Consider the table of standard reduction potentials shown below. Half-reaction $$E^{\circ}$$ $$Cl_{2} + 2e^{-}\rightarrow 2Cl^{-}$$ $$1.36\ V$$ $$O_{2} + 4H^{+} + 4e^{-} \rightarrow 2H_{2}O$$ $$1.23\ V$$ $$2H_{2}O + 2e^{-} \rightarrow H_{2} + 2OH^{-}$$ $$-0.83\ V$$ $$Rb^{+} + e^{-} \rightarrow Rb$$ $$-2.93\ V$$ Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

$$2Rb^{+} + 2Cl^{-} \rightarrow 2Rb + Cl_{2}$$

$$2H_{2}O \rightarrow 2H_{2} + O_{2}$$

$$H_{2} + 2OH^{-} + 2Rb^{+} \rightarrow 2Rb + 2H_{2}O$$

$$4Cl^{-} + O_{2} + 4H^{+} \rightarrow 2H_{2}O + 2Cl_{2}$$

Fill up the table from the given choice. Element Oxidation number Oxygen -2 in most compounds ____(i) in $$H_2O_2$$ and _____(ii) in $$ OF_2$$ Halogen -1 for_____(iii) in all its compounds Hydrogen _____(iv) in most of its compounds ______(v)in binary metallic hydrides Sulphur ______(vi) in all sulphides

$$(i) -1 (ii) +2 (iii) F (iv) +1 (v) -1 (vi) -2 $$

$$(i) +1 (ii) +1 (iii) Cl (iv) +1 (v) -1 (vi) +2 $$

$$(i) -1 (ii) +1 (iii) F (iv) +1 (v) +2 (vi) +2$$

$$(i) +1 (ii) +2 (iii) Cl (iv) +1 (v) +1 (vi) +6$$

Match the column I with column II with the type of reaction and mark the appropriate choice. Column I Column II $$(A)$$ $$3Mg_(s) + N_{2(g)}\xrightarrow{\Delta } Mg_3N_{2(s)}$$ $$(i)$$ Displacement $$(B)$$ $$NaH_(s) + H_2O_(l)\rightarrow NaOH_{(aq)} + H_{2(g)}$$ $$(ii)$$ Decomposition $$(C)$$ $$3Cl{ O }_{( aq) }^{ - }\rightarrow 2C{ l}_{( aq) }^{ - } + Cl{ O_3 }_{ (aq) }^{ - }$$ $$(iii)$$ Combination $$(D)$$ $$2KClO_{3(s)}\rightarrow 2KCl_(s) + 3O_{2(g)}$$ $$(iv)$$ Disproportionation

$$(A)\rightarrow (iii) , (B)\rightarrow (i) , (C)\rightarrow (iv) ,D\rightarrow (ii)$$

$$(A)\rightarrow (i) , (B)\rightarrow (iii) , (C)\rightarrow (ii) ,D\rightarrow (iv)$$

$$(A)\rightarrow (iv) , (B)\rightarrow (iii) , (C)\rightarrow (ii) ,D\rightarrow (i)$$

$$(A)\rightarrow (ii) , (B)\rightarrow (i) , (C)\rightarrow (iii) ,D\rightarrow (iv)$$

MCQ Questions for Class 11 Medical Chemistry Redox Reactions Quiz 12

Statement 1 : The oxidation state of $$\displaystyle Cr$$ in $$\displaystyle { { Al }_{ 2 }\left( { Cr }_{ 2 }{ O }_{ 7 } \right) }_{ 3 }$$ is +3.
Statement 2 : As a neutral compound, the sum of oxidation numbers of all the atoms must equal to zero.

0%

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.
0%

Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
0%

Statement 1 is correct but Statement 2 is not correct.
0%

Statement 1 is not correct but Statement 2 is correct.
0%

Both the Statement 1 and Statement 2 are not correct.

Which one has the highest oxidation number ?

