CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 8 - MCQExams.com

Examples of few compounds in a particular oxidation state are given . Mark the example which is not correct.
  • Phosphorus in +1 oxidation state - $$H_3PO_2$$
  • Chlorine in +7 oxidation state - $$HClO$$
  • Chromium in +6 oxidation state -$$ CrO_2Cl_2$$
  • Carbon in 0 oxidation state - $$C_{12}H_{22}O_{11}$$
Which of the following oxidation numbers is not correctly matched?
  • $$P$$ in $$ NaH_2PO_4 = +5$$
  • $$Ni$$  in $$ [ Ni(CN)_6]^{4-} = +2$$
  • $$P$$ in $$Mg_2P_2O_7 = +6$$
  • $$Cr$$ in $$(NH_4)_2Cr_2O_7 =+6$$
Oxidation number of sulphur in peroxomonosulphuric acid $$(H_2SO_5)$$ is:
  • +4
  • +2
  • +6
  • -2
In which of the following compounds oxidation state of chlorine has two different values?
  • $$CaCl_2$$
  • $$NaCl$$
  • $$CaOCl_2$$
  • $$CCl_4$$
Match the column I with column II and mark the appropriate choice.
Column I
( Compound )		Coloumn II
(Oxidation state of $$Fe$$)
( A )$$K_3[(Fe(OH)
_6]$$		(i)+8/3
( B )$$ K_2[FeO_4]$$(ii)+2
( C )$$FeSO_4, (NH_4)_2SO_46H_2O$$(iii)+3
( D)$$Fe_3O4$$(iv)+6
  • $$( A ) \rightarrow ( iii ) , ( B ) \rightarrow ( i ) , ( C ) \rightarrow ( ii ) ,( D ) \rightarrow ( iv )$$
  • $$( A ) \rightarrow ( iii ) , ( B ) \rightarrow ( iv ) , ( C ) \rightarrow ( ii ) ,( D ) \rightarrow ( i )$$
  • $$( A ) \rightarrow ( i ) , ( B ) \rightarrow ( iii ) , ( C ) \rightarrow ( ii ) ,( D ) \rightarrow ( iv )$$
  • $$( A ) \rightarrow ( iv ) , ( B ) \rightarrow ( ii ) , ( C ) \rightarrow ( i ) ,( D ) \rightarrow ( iii )$$
Mark the correct statement from the following.
  • Copper metal can be oxidised by $$Zn^{2+}$$ ions
  • Oxidation number of phosphorus in $$ P_4$$ is 4
  • An element in the highest oxidation state acts only as a reducing agent.
  • The element which shows highest oxidation number of +8 is $$OsO_4$$
The oxidation state of $$Fe$$ in $$K_4[Fe(CN)_6]$$ is:
  • +2
  • +3
  • +4
  • +6
In which of the following compounds carbon is in highest oxidation state?
  • $$CH_3Cl$$
  • $$CCl_4$$
  • $$CHCl_3$$
  • $$CH_2Cl_2$$
What is the oxidation state of $$P$$ in $$ Ba(H_2PO_2)_2$$?
  • +3
  • +2
  • +1
  • -1
What are the oxidation states of phosphorus in the following compounds?
$$H_3PO_2,H_3PO_4,Mg_2P_2O_7,PH_3,HPO_3$$
  • $$+1, +3, +3, +3, +5$$
  • $$+3, +3, +5, +5, +5$$
  • $$+1, +2 ,+3, +5, +5$$
  • $$+1, +5 ,+5 ,-3 , +5$$
The oxidation state of molybdenum in its oxo complex species$$ [Mo_2O_4(C_2H_4)_2(H_2O_2)]^{2-}]$$.
  • +2
  • +3
  • +4
  • +5
Which of the following reaction shows reduction of water? 
  • $$2H_2O+2Na\rightarrow 2NaOH+H_2$$
  • $$6CO_2+12H_2O\rightarrow C_6H_12O_6+6H_2O+6O_2$$
  • $$2F_2+2H_2O\rightarrow 4H^++4F^-+O_2$$
  • $$P_4O_10+6H_2O\rightarrow 4H_3PO_4$$
The sum of oxidation states of sulphur in $$H_2S_2O_8$$ is?
