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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 - H3PO2
  • Chlorine in +7 oxidation state - HClO
  • Chromium in +6 oxidation state -CrO2Cl2
  • Carbon in 0 oxidation state - C12H22O11
Which of the following oxidation numbers is not correctly matched?
  • P in NaH2PO4=+5
  • Ni  in [Ni(CN)6]4=+2
  • P in Mg2P2O7=+6
  • Cr in (NH4)2Cr2O7=+6
Oxidation number of sulphur in peroxomonosulphuric acid (H2SO5) is:
  • +4
  • +2
  • +6
  • -2
In which of the following compounds oxidation state of chlorine has two different values?
  • CaCl2
  • NaCl
  • CaOCl2
  • CCl4
Match the column I with column II and mark the appropriate choice.
Column I
( Compound )
Coloumn II
(Oxidation state of Fe)
( A )K3[(Fe(OH)6](i)+8/3
( B )K2[FeO4](ii)+2
( C )FeSO4,(NH4)2SO46H2O(iii)+3
( D)Fe3O4(iv)+6
  • (A)(iii),(B)(i),(C)(ii),(D)(iv)
  • (A)(iii),(B)(iv),(C)(ii),(D)(i)
  • (A)(i),(B)(iii),(C)(ii),(D)(iv)
  • (A)(iv),(B)(ii),(C)(i),(D)(iii)
Mark the correct statement from the following.
  • Copper metal can be oxidised by Zn2+ ions
  • Oxidation number of phosphorus in P4 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 OsO4
The oxidation state of Fe in K4[Fe(CN)6] is:
  • +2
  • +3
  • +4
  • +6
In which of the following compounds carbon is in highest oxidation state?
  • CH3Cl
  • CCl4
  • CHCl3
  • CH2Cl2
What is the oxidation state of P in Ba(H2PO2)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}=1.10V. E^{\ominus}_{Cell} for the galvanic cell will be?
  • 2.14V
  • 1.80V
  • 1.07V
  • 0.82V
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^oC, Sr_{(s)}+Mg^{2+}_{(aq)}\rightarrow Sr^{2+}_{(aq)}+Mg_{(s)}, that occurs in a galvanic cell. E^o_{{Mg^{2+}}/{Mg}}=-2.37V and E^o_{{Sr}^2+/Sr}=-2.89V.
  • 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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