CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 9 - MCQExams.com

In which of the following compounds iron has lowest oxidation state :-
  • $$FeSO_4(NH_4)_2SO_4.6H_2O$$
  • $$K_4[Fe(CN)_6]$$
  • $$[Fe(CO)_5]$$
  • $$Fe_{0.94}O$$
Heated saw dust catches fire when a drop of concentrated nitric acid is added to it. This is due to
  •  dehydration
  • oxidation
  • reduction
  • dehydrogenation
Which of the following show non-zero multiple oxidation state?
  • $$S$$
  • $$O$$
  • $$Zn$$
  • $$H$$
Four $$Cl_{2}$$ molecules undergo a loss and gain of $$6$$ mole of electrons to form two oxidation states of $$Cl$$ in auto redox change. What are the $$+ve$$ and $$-ve$$ oxidation states of $$Cl$$ in the change:
  • $$Cl^{5+},Cl^{o}$$
  • $$Cl^{7+},Cl^{-}$$
  • $$Cl^{3+},Cl^{o}$$
  • $$Cl^{3+},Cl^{-}$$
In which of the following compounds, the oxidation state of $$I-$$atom is highest?
  • $${KI}_{3}$$
  • $$KI{O}_{4}$$
  • $$KI{O}_{3}$$
  • $$All\ of\ the \ above$$
Sulphur has highest oxidation state in:
  • $${ H }_{ 2 }S$$
  • $${ { H }_{ 2 }SO }_{ 4 }$$
  • $$Na_{ 2 }{ S }_{ 2 }{ O }_{ 3 }$$
  • $$Na_{2}S_{4}O_{6}$$
Oxidation state of oxygen in $$Cr{ O }_{ 5 }$$ is :
  • -1
  • -2
  • Both $$A$$ and $$B$$
  • $$-\frac { 1 }{ 2 } $$
What is the oxidation number of chromium in the dimeric hydroxo bridged species :-
1079025_3678a116bab4414fa930254fbf5dea73.PNG
  • $$+6$$
  • $$+4$$
  • $$+3$$
  • $$+2$$
The sum of the oxidation numbers of all the carbons in $$C_6H_5CHO$$ is :
  • 0
  • +2
  • +4
  • -4
A solution contains $${Fe}^{+2},{Fe}^{+3}$$ and $${I}^{-}$$ ions. This solution was treated with iodine at $${35}^{o}C$$. Then the favourable redox reaction is: 
(Given that $${ E }_{ { Fe }^{ +3 }/{ Fe }^{ +2 } }^{ o }=+0.77V;\quad { E }_{ { I }_{ 2 }/{ I }^{ - } }^{ o }=0.536V$$)
  • $${I}_{2}$$ will be reduced to $${I}^{-}$$
  • there will be no redox reaction
  • $${I}^{-}$$ will be oxidised to $${I}_{2}$$
  • $${Fe}^{+}$$ will be oxidised to $${Fe}^{+3}$$
Average oxidation number of iodine in $$KI_3$$?
  • $$+1/3$$
  • $$-1/3$$
  • $$+3$$
  • $$-1$$
The oxidation number of nitrogen in $$NCI_3$$ is ?
  • $$+3$$
  • $$-3$$
  • $$Zero$$
  • -$$1/3$$
$${ KMnO }_{ 4 }$$ can be prepared from $${ K }_{ 2 }MnO_{ 4 }$$ as per the reaction,

$${ 3MnO }_{ 2 }^{ 2- }+{ 2H }_{ 2 }O\rightleftharpoons { 2MnO }_{ 4 }^{ - }+{ MnO }_{ 2 }{ +4OH }^{ - }$$

The reaction can go to completion by removing $${ OH }^{ - }$$ ions by adding:
  • $$KOH$$
  • $${ CO }_{ 2 }$$
  • $$SO$$
  • $$HCl$$
Of the following elements, which one has the same oxidation state in all of its compounds?
  • Hydrogen
  • Fluorine
  • Carbon
  • Oxygen
Oxidation number of sodium in sodium amalgam is:
  • +2
  • +1
  • -3
  • 0
The oxidation state of Cr is $$[Cr(NH_3)_4Cl_2]$$ is?
  • $$+3$$
  • $$+2$$
  • $$+1$$
  • $$0$$
Which of the following shows highest oxidation number in combined state?
  • $$O$$
  • $$Ru$$
  • Both $$(A)$$ and $$(B)$$
  • None of the above
What is the oxidation state of $$Co$$ in $$[Co(H_2O)_5Cl]^{2+}$$?
  • $$+2$$
  • $$+3$$
  • $$+1$$
  • $$+4$$
$${ I }_{ 2 }+KI\rightarrow { KI }_{ 3 }\quad $$
In the above reaction:
  • only oxidation takes place
  • only reduction takes place
  • both of the above
  • none of these
Oxidation state of oxygen in hydrogen peroxide is?