0%
$$NO$$
0%
$$N_2O$$
0%
$$NO_2$$
0%
$$N_2O_4$$
0%
$$NO_{3}{^-}$$

Oxidation number of iodine in $${ IO }_{ 3 }^{ - }, { IO }_{ 4 }^{ - }, KI$$ and $$I_2$$ respectively is _____

0%
-2, -5, -1 ,0.
0%
+5, +7, -1 , 0.
0%
+2, +5, +1 , 0.
0%
-1, +1 , 0, +1.

$$\displaystyle 2Al\left( s \right) +6HCl\left( aq \right) \rightarrow 2{ Al }^{ 3+ }\left( aq \right) +6{ Cl }^{ - }\left( aq \right) +3{ H }_{ 2 }\left( g \right) $$
Which of the following is correct about the above reaction?

0%
Precipitation reaction
0%
Acid/base reaction
0%
Redox reaction
0%
Combustion reaction
0%
Decomposition reaction

Consider the table of standard reduction potentials shown below.

Half-reaction	$$E^{\circ}$$
$$Cl_{2} + 2e^{-}\rightarrow 2Cl^{-}$$	$$1.36\ V$$
$$O_{2} + 4H^{+} + 4e^{-} \rightarrow 2H_{2}O$$	$$1.23\ V$$
$$2H_{2}O + 2e^{-} \rightarrow H_{2} + 2OH^{-}$$	$$-0.83\ V$$
$$Rb^{+} + e^{-} \rightarrow Rb$$	$$-2.93\ V$$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

0%
$$2Rb^{+} + 2Cl^{-} \rightarrow 2Rb + Cl_{2}$$
0%
$$2H_{2}O \rightarrow 2H_{2} + O_{2}$$
0%
$$H_{2} + 2OH^{-} + 2Rb^{+} \rightarrow 2Rb + 2H_{2}O$$
0%
$$4Cl^{-} + O_{2} + 4H^{+} \rightarrow 2H_{2}O + 2Cl_{2}$$

A steady current of $$10.0$$ Amps is passed through a nickel production cell of $$15$$ minutes.
Which of the following is the correct expression for calculating the number of grams of nickel produced?
Note:
$$\bullet 1\ faraday = 96,500\ Coulombs$$
$$\bullet$$ The electroytic cell involves the following half-reaction:
$$Ni_{(aq)}^{2+} + 2e^{-} \rightarrow Ni_{(s)}$$

0%
$$\dfrac {(10.0)(15)(96,500)}{(59)(60)} g$$
0%
$$\dfrac {(10.0)(15)(59)}{(60)(96,500)} g$$
0%
$$\dfrac {(10.0)(15)(60)(59)}{(96,500)(2)} g$$
0%
$$\dfrac {(96,500)(59)}{(10)(15)(60)(2)} g$$

Oxidation number of the nitrogen atom in $$HNO_3$$ is :

0%
-1
0%
+1
0%
0
0%
+4
0%
+5

Match the List - I with List - II and select the correct matching from the codes given below:

Column - I	Column - II
A. $$NaN_3$$	+5
B. $$N_2H_4$$	+1
C. $$NH_2OH$$	-1/3
D. $$N_2O_5$$	-2

0%
A-3 B-4 C-2 D-1
0%
A-4 B-3 C-1 D-2
0%
A-3 B-4 C-1 D-2
0%
A-4 B-3 C-2 D-1

For the redox process,
$$Zn(s) + Cu^{2+} \rightleftharpoons Zn^{2} + Cu(s)\ E_{cell}^{\circ} = + 1.10\ V$$
which graph correctly represents $$E_{cell}$$ (Y-axis) as a function of $$\log \dfrac {[Zn^{2+}]}{[Cu^{2+}]}$$ (X-axis)?

The Metal with the highest oxidation state present in $$K_2CrO_4$$, $$NbCl_5$$ and $$MnO_2$$ is:

0%
$$Nb$$
0%
$$Mn$$
0%
$$K$$
0%
$$Cr$$

Oxidation number of N in $$NH_4NO_3$$ is:

0%
$$-3$$
0%
$$+5$$
0%
$$-3$$ and $$+5$$
0%
$$+3$$ and $$-5$$

A mixture of potassium chlorate, oxalic acid and sulphuric acid is heated. During the reaction which element undergoes maximum change in the oxidation number?

0%
Cl
0%
C
0%
S
0%
H

Among the following, identify the species with an atom in $$+6$$ oxidation state.

