Question # 1

The process of electrical coating of one metal on another to protect, decorate or to have greater resistance to corrosion is called

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Electroplating

Electrolysis

Conduction

Induction

2.5 faradays of electricity is passed through solution of CuSO_{4. The number of gram equivalents of copper deposited on the cathode would be}

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1

2

2.5

1.25

Standard reduction of Zn = -0.76 V and that of Ni is -0.25 V. On coupling them by a salt bridge which of these will act as anode

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Salt bridge will act as anode

Zn will act as anode

Ni will act as anode

None of these

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

In electrolysis of NaCl when Pt electrode is taken then H₂is liberated at cathode while with Hg cathode it forms sodium amalgam

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Hg is more inert than Pt

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

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

Conc. of H⁺ions is larger when Pt electrode is taken

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

Metallic conduction is due to the

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Movement of electrons

Movement of ions

Both a and b

None of these

When fused PbBr₂is electrolyed then

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Bromine appears at cathode

Lead deposited at the cathode

Lead appears at the anode

None of these happens

A standard hydrogen electrode (S.H.E) consists of a platinized platinum electrode dipped in 1 molar solution of H⁺ions and hydrogen gas is passed at a pressure of

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One pascal

One kilo pascal

One atmoshpere

Then atmoshpere

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

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

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0.25 mole

0.5 mole

1.0 mole

2.00 mole

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)

An electric current is passed through silver nitrate solution using silver electrodes.10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is

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6.4 g

2.3 g

128.8 g

3.2 g

Coinage metals like Au, Pt, Ag and Cu are the least reactive metals and don't liberate H₂gas when treated with acids because

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These have very high positive values of reduction potentials

These have very high negative values of reduction potentials

Their ionization potentials are lowest

Their reduction potentials are close to SHE

While balancing an equation by ion electron method, the number of oxygen atoms are balanced by

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OH^-

H₂O

O₂

H⁺

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

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1.08 g

2.16 g

0.54 g

0.27 g

Pick out the wrong statement. In electrochemical cell

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Electrons are released at anode

Cathode is regarded as negative electrode

Chemical energy is converted into electrical energy

Salt bridge maintains the electrical neutrality of the solution

Cell potential depends upon :

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Concentration of ions

Nature of electrolyte

Temperature

All of 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.

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

Calculate the amount of charge flowing in 2 minute in a wire of resistance 10Ωwhen a potential difference of 20 V is applied

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120 C

240 C

20 C

4 C

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

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.

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

Prevention of corrosion of iron by Zn coating is called

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Galvanization

Cathodic protection

Electrolysis

Photoelectrolysis

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

A dry alkaline cell has porous Zn anode and MnO₂as cathode the electrolyte used is

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Ca(OH)₂

NaOH

KOH

NH₄OH

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Iodine can oxidise iron

Bromine can oxidise iron

Iodine can oxidise bromine

Iron can oxidise bromine

The oxidation state of an element is zero when

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It forms an oxide

It forms hydride

It is in free state

Only for noble gases

Which statement is correct for the fuel cells

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These cells operate at low temperature

No catalyst used for the formation of water

MnO₂is used as electrolyte

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

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