  • $$+2$$
  • $$+6$$
  • $$+7$$
  • $$+12$$
The correct sequence of the oxidation state of Fe, Ta, P and N elements in the given compounds are respectively :
$$ Na_2[Fe(CN)_5NO],\ K_2TaF_7,\ Mg_2P_2O_7,\ Na_2S_4O_6,\ N_3H$$
  • $$+3, +5 ,+5 .+2.5,-\frac { 1 }{ 3 }$$
  • $$+5,+3,+5,+3,+\frac { 1 }{ 3 }$$
  • $$+3, +3 ,+5 ,+5 ,-\frac { 1 }{ 3 }$$
  • $$+5 , +5 ,+3 ,+2.5, +\frac { 1 }{ 3 }$$
Which of the following arrangements represent increasing oxidation number of the central atom ?
  • $$CrO_{2}^{-}$$, $$ClO_{3}^{-}$$ ,$$CrO_{4}^{2-}$$, $$MnO_{4}^{-}$$,
  • $$ClO_{3}^{-}$$, $$CrO_{4}^{2-}$$, $$MnO_{4}^{-}$$, $$CrO_{2}^{-}$$,
  • $$CrO_{2}^{-}$$,$$ClO_{3}^{-}$$,$$MnO_{4}^{-}$$,$$CrO_{4}^{2-}$$,
  • $$CrO_{4}^{2-}$$,$$MnO_{4}^{-}$$,$$CrO_{2}^{-}$$,$$ClO_{3}^{-}$$,
The largest oxidation number exhibited by an element depends on its outer
electronic configuration. With which of the following outer electronic configurations
the element will exhibit the largest oxidation number?
  • $$3d^{1}4s^{2}$$
  • $$3d^{3}4s^{2}$$
  • $$3d^{5}4s^{1}$$
  • $$3d^{5}4s^{2}$$
In the reaction : $$I_2+2S_2{ O }_{ 3 }^{ 2- }\rightarrow 2I^- +S_4{ O }_{ 6 }^{ 2- }$$?
  • $$ I_2 $$ is reducing agent
  • $$ I_2 $$ is oxidising agent and $$ S_2{ O }_{ 3 }^{ 2- } $$ is reducing agent
  • $$ S_2{ O }_{ 3 }^{ 2- } $$ is oxidising agent
  • $$ I_2 $$ is reducing agent and $$ S_2{ O }_{ 3 }^{ 2- } $$ is oxidising agent
Calculate the oxidation number of underlined element in the given compound.
$$K[\underline{Co}(C_2O_4)_2(NH_3)_2]$$
  • +5
  • +6
  • +2
  • +3
Which of the following arrangements represent increasing oxidation number of the central atom?
  • $${CrO}_{2}^{-},{ClO}_{3}^{-},{CrO}_{4}^{2-},{MnO}_{4}^{-}$$
  • $${ClO}_{3}^{-},{CrO}_{4}^{2-},{MnO}_{4}^{-},{CrO}_{2}^{-}$$
  • $${CrO}_{2}^{-},{ClO}_{3}^{-},{MnO}_{4}^{-},{CrO}_{4}^{2-}$$
  • $${CrO}_{4}^{2-},{MnO}_{4}^{-},{CrO}_{2}^{-},{ClO}_{3}^{-}$$
$$H^+$$ ions are present in the balanced chemical equation of reaction in a basic medium.
Is the above statement true or false?
  • True
  • False
$$2OH^- + 2OCN^- + 3OCl^- \rightarrow  2CO_3{2^-} + N_2 + 3Cl^- + H_2O$$
This is the balanced chemical equation of the reaction in which medium?
  • Acidic
  • Basic
  • Neutral
  • Any of the above
In the reaction $$4Fe+3O_2\rightarrow 4Fe^{3+}+6O^{2-}$$ which of the following statements is incorrect?