0%
$$MnO^-_4$$
0%
$$Cr(CN)^{3-}_6$$
0%
$$NiF^{2-}_6$$
0%
$$CrO_2Cl_2$$

The oxidation numbers of the sulphur atoms in peroxomonosulphuric acid $$(H_{2}SO_{5})$$ and peroxodisulphuric acid $$(H_{2}S_{2}O_{8})$$ are respectively

0%
$$+8$$ and $$+7$$
0%
$$+3$$ and $$+3$$
0%
$$+6$$ and $$+6$$
0%
$$+4$$ and $$+6$$

$$CH_3COOH$$ is neutralized by $$NaOH$$. Conductometric titration curve will be of the type:

Fill up the table from the given choice.

Element	Oxidation number
Oxygen	-2 in most compounds ____(i) in $$H_2O_2$$ and _____(ii) in $$ OF_2$$
Halogen	-1 for_____(iii) in all its compounds
Hydrogen	_____(iv) in most of its compounds ______(v)in binary metallic hydrides
Sulphur	______(vi) in all sulphides

0%
$$(i) +1 (ii) +1 (iii) Cl (iv) +1 (v) -1 (vi) +2 $$
0%
$$(i) -1 (ii) +2 (iii) F (iv) +1 (v) -1 (vi) -2 $$
0%
$$(i) -1 (ii) +1 (iii) F (iv) +1 (v) +2 (vi) +2$$
0%
$$(i) +1 (ii) +2 (iii) Cl (iv) +1 (v) +1 (vi) +6$$

In the reaction, $$4Fe+{ 3O }_{ 2 }\rightarrow { 4Fe }^{ 3+ }+{ 6O }^{ 2- } $$ which of the following statement is incorrect?

0%
It is redox reaction
0%
Metallic iron is a reducing agent
0%
$${ Fe }^{ 3+ }$$ is an oxidising agent
0%
Metallic iron is reduced to $${ Fe }^{ 3+ }$$

$${ H }_{ 2 }{ O }_{ 2 }(aq)+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { O }_{ 2 }(g)+{ Cr }^{ 3+ }(aq)$$

This reaction occurs in acidic medium.

0%
True
0%
False

Arrange the following in increasing order of oxidation state of $$Ni$$.
$$K_2[Ni(CN)_4],K_2[NiF_6],Ni(CO)_4$$

0%
$$Ni(CO)_4,K_2[Ni(CN)_4],K_2[NiF_6]$$
0%
$$K_2[Ni(CN)_4],Ni(CO)_4,K_2[NiF_6]$$
0%
$$Ni(CO)_4,K_2[NiF_6],K_2[Ni(CN)_4]$$
0%
$$K_2[NiF_6],K_2[Ni(CN)_4],K_2[Ni(CN)_4]"$$

When a piece of sodium metal is dropped in water, hydrogen gas evolved because:

0%
sodium is reduced and acts as an oxidising agent
0%
water is oxidised and acts as a reducing agent
0%
sodium loses electrons and is oxidised while water in reduced
0%
water loses electrons and is oxidised to hydrogen

For the redox reaction, $$MnO_{4}^{-} + C_{2}O_{4}^{2-} + H^{+}\rightarrow Mn^{2+} + CO_{2} + H_{2}O$$, the correct coefficients of the reactants for the balanced equation are _____________.

0%
$$MnO_{4}^{-} = 2, C_{2}O_{4}^{2-} = 16, H^{+} = 5$$
0%
$$MnO_{4}^{-} = 16, C_{2}O_{4}^{2-} = 5, H^{+} = 2$$
0%
$$MnO_{4}^{-} = 5, C_{2}O_{4}^{2-} = 16, H^{+} = 2$$
0%
$$MnO_{4}^{-} = 2, C_{2}O_{4}^{2-} = 5, H^{+} = 16$$

In the chemical reaction
$${ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }+x{ H }_{ 2 }{ SO }_{ 4 }+y{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ Cr }_{ 2 }{ \left( { SO }_{ 4 } \right) }_{ 3 }+z{ H }_{ 2 }O$$
Values of x, y and z are:

0%
1, 3, 1
0%
4, 1, 4
0%
3, 2, 3
0%
2, 1, 2

A metal, M forms chlorides in its +2 and +4 oxidation states. Which of the following statements about these chlorides is correct?

