Question # 1

K,Ca and Li metals may be arranged in decreasing order of their reduction potential as :

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Li, k, Ca

Ca, K, Li

Li, Ca, K

K, Ca, Li

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

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Generate heat

Remove adsorbed oxygen from electrode surfaces

Produce High purity water

Create potential difference between two electrodes

Oxidation number of oxygen in OF₂is

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+1

-1

+2

-2

Which one of the following reactions is not spontaneous

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For spontaneity of a cell, which is correct?

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ΔG = 0,ΔE = 0

ΔG = -ve ,ΔE = 0

ΔG = +ve ,ΔE = 0

ΔG = -ve

An electrolyte

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Forms complex ions solution

Gives ions only when electricity is passed

Possesses ions even in solid state

Gives ions only when dissolved in water

When aqueous solution of NaOH is electrolysed useing graphite electrodes, the product obtained at anode is

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O₂gas

H₂gas

Na metal

Na₂O

Best way to prevent rusting of iron is by

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Making iron cathode

Putting it in saline water

Both of these

None of these

The oxidation number of chromium in K₂Cr₂O₇is

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14

12

6

None of these

Lead accumulator stops discharging current when

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Lead at anode converted to PbO₂

PbO₂at cathode converted to Pb

Both electrodes are completely covered with PbSO₄

Both electrodes are completely covered with Pb(OH)₂

Sodium metal is obtained by the electrolysis of fused NaCl in cell is called

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Nelson's cell

Down's cell

Daniell cell

Voltaic cell

An electrochemical cell is based upon

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Acid-base reaction

Redox reaction

Nuclear reaction

None of the above

The cell in which a non-spontaneous redox reaction takes place as a result electricity is known as :

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Electrolytic cell.

Voltaic cell.

Daniel cell.

Dry cell.

The function of salt bridge is :

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To increase movement onions.

To increase the emf of cell.

To decrease the temperate

To maintain electrical neutrality

In a Galvanic cell

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Chemical energy is converted into electricity

Chemical energy is converted into heat

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

Coupling of Pb with its Pb⁺⁺/Pb = -0.13 V and Ag with Ag⁺/ Ag = +0.80 V, the cell reaction

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Which of the following yield both hydrogen and chlorine on electrolysis:

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Electrolysis of acidified water.

Electrolysis of molten NaCl

Electrolysis of aqueous NaCl

Electrolysis of saline water

When electric current is used to carry out non-spontaneous redox, the process is called

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Hydrolysis

Electrolysis

Decomposition

Neutralization

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

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ZnCl₂

CuSO₄

Hg₂Cl₂

HgCl₂

When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

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1.08 g

10.8 g

21.6 g

108 g

Li has the lowest reduction potential while the element with highest reduction potential is

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H

F

O

N

Reduction or oxidation potential of standard hydrogen electrode is :

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0.0 Volt

0.8Volt

1.0Volt

1.8Volt

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

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Na, Pt and graphite

Na and Hg

Pt and graphite only

Na and S only

A cell in which electric current is produced as a result spontaneous redox reaction is called :

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Dry cell

Electrolytic cell

Galvanic cell

Standard cell

Electrochemistry is concerned with the conversion of electrical energy into chemical energy in :

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Galvanic cell

Electrolytic cell

Voltaic cell

Both (a) and (c)

Most metals are conductors of electricity because of the :

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Light weight.

Immobility of the electrons.

Lustrous surfaces

Relatively free movement of their electrons

In the reaction K₂Cr₂O₇+ HCl + CrCl₃+ Cl₂+ H₂O the element which is reduced is

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K

Cl

Cr

H

During electrolysis of KNO₃, H₂is evolved

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Anode

Cathode

Both a and b

None

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

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2.0

1.5

1.0

0.5

Electrochemical series is a list of element S arranged into the increasing order of their

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Standard oxidation potential

Standard reduction potential

Cell voltage

Ionization potential

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