Daily Practice Problems Redox Reactions

Question1.

Which of the following is redox reaction?

1) H₂SO₄ with NaOH

2) In atmosphere, O₃ from O₂ by lightening

3) Formation of Nitrogen monoxide from Nitrogen and oxygen by lightening

4) Evaporation of H₂O

Question2.

A compound contains atoms of three elements A, B and C. Oxidation number of A is +2, B is +5 and that of C is -2, then possible formula of the compound is

1) A₂(BC₃)₂

2) A₃(BC₄)₂

3) A₃(B₄C)₂

4) ABC₂

Question3.

Oxidation number of oxygen atom in O₂^2-ion is

a) -1

b) -4

c) -3

d) -2

Question4.

Which of the following element has same oxidation state in all of its compound?

1) H

2) O

3) C

4) F

Question5.

Match the different compounds of Mn with oxidation number of Mn in those compounds.

Compounds of Mn Oxidation No. of Mn

1) Mn(HCO₃)₂ a) +3

2) Mn₂O₃b) +2

3) MnO₂c) +6

4) K₂MnO₄d) +7

5) MnO₃HSO₄e) +4

Question6.

In a reaction, KCl is converted into KClO₄. Oxidation number of Cl in KClO₄ is

a) +3

b) +5

c) +7

d) +1

Question7.

If 10g V₂O₅is dissolved in acid and reduced to V²⁺by treatment with zinc metal, how many moles of I₂could be reduced by the resulting V²⁺solution, as it is oxidised to V⁴⁺?

Atomic mass of (V = 51)

V₂O₅ + 10H⁺+ 6e^- 2V²⁺+ 5H₂O

V²⁺+ I₂+ H₂O 2I^-+ VO²⁺+ 2H⁺

Question8.

Highest oxidation number exhibited by main group elements other than first two groups is given by:

1) Group Number

2) Group Number – 8

3) Group Number – 10

4) Group Number – 2

Question9.

Which of the following elements does not show disproportionation tendency?

(i) P

(ii) Br

(iii) F

(iv) S

Question10.

Write balanced chemical equation for the following reaction: Permanganate ion (MnO₄^–) reacts with sulphur dioxide gas in acidic medium to produce Mn²⁺ and hydrogensulphate ion. (Balance by oxidation number method)

Question11.

Write balanced chemical equation for the following reaction: Reaction of liquid hydrazine (N₂H₄) with chlorate ion (ClO₃^–) in basic medium produces nitric oxide gas and chloride ion in gaseous state. (Balance by ion electron method)

Question12.

Which of the following reaction is not a redox reaction?(Heat is provided in each case)

1) C + O₂ $\to$ CO₂

2) 2KClO₃ $\to$ 2KCl + 3O₂

3) V₂O₅ + 5Ca $\to$ 2V + 5CaO

4) CaCO₃ $\to$ CaO + CO₂

Question13.

Using stock notation represent the following compounds:

1) V₂O₅

2) Cu₂O.

Question14.

Calculate the oxidation number of phosphorus in the following species.

1) PH₃

2) H₂PO₂^-

Question15.

What is redox couple?

Question16.

A negative Standard Electrode Potential means that the redox couple is

1) weaker reducing agent than the H⁺/H₂ couple.

2) stronger reducing agent than the H⁺/H₂ couple.

3) stronger oxidising agent than the H⁺/H₂ couple.

4) weaker oxidising agent than the H⁺/H₂ couple.

Question17.

What is salt bridge? What is its use?

Question18.

The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is correct in this respect?

(i) The oxidation number of hydrogen is always +1.

(ii) The algebraic sum of all the oxidation numbers in a compound is not equal to zero.

(iii) An element in the free or the uncombined state bears oxidation number zero.

(iv) In all its compounds, the oxidation number of chlorine is – 1.

Question19.

Using given standard electrode potentials, find out whether redox reaction between Fe³⁺

& Cu is feasible or not.

Standard electrode potential values: Fe³⁺/Fe²⁺= +0.77 V; Cu²⁺/Cu = +0.34 V

Question20.

By using standard electrode potentials, arrange the metals in decreasing order of their

reducing power.

Zn²⁺/Zn = -0.76 V

Ca²⁺/Ca= -2.87 V

Pb²⁺/Pb = -0.13 V

Ni²⁺/Ni = -0.25 V

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