0%
$$MCl_2$$ is less ionic than $$MCl_4$$
0%
$$MCl_2$$ is less easily hydrolysed than $$MCl_4$$
0%
$$MCl_2$$ is more volatile than $$MCl_4$$
0%
$$MCl_2$$ is more soluble in anhydrous ethanol than $$MCl_4$$

Which of the following reaction(s) is/are example(s) of intra-redox reaction?

0%
$$2NaAg{\left( {CN} \right)_2} + Zn \to N{a_2}Zn{\left( {CN} \right)_4} + 2Ag$$
0%
$$Ba{O_2} + {H_2}S{O_4} \to BaS{O_4} + {H_2}O$$
0%
$${N_2}{O_5} + {H_2}O \to 2HN{O_3}$$
0%
$$AgN{O_3} + KI \to AgI + KN{O_3}$$

For the redox reaction:

$$Zn+N{ O }^-_3\rightarrow Zn^{2+}+NH^+_4$$

in a basic medium, coefficients of $$Zn, \ NO^-_3$$ and $$OH^-$$ in the balanced equation respectively are:

0%
$$4, 1, 7$$
0%
$$7, 4, 1$$
0%
$$4, 1, 10$$
0%
$$1, 4, 10$$

Half cell reactions for some electrodes are given below:

I. $$A+{ e }^{ - }\longrightarrow { A }^{ - }\ ;\quad \quad \ { E }^{ 0 }=0.96V$$

II. $${ B }^{ - }+{ e }^{ - }\longrightarrow { B }^{ 2- }\ ;\quad { E }^{ o }=-0.12V$$
III. $${ C }^{ + }+{ e }^{ - }\longrightarrow C\ ;\quad \ { E }^{ o }=+0.18V$$

IV. $${ D }^{ 2+ }+{ 2e }^{ - }\longrightarrow D\ ;\quad { E }^{ o }=-1.12V$$

The largest potential will be generated in which cell?

0%
$${ A }^{ - }|A\parallel { B }^{ - }|{ B }^{ 2 }$$
0%
$$D|{ D }^{ 2+ }\parallel A|{ A }^{ - }$$
0%
$${ B }^{ 2 }|{ B }^{ - }\parallel { C }^{ + }|C$$
0%
$$D|{ D }^{ 2+ }\parallel { C }^{ + }|C$$

Match the column I with column II with the type of reaction and mark the appropriate choice.

	Column I		Column II
$$(A)$$	$$3Mg_(s) + N_{2(g)}\xrightarrow{\Delta } Mg_3N_{2(s)}$$	$$(i)$$	Displacement
$$(B)$$	$$NaH_(s) + H_2O_(l)\rightarrow NaOH_{(aq)} + H_{2(g)}$$	$$(ii)$$	Decomposition
$$(C)$$	$$3Cl{ O }_{( aq) }^{ - }\rightarrow 2C{ l}_{( aq) }^{ - } + Cl{ O_3 }_{ (aq) }^{ - }$$	$$(iii)$$	Combination
$$(D)$$	$$2KClO_{3(s)}\rightarrow 2KCl_(s) + 3O_{2(g)}$$	$$(iv)$$	Disproportionation

0%
$$(A)\rightarrow (i) , (B)\rightarrow (iii) , (C)\rightarrow (ii) ,D\rightarrow (iv)$$
0%
$$(A)\rightarrow (iv) , (B)\rightarrow (iii) , (C)\rightarrow (ii) ,D\rightarrow (i)$$
0%
$$(A)\rightarrow (ii) , (B)\rightarrow (i) , (C)\rightarrow (iii) ,D\rightarrow (iv)$$
0%
$$(A)\rightarrow (iii) , (B)\rightarrow (i) , (C)\rightarrow (iv) ,D\rightarrow (ii)$$

$$KMnO_4$$ acts as an oxidizing agent in acidic medium. The number of moles of $$KMnO_4$$ that will be needed to react with one mole of sulphide ions in acidic solution is:

0%
$$\dfrac{2}{5}$$
0%
$$\dfrac{3}{5}$$
0%
$$\dfrac{4}{5}$$
0%
$$\dfrac{1}{5}$$

In the electrolysis of aqueous sodium chloride solution which of the half-cell reaction will occur at the anode?

