Question # 1

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 redox reaction an oxidizing agent

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Gains electrons

Is oxidized

Loses electrons

Hydrolysed

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

Specific conductivity of a solution

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Increases with dilution

Decreases with dilution

Remains unchanged with dilution

Depends on mass of electrolyte

Electrolysis is used for :

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Manufacture of caustic soda

Refining of copper

Electroplating

All of above

The conductivity of strong electrolyte

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Increases on dilution slightly

Does not change on dilution

Decreases on dilution

Depends on density of electrolyte it self

The cell which generates electricity as a result of spontaneous oxidation-reduction reaction is called

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Electrolytic cell

Nelson's cell

Galvanic cell

Down's cell

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Iodine can oxidise iron

Bromine can oxidise iron

Iodine can oxidise bromine

Iron can oxidise bromine

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 substance having highest conductivity at room temperature among the following is

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0.1 N HCl

0.1 N NaCl

Graphite

Glass

Strong oxidizing agents have

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Greater positive value of standard reduction potential

Lesser positive value of standard

Greater negative value of standard

None of these

The electrolysis of CuSO₄aqueous solution using copper as cathode as well an anode the substance which deposits at cathode is

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H₂SO₄

Oxygen

Copper

Hydrogen

Which of the following statements is true about Galvanic cell

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Anode is negatively charged

Reduction occurs at anode

Cathode is positively charge

Reduction occurs at cathode

A standard hydrogen electrode is used as standard electrode of which electrode potential is arbitrarily taken as

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+1

-1

0.1

Zero

The value of SHE is cathode and anode is always taken to be

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One

Zero

Different

Same

The oxidation number of free element is always taken to be

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0

1

2

-1

The specific conductance of 0.1 M NaCl solution is 1.06 x 10^-2ohm^-1mol^-1. Its molar conductance in ohm^-1cm²mol^-1is

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1.06 x 10²

1.06 x 10³

1.06 x 10⁴

53

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

In lead accumulator the electrolyte is H₂SO₄solution is

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30% H₂SO₄

60% H₂SO₄

80% H₂SO₄

90% H₂SO₄

Pure water does not conduct electricity because it

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Has low boiling point

Is almost unionized

Is neutral

Is readily decomposed

F₂, Cl₂, Br₂and l₂lie below SHE is the Electro chemical series that is why these

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Undergo reduction

Undergo oxidation

Liberate H₂gas with steam

None of these

A solution of sodium sulphate was electrolysed using some insert electrodes. The products at the electrodes are

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O₂, H₂

O₂, Na

O₂, SO₂

O₂, S₂O₈²

Oxidation number of oxygen in OF₂is

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+1

-1

+2

-2

The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm^-1cm^-1. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

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0.142 cm^-1

0.66 cm^-1

0.916 cm^-1

1.12 cm^-1

Which of the following (1 M) conducts more electricity?

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Sulphuric acid

Boric acid

Nitric acid

Phosphorus acid

Which of the following is the use of electrolysis?

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Eletrorefining

Electroplating

Both A and B

None of the above

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

An electrochemical cell is based upon

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Acid-base reaction

Redox reaction

Nuclear reaction

None of the above

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

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.

When fused PbBr2 is electrolyzed :

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Lead appears at anode.

Lead appears at cathode.

Bromine appears at cathode.

Lead appears at both electrodes.

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