Question # 1

The voltaic or galvanic cells which cannot be recharged are called

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Primary cells

Secondary cells

Infinite cells

Fuel cells

During electrolysis, electrons are :

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Lost by anions and gained by cations

Gained by anions and lost by cations

Gained only

Lost only

Specific conductivity of a solution

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Increases with dilution

Decreases with dilution

Remains unchanged with dilution

Depends on mass of electrolyte

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A strong reducing agent

A strong oxidising agent

Better oxidising agent than hydrogen

Less reducing agent than hydrogen

In passage of electricity through aqueous solution of AgNO₃silver dissolves at anode to form Ag⁺, the electrodes are

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Silver metal

Pt metal

Graphite

Copper metal

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

During electrolysis, the reaction that takes place at cathode is :

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Reduction

Both (a) and (c)

Oxidation

No reaction occurs

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

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ZnCl₂

CuSO₄

Hg₂Cl₂

HgCl₂

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

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Decrease rapidly

Decrease slowly

Does not change

Drops to zero

Which of the following will be good conductor of electricity

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Pure distilled water

Molten NaCl

Dilute solution of glucose

Chloroform

Reduction or oxidation potential of standard hydrogen electrode is :

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0.0 Volt

0.8Volt

1.0Volt

1.8Volt

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

Time required to deposit one millimole of aluminium metal by the passage of 9.65 amperes through molten electrolyte containing aluminium ion is

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30 s

10 s

30,000 s

10,000 s

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

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Standard electrode potential

Electric charge

Ionization potential

Electroplating

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

Matals usually conduct electricity because

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There are mobile electrons in the metallic structure

Metals are decomposed by current

Metals have high resistance

In metals the ions are free to move

Purification of an impure copper is made by electrolytic cell, in which impure copper is anode and pure copper is cathode, and the electrolyte used is

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H₂SO₄

CuSO₄

ZnSO₄

Na₂SO₄

When quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

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One gm, atomic weight

One gm, Equivalent

Eletrochemical equivalent

None of the above

The cathodic reaction in the electrolysis of dill H₂SO₄with Pt electrodes

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Reduction

Oxidation

Both oxidation and reduction

neither oxidation or reduction

When aluminium electrode is coupled with copper electrode in a galvanic cell :

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Reduction takes place at aluminium electrode.

Oxidation takes place at copper electrode.

Reduction takes place at copper electrode.

Both (a) and (c)

During electrolysis of KNO₃, H₂is evolved

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Anode

Cathode

Both a and b

None

Alkaline battery has a voltage of

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4.5 V

3.5 V

2.5 V

1.5 V

What are the products electrolysis of aqueous sodium chloride at two electrodes

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Chlorine at anode and oxygen at cathode.

Hydrogen at anode and chlorine at cathode.

Chlorine at anode and hydrogen at cathode.

Chlorine at anode and sodium at cathode.

In a Galvanic cell, the electrons flow from

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A node to cathode through the solution

Cathode to anode through the external circuit

Anode to cathode through the external circuit

In KO₂the oxidation state of oxygen is

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-2

-1

+1/2

-1/2

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Fe is reduced

Fe is oxidized

Cl₂is oxidized

None of these

In lead accumulator the electrolyte is H₂SO₄solution is

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30% H₂SO₄

60% H₂SO₄

80% H₂SO₄

90% H₂SO₄

The reduction potential to copper electrode is +0.34 V and that of Zn electrode is -0.76 V. when these two are coupled the e.m.f. of the cell is

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-0.42 V

+0.42

-1.10 V

+1.10 V

During redox reaction an oxidizing agent

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Gains electrons

Is oxidized

Loses electrons

Hydrolysed

The oxidation number of Mn is KMnO₄is

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+2

+4

+6

+7

The two half cells of a galvanic cell are connected by

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Ammeter

Salt bridge

Hydrogen electrode

Copper electrode

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