0%
$$Na^+_{(aq)}+e^-\rightarrow Na_{(s)}; E^o_{cell}=-2.71$$V
0%
$$2H_2O_{(l)}\rightarrow O_{2(g)}+4H^+_{(aq)}+4e^-; E^o_{cell}=1.23$$V
0%
$$H^+_{aq}+e^-\rightarrow \dfrac{1}{2}H_{2(g)}; E^o_{cell}=0.00$$V
0%
$$Cl^-_{(aq)}\rightarrow \dfrac{1}{2}Cl_{2(g)}+e^-; E^o_{cell}=1.36$$V

Which of the following is $$\textbf{not}$$ an example of redox reaction?

0%
$$CuO + H_{2} \rightarrow Cu + H_{2}O$$
0%
$$Fe_{2}O_{3} + 3CO \rightarrow 2Fe + 3CO_{2}$$
0%
$$2K + F_{2} \rightarrow 2KF$$
0%
$$BaCl_{2} + H_{2}SO_{4} \rightarrow BaSO_{4} + 2HCl$$

Based on the cell notation for spontaneous reaction, at the anode:
$$Ag(s)|AgCl(s)|{ Cl }^{ - }(aq)\parallel { Br }^{ - }(aq)|{ Br }_{ 2 }(I)|C(s)$$

0%
$$AgCl$$ gets reduced
0%
$$Ag$$ gets oxidized
0%
$${ Br }^{ - }$$ gets oxidized
0%
$${ Br }_{ 2 }$$ gets reduced

The oxidation number and coordination number of $$M$$ in the compound, $$[M(SO_4)(NH_3)_5]$$ will be:

0%
10 and 3
0%
1 and 6
0%
6 and 4
0%
2 and 6

The magnetic moment of $$M^{x+}$$ (atomic number $$= 25$$) is $$\sqrt{15}$$ . Then, the oxidation number $$x$$ of $$M$$ is:

0%
4
0%
3
0%
2
0%
none of these

Oxidation number of $$'Co'$$ in $$Hg[Co(SCN)_{4}]$$

0%
$$+2$$
0%
$$+1$$
0%
$$+3$$
0%
$$+5$$

In acid medium, the standard reduction potential of $$NO$$ converted to $${ N }_{ 2 }O$$ is $$1.59 V$$. Its standard potential in alkaline medium would be:

0%
$$-1.59 V$$
0%
$$-0.764 V$$
0%
$$0.764 V$$
0%
$$0.062 V$$

Write balanced equations for the half reactions and calculate the reduction potentials at $$25^0C$$ for the following half cells :
$$Cl^-(1.2M) | Cl_2(g, 3.6 atm) | Pt E^o = 1.36 V$$

0%
$$1.372 V$$
0%
$$1.363 V$$
0%
$$1.358 V$$
0%
$$1.342 V$$

The pair of compounds in which both the metals are in the highest possible oxidation state is

0%
$$FeSO_{4},CuS_{2}$$
0%
$$CrO_{2}Cl_{2}, MnO_{4}^{-}$$
0%
$$TiO_{2},MnO_{2}$$
0%
$$[Co(CN_{3})]^{3-}, MnO_{3}$$

Oxidation number of Cl in $$KClO_3$$ :

0%
-1
0%
-5
0%
+1
0%
+5

In the given reaction, the increase in the oxidation number of sulphur is:

$${H_2}{O_2} + PbS \to {H_2}O + PbS{O_4}$$

0%
$$2$$ units
0%
$$4$$ units
0%
$$6$$ units
0%
$$8$$ units

The oxidation state of A,B and C in compaund are -2, +5, and -2, respectively. the compound is ?

0%
$$A_3( BC)_{2}$$
0%
$$A_2( BC )_{3}$$
0%
$$A_2 ( BC )_{4}$$
0%
$$A_2 ( BC )_{5}$$

Justify that the following reactions are redox reactions.