  • It is a redox reaction
  • Metallic iron is a reducing agent
  • $$Fe^{3+}$$ is an oxidising agent
  • Metallic iron is reduced to $$Fe^{3+}$$
Oxidation number of $$Cr$$ in $$CrO_5$$ is:
  • $$+10$$
  • $$+6$$
  • $$+4$$
  • $$+5$$
In which of the following conditions is the potential for the following half-cell reaction maximum?
$$2H^+ + 2e^{-} \longrightarrow H_2$$
  • $$1.0 \,M \,HCl$$
  • A solution having $$pH = 4$$
  • Pure water
  • $$1.0 \,M \,NaOH$$
In the case of $$CH_3COOH$$, the oxidation number of carbon of the carboxylic group is:
  • $$-3$$
  • zero
  • $$+1$$
  • $$+3$$
The oxidation states of Cr in $$\left[ Cr\left( { H }_{ 2 }O \right)  \right] { Cl }_{ 3 },\left[ { Cr\left( { C }_{ 6 }{ H }_{ 6 } \right)  }_{ 2 } \right] ,$$ and $${ K }_{ 2 }\left[ Cr{ \left( CN \right)  }_{ 2 }{ \left( O \right)  }_{ 2 }{ \left( O \right)  }_{ 2 }\left( { NH }_{ 3 } \right)  \right] $$ respectively are :
  • +3,+4, and +6
  • +3,+2, and +4
  • +3, 0, and +6
  • +3, 0, and +4
For the redox reaction, $$Zn+Cu^{2+}_{(0.1M)}\rightarrow Zn^{2+}_{(1M)}+Cu$$ taking place in a cell $$E^{\ominus}_{cell}=1.10$$V. $$E^{\ominus}_{Cell}$$ for the galvanic cell will be?
  • $$2.14$$V
  • $$1.80$$V
  • $$1.07$$V
  • $$0.82$$V
When zinc reacts with very dilute $$HNO_3$$, the oxidation state of nitrogen changes from:
  • $$+5$$ to $$+1$$
  • $$+5$$ to $$-3$$
  • $$+5$$ to $$+4$$
  • $$+5$$ to $$+3$$
CompoundsO.N.
(A)$$KMn^*O_4$$(1)+4
(B)$$Ni^*(CO)_4$$(2)+7
(C)$$[Pt^*(NH_3)Cl_2]Cl_2$$(3)0
(D)$$Na_2O^*_2$$(4)-1
The correct code for the O.N. of asterisked atom would be:
  • A -1, B - 2, C - 3, D - 4
  • A -4, B - 3, C - 2, D - 1
  • A -2, B - 3, C - 1, D - 4
  • A -4, B - 1, C - 2, D - 3
The oxidation number of $$Pt$$ in $$[Pt({ C }_{ 2 }{ H }_{ 4 }{ ) }Cl_3]^{ - }$$ is:
  • $$+1$$
  • $$+2$$
  • $$+3$$
  • $$+4$$
The oxidation number of phosphorus vary from:
  • -3 to +5
  • -1 to +1
  • -3 to + 3
  • -5 to +1
Calculate the equilibrium constant for the redox reaction at $$25^o$$C, $$Sr_{(s)}+Mg^{2+}_{(aq)}\rightarrow Sr^{2+}_{(aq)}+Mg_{(s)}$$, that occurs in a galvanic cell. $$E^o_{{Mg^{2+}}/{Mg}}=-2.37$$V and $$E^o_{{Sr}^2+/Sr}=-2.89$$V.
  • $$2.69\times 10^{15}$$
  • $$2.69\times 10^{17}$$
  • $$3.69\times 10^{17}$$
  • $$3.69\times 10^{15}$$

In $$Ni{(CO) }_{ 4 }$$ the oxidation state of Ni is:
  • 4
  • 0
  • 2
  • 8
Two oxidation states for chlorine are found in the compound:
  • $${ CaOCl }_{ 2 }$$
  • $$KCL$$
  • $${ KClO }_{ 3 }$$
  • $${ Cl }_{ 2 }{ O }_{ 7 }$$
Oxidation state of cobalt in $$[{ Co }(NH_{ 3 }{ ) }_{ 4 } ({ H }_{ 2 }O)Cl]{ SO }_{ 4 }$$ ?
