrolysis

Answer 324

Altered reaction in presence of H₂O

Answer 325

Electrochemical phenomenon

Answer 326

Union between two light metals and a heavy metal

Answer 327

Interaction

Answer 328

None of these

Answer 329

Standard electrode potential

Answer 330

Electric change

Answer 331

Ionization potential

Answer 332

Electroplating

Answer 333

Cell voltage

Answer 334

Standard reduction potential

Answer 335

Standard oxidation potential

Answer 336

Ionization potential

Answer 337

5.58g NaCl/100m

Answer 338

20g NaCl/100ml

Answer 339

10.0g NaCl/100ml

Answer 340

58.5g NaCl/100ml

Answer 341

Hg₂Cl₂

Answer 342

Greater negative value of standard reduction potential

Answer 343

None of these

Answer 344

Greater positive value of standard reduction potential

Answer 345

Lesser positive value of standard reduction potential

Answer 346

Ohm¯¹ cm¯¹

Answer 347

Ohm¯¹ cm

Answer 348

Ohm cm¯¹

Answer 349

Ohm cm¯²

Answer 350

Increase in oxidation number of the elements in reactants

Answer 351

Increase in oxidation number of element

Answer 352

Decrease in oxidation number of element

Answer 353

Oxidation number neither increases nor decreases

Answer 354

Electroplating

Answer 355

Electrolysis

Answer 356

Conduction

Answer 357

Elevation in boiling point

Answer 358

Ionic concentration

Answer 359

Diffusion rate of the solute

Answer 360

Flow of solvent from a concentrated to a dilute solution

Answer 361

Does not change

Answer 362

Decrease rapidly

Answer 363

Decreases slowly

Answer 364

Drops to zero

Answer 365

Sum of reduction and oxidation potentials

Answer 366

Both Na⁺ and CI¯

Answer 367

None of these

Answer 368

1 – 2 α

Answer 369

Hg₂Cl₂

Total Questions:	192
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Total Marks:	192
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