  • -1
  • +1
  • 0
  • -2
Oxidation number of sulphur in $$Na_2S_2O_3$$ would be :
  • +4 
  • +2
  • -2
  • 0
Which of the following is not correctly matched?
  • $$CrO_5$$ ; oxidation number of $$Cr =$$ $$+10$$
  • $$Fe_3O_4$$; oxidation state of $$Fe = -\dfrac{8}{3}$$
  • $$Na - Hg$$; oxidation number of $$Na$$ is = $$+1$$
  • None of the above
Oxidation number of gold metal is 
  • +1
  • -1
  • 0
  • All of these
$$4Zn+10H{NO}_{3}\rightarrow 4Zn{({NO}_{3})}_{2}+{NH}_{4}{NO}_{3}+3{H}_{2}O$$
In this reaction one mole of $$H{NO}_{3}$$ is reduced by
  • $$26g$$ $$Zn$$
  • $$64g$$ $$Zn$$
  • $$128g$$ $$Zn$$
  • $$256g$$ $$Zn$$
For the half reaction
$$B(s) \rightarrow B^{2+} + 2e^{-}$$         $$E_{1}^{\circ} = - 0.44 V$$
and  $$B_{2}+\rightarrow B^{3+} + e^{-}$$    $$E_{2}^{\circ} = 1.3 V$$
What is $$E^{\circ}$$ for the reaction,
$$3e^{-} + B^{+3} \rightarrow B(s)$$
  • $$0.86$$ V
  • $$0.14$$ V
  • $$-0.14$$ V
  • $$-0.28$$ V
The oxidation number of S is $$(CH_{3})_{2}SO$$ is ?
  • 1
  • 2
  • 0
  • 3
The oxidation number of S in $$(CH_{3})_{2}SO$$ is ?
  • 1
  • 2
  • 0
  • 3
Highest positive oxidation state shown by:
  • Cl
  • Os
  • Mn
  • Cr
The elements having lowest and highest oxidation number respectively are:
  • $$Sc,Fe$$
  • $$Sc,Mn$$
  • $$Ag,Mn$$
  • $$Fe,Mn$$
A gas X at 1 atm is bubbled through the solution containing a mixture of 1MY and 1MZ  at 25 degrees. If the order of reduction potential is Z > Y > X, then 
  • Y will oxidise X not Z
  • Y will oxidise Z not X
  • Y will oxidise both X and Y
  • Y will reduce both X and Y
The complex compound in which metal is not present in zero oxidation state?
  • $${ Mn }_{ 2 }{ \left( CO \right) }_{ 10 }$$
  • $$\left[ Ni{ \left( CO \right) }_{ 4 } \right]$$
  • $$\left[ Cr{ \left( { C }_{ 6 }{ H }_{ 6 } \right) }_{ 2 } \right]$$
  • $$K\left[ { PtCl }_{ 3 }\left( { C }_{ 2 }{ H }_{ 4 } \right) \right]$$
How many oxygen atoms in blue per chomate $${ CrO }_{ 5 }$$  are having $$-1$$ oxidation state?
  • 1
  • 2
  • 4
  • 5
In which of the following compounds, the metal is in the lower oxidation state
  • $$ [Co( NH_{3})_{5}Br_{2}]SO_{4}$$
  • $$Fe_{3} [Fe( CN)_{6}]_{2}$$
  • $$[Mn_{2}(CO)_{10}]$$
  • $$K[ PtCI_{3}(C_{2} H_{4})]$$
Oxidation numbers of chlorine atoms in CaOCl$$_2$$ are
  • 0,0
  • -1,-1
  • -1+1
  • None of these
Oxidation numbers of P in $$P{ O }_{ 4 }^{ 3- }$$, of S in $$S{ O }_{ 4 }^{ 2- }$$ and that of Cr in $$C{ r }_{ 2 }{ O }_{ 7 }^{ 2- }$$ are respectively:
  • +3,+6 and +5
  • +5,+3and +6
  • -3,+6 and +6
  • +5,+6 and +6
Fe shows an oxidation state of $$+1$$ in:
  • $$Fe(CO)_5$$
  • $$[Fe(H_2O)_5 NO]SO_4$$
  • $$Fe_4[Fe(CN)_6]$$
  • $$FeCl_4^-$$
Which is not a redox reaction?
  • $$BaO_{2}+H_{2}SO_{4}\rightarrow BaSO_{4}+H_{2}O_{2}$$
  • $$2BaO_+O{_2}\rightarrow 2BaO_{2}$$
  • $$4KClO_{3}\rightarrow 4KClO_{2}+2O_{2}$$
  • $$SO_{2}+2H_{2}S\rightarrow 2H_{2}O+3S$$
In which of the compounds does hydrogen have an oxidation state of - 1 ?