  • $$0$$
  • $$+4$$
  • $$-2$$
  • $$+3$$
Find the oxidation state of Cr in the given complex $$K_2[Cr(NO)(NH_3)(CN)_4]$$, $$\mu$$ = 1.73 BM.
  • + 1
  • + 2
  • +3
  • None of these
Oxidation number of $$Fe$$ in $${ Fe }_{ 3 }{ O }_{ 4 }$$ are:
  • $$+2$$ and $$+3$$
  • $$+1$$ and $$+2$$
  • $$+1$$ and $$+3$$
  • None
In which of the following pair oxidation number of $$Fe$$ is same:
  • $${ K }_{ 3 }{ Fe(CN) }_{ 6 },{ Fe }_{ 2 }{ O }_{ 3 }$$
  • $${ Fe(CN) }_{ 5 },{ Fe }_{ 2 }{ O }_{ 3 }$$
  • $${ Fe }_{ 2 }{ O }_{ 3, }FeO$$
  • $${ Fe }_{ 2 }({ SO }_{ 4 })_{ 3 },{ K }_{ 4 }Fe({ C) }_{ 6 }$$
Oxidation number of carbon in sucrose is:
  • $$0$$
  • $$+12$$
  • $$-12$$
  • $$+7$$
Oxidation number of P in $${ KH }_{ 2 }{ PO }_{ 3 }$$ is:
  • $$-1$$
  • $$-3$$
  • $$+5$$
  • $$+3$$
Oxidation number of Cr atom in $$CrO_5$$ and $$K_3CrO_8$$ respectively:
  • +6 , +6
  • +5 , + 6
  • +6 , + 5
  • + 5 , + 5
Oxidation number of $$Cr$$ in the following complex is:
1105897_56e9a940ffbc4eceb8a6bc0b080b451c.png
  • 3
  • 6
  • 4
  • 5
In substance $$Mg({ HXO }_{ 3 })$$, the oxidation number of X is :-
  • $$0$$
  • $$+2$$
  • $$+3$$
  • $$+4$$
Which of the following, oxidation number of carbon is -1?
  • $${ CH }_{ 4 }$$
  • $${ C }_{ 6 }{ H }_{ 6 }$$
  • $${ C }Cl_{ 4 }$$
  • $$HCHCl$$
In which reaction, there is change in oxidation number of N atom ?
  • $$2NO_2 \rightleftharpoons N_2O_4$$
  • $$2NO_2 + H_2O \rightarrow HNO_3 + HNO_2$$
  • $$NH_4OH \rightarrow NH^+_4 + OH^-$$
  • $$N_2O_5 + H_2O \rightarrow 2HNO_3$$
Reaction $$(A) S^{-2} + 4 H_2O_2 \rightarrow  SO^{2-}_4 + 4H_2O$$
$$(B)Cl_2 + H_2O_2 \rightarrow 2HCl + O_2$$
The true statement regarding the above reactions is :
  • $$H_2O_2$$ act as reductant in both the reactions.
  • $$H_2O_2$$ acts as oxidant in reaction (A) and reductant in reaction (B).
  • $$H_2O_2$$ acts as an oxidant in reaction in both the reactions.
  • $$H_2O_2$$ acts as reductant in reaction (A) and oxidant in reaction (B).
The brown ring complex compound is formulated as $$[Fe(H_2O)_5NO]SO_4$$. The oxidation state of iron is:
  • + 1
  • + 2
  • + 3
  • + 6
Oxidation number of oxygen atom in  $$O_3$$ molecules is:
  • $$0$$
  • $$-2$$
  • $$+ 2$$
  • $$+1$$
Which of the following is not a redox change ?
  • $$2H_2S + SO_2 \rightarrow 2H_2O + 3S$$
  • $$2BaO + O_2 \rightarrow 2BaO_2$$
  • $$BaO_2 + H_2SO_4 \rightarrow BaSO_4 + H_2O_2$$
  • $$2KClO_3 \rightarrow 2KCl + 3O_2$$
Which of the following is not a redox reaction ?
  • $$H_2 + Cl_2 \rightarrow 2HCl$$
  • $$NaOH + HCl \rightarrow NaCl + H_2O$$
  • Photosynthesis
  • Cell respiration
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