0%
$$CuO\left( s \right) +{ H }_{ 2 }\left( g \right) \rightarrow Cu\left( s \right) +{ H }_{ 2 }O\left( g \right) $$
0%
$${ Fe }_{ 2 }{ O }_{ 3 }\left( s \right) +3CO\left( g \right) \rightarrow 2Fe\left( s \right) +3{ CO }_{ 2 }\left( g \right) $$
0%
$$4{BCl }_{ 3 }\left( g \right) +3Li{AlH }_{ 4 }\left( s \right) \rightarrow 2{ B }_{ 2 }{ H }_{ 6 }\left( s \right) +3LiCl\left( s \right)+3{AlCl }_{ 3 }\left( s \right) $$
0%
$$2K\left( s \right) +{ F }_{ 2 }\left( g \right) \rightarrow { 2K }^{ + }{ F }^{ - }\left( s \right)$$

Which of the following is a redox

0%
$$2NaAg(CN{ ) }_{ 2 }+Zn\quad \longrightarrow N{ a }_{ 2 }Zn(CN{ ) }_{ 4 }+2\quad Ag$$
0%
$$Ba{ O }_{ 2 }+{ H }_{ 2 }S{ O }_{ 4 }\quad \longrightarrow BaS{ O }_{ 4 }+{ H }_{ 2 }{ O }_{ 2 }$$
0%
$${ N }_{ 2 }{ O }_{ 5 }+{ H }_{ 2 }O\longrightarrow 2HN{ O }_{ 3 }$$
0%
$$AgN{ O }_{ 3 }+KI\longrightarrow AgI+KN{ O }_{ 3 }\\ $$

In the balanced equation
$${MnO_{4}}^{-}+H^{+}+{C_{2}O_{4}}^{2-}\rightarrow Mn^{2+}+CO_{2}+H_{2}O$$, the moles of $$CO_{2}$$ formed are :-

0%
2
0%
4
0%
5
0%
10

Oxidation numbers of $$P$$ in $$PO_{4}^{3-}$$ , $$S$$ in $$SO_{4}^{2-}$$ and that of $$Cr$$ in $$Cr_{2}O_{7}^{2-}$$ are respectively::

0%
+3, +6 and +5
0%
+5, +3 and +6
0%
-3, +6 and +6
0%
+5, +6 and +6

Which of the following is a strong oxidising agent?

0%
$$AlCl_{3}$$
0%
$$TlCl_{3}$$
0%
$$NF_{3}$$
0%
$$PCl_{3}$$

What is the oxidation number of xenon(Xe) in the $$Ba_2XeO_6$$?

0%
ZERO
0%
+8
0%
+6
0%
None of these

A compound contains three elements A,B and C, if the oxidation number of $$A=+2, B=+5$$ and $$C= -2,$$ the possible formula of the compound is :

0%
$$A_3(B_4C)_2$$
0%
$$A_3(BC_4)_2$$
0%
$$A_2(BC_3)_2$$
0%
$$ABC_2$$

The formal charge on carbon atom in carbonate ion is

0%
$$+1$$
0%
$$-1$$
0%
$$+4$$
0%
$$Zero$$

The compound $$YBa_2Cu_3O_7$$, which shows super conductivity, has copper in the oxidation state:

0%
$$+\dfrac{7}{3}$$
0%
$$+\dfrac{3}{7}$$
0%
$$3$$
0%
$$7$$

The value of n in the molecular formula $$Be_n Al_{2}Si_{6}O_{18}$$ is

0%
1
0%
2
0%
3
0%
4

	Column I	Column II	Reason
$$A$$	$$3Mg(s)+N_2(g) \rightarrow Mg_3N_2(s)$$	(iii) Combination	A combination reaction is defined as a chemical reaction in which two or more substances combine to form a single substance under suitable conditions.
$$B$$	$$NaH(s)+H_2O(l)\rightarrow NaOH(aq)+H_2(g)$$	(i) Displacement	Displacement reaction is a chemical reaction in which a more reactive element (NaH) displaces a less reactive element ($$H_2O \rightarrow H_2$$) from its compound. Both metals and non-metals take part in displacement reactions.
$$C$$	$$3ClO^−(aq) \rightarrow 2Cl^−(aq)+ClO_3^−(aq)$$	(iv) Disproportionation	Disproportionation reaction is a redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states as: $$3\overset {+1}{Cl}O^−(aq) \rightarrow 2\overset {-1}{Cl^−}(aq)+\overset {+5}{Cl}O_3^−(aq)$$
$$D$$	$$2KClO_3(s) \rightarrow 2KCl(s)+3O_2(g)$$	(ii) Decomposition	A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more elements or new compounds.

CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 12 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 12 - MCQExams.com

0:0:1

Practice Class 11 Medical Chemistry Quiz Questions and Answers

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