Question # 1

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

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

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Iodine can oxidise iron

Bromine can oxidise iron

Iodine can oxidise bromine

Iron can oxidise bromine

Electrolytes in the form of solution or in the fused state have the ability to conduct :

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Light.

Electricity.

Ions.

Electrons.

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

96500 C of electricity liberates from CuSO₄solution

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63.5 g of Cu

31.75 g of Cu

96500 g of Cu

100 g of Cu

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

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

Which statement is incorrect about standard hydrogen electrode

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Its oxidation and reduction potential is zero

It consists of Pt wire dipped on 1 molar HCI solution

The electrolyte is 1 molar NaOH solution

H₂gas is passes in it at 1 atmospheric pressure

Same amount of electric current is passed through solutions of AgNO₃and 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

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112 cm³

22400 cm³

224 cm³

1.008 g

Metals like Fe, Mg, Al, Cr, Zn have more negative reduction potentials that is whey

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These don't react with steam

These react very slowly with steam to liberate H₂gas

These react rapidly with steam to produce the metallic oxides and liberate H₂gas

These react with cold water violently

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

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

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A strong reducing agent

A strong oxidising agent

Better oxidising agent than hydrogen

Less reducing agent than hydrogen

Reaction takes place at anode is

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Ionization

Reduction

Oxidation

Hydrolysis

Oxidation number of oxygen in OF₂is

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+1

-1

+2

-2

Zn does not displace Mg from MgSO₄solution because

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Zn is more electropositive than Mg

Zn is below Mg in electropositive series

Zn is above Mg in electrochemical series

Zn is trivalent Mg is divalent

In KO₂the oxidation state of oxygen is

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-2

-1

+1/2

-1/2

A cell in which spontaneous redox reaction generates an electric current is called

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Electrolytic cell

Electrochemical cell

Voltaic or Galvanic cell

Biological cell

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

Which of the following will be good conductor of electricity

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Pure distilled water

Molten NaCl

Dilute solution of glucose

Chloroform

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)

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0.399 V

0.281 V

0.222 V

0.176 V

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Fe is reduced

Fe is oxidized

Cl₂is oxidized

None of these

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

Pure water does not conduct electricity because it

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Has low boiling point

Is almost unionized

Is neutral

Is readily decomposed

Ionization is the process in which ionic compounds when fused or dissolved in water split up into charged particles called :

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Atoms.

Electrons.

Protons .

Ions

Strong reducing agents gave

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Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

Lesser positive value of standard reaction potential

None of these

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

The conversion of chemical energy into electrical energy requires :

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Electrolytic cell

Galvanic cell

Voltaic cell

Both (b) and (c)

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

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

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