  • $$ CH_4 $$
  • $$ NH_3 $$
  • $$ HCI $$
  • $$ CaH_2 $$
The correct order of decreasing oxidation number of P in compounds is:
  • $${{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{3}}}{\kern 1pt} {\text{ < }}{\kern 1pt} {{\text{H}}_{\text{4}}}{{\text{P}}_{\text{2}}}{{\text{O}}_{\text{7}}}{\kern 1pt} {\text{ < }}{\kern 1pt} {{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{2}}}{\kern 1pt} {\text{ < }}{\kern 1pt} {{\text{P}}_{\text{4}}}$$
  • $${{\text{H}}_{\text{4}}}{{\text{P}}_{\text{2}}}{{\text{O}}_{\text{7}}}{\kern 1pt} {\text{>}}{\kern 1pt} {{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_3}{\kern 1pt} > {\kern 1pt} {{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_2}{\kern 1pt} {\text{ > }}{\kern 1pt} {{\text{P}}_{\text{4}}}$$
  • $${{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_3}{\kern 1pt} < {\kern 1pt} {{\text{H}}_{\text{4}}}{{\text{P}}_{\text{2}}}{{\text{O}}_{\text{7}}}{\kern 1pt} {\text{ < }}{\kern 1pt} {{\text{P}}_{\text{4}}}{\kern 1pt} {\kern 1pt} {\text{ < }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_2}$$
  • $${{\text{H}}_{\text{4}}}{{\text{P}}_{\text{2}}}{{\text{O}}_{\text{7}}}{\kern 1pt} {\text{ < }}{\kern 1pt} {{\text{P}}_{\text{4}}}{\kern 1pt} {\kern 1pt} {\text{ < }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_2}{\kern 1pt} {\text{ < }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_3}{\kern 1pt} $$
Ratio of number of oxygen atoms which show -1 and -2 oxidation states in the compound $${ H }_{ 2 }{ S }_{ 2 }{ O }_{ 8 }$$ is
  • 1 : 3
  • 1 : 2
  • 3 : 1
  • None of these
Oxidation number of fluorine in $${F}_{2}O_2$$ is:
  • $$+1$$
  • $$+2$$
  • $$-1$$
  • $$-2$$
Which of the following equation depict the oxidising nature of $$H_{2}O_{2}$$?
  • $$2MnO^{-}_{4}+6H^{+}+5H_{2}O_{2}\rightarrow 2Mn^{2}+8H_{2}O+5O_{2}$$
  • $$2Fe^{3+}+2H^{+}+H_{2}O_{2}\rightarrow 2Fe^{2}+2H_{2}O+O_{2}$$
  • $$2I^{-}+2H^{+}+H_{2}O_{2}\rightarrow I_{2}+2H_{2}O$$
  • $$KIO_{4}+H_{2}O_{2}\rightarrow KIO_{3}+H_{2}O+O_{2}$$
The oxidation number of Cr is +6 in:
  • $$K_{2}CrO_{4}$$
  • $$K_{2}Cr_{2}O_{7}$$
  • $$KCrO_{3}CI$$
  • All of these
The oxidation state of Fe in $$ \left[ Fe\left( { H }_{ 2 }{ O } \right) _{ 5 }NO \right] { SO }_{ 4 }$$ is :
  • $$+1$$
  • $$+2$$
  • $$+3$$
  • $$+4$$
Given that $$ { Cl }_{ 2\left( g \right)  }+{ 2e }^{ - }\longrightarrow { 2Cl }^{ - }\left( aq \right)$$ is the reduction half-reaction for the overall reaction $$ 2Ag\left( s \right) +{ Cl }_{ 2 }\left( g \right) \longrightarrow 2AgCl\left( s \right)$$. 
What is the oxidation half reaction?
  • $$ Ag\left( s \right) \longrightarrow Ag^{ + }\left( aq \right) +e^{ - }$$
  • $$ Ag\left( s \right) +{ Cl }^{ - }\left( aq \right) \longrightarrow Ag\left( s \right) +e^{ - }$$
  • $$ Ag\left( s \right) +{ Cl }_{ 2 }\left( g \right) +e^{ - }\longrightarrow AgCl\left( s \right) +Cl^{ - }\left( aq \right)$$
  • $$ { 2Cl }^{ - }\left( aq \right) \longrightarrow { Cl }_{ 2 }\left( g \right) +2e^{ - }$$
The oxidation state(s) of $$Cl$$ in $$CaO_{2}Cl_{2}$$ (bleaching powder) is/are:
  • +1 only
  • -1 only
  • +1 and -1
  • none of these
The oxidation state of $$Xe$$ in $$XeO_{3}$$ and bond angle in it are:
  • $$+6,\ 109^{o}$$
  • $$+8,\ 103^{o}$$
  • $$+6,\ 103^{o}$$
  • $$+8,\ 120^{o}$$
When $$SO_2$$ is passed in acidified potassium dichromate solution, the oxidation number of $$S$$ is changed from:
  • $$+4$$ to zero
  • $$+4$$ to $$+2$$
  • $$+4$$ to $$+6$$
  • $$+6$$ to $$+4$$
Oxidation number of N in HNO$$_3$$ is :
  • $$-3.5$$
  • $$+3.5$$
  • $$-6$$
  • none of these
Which one of the following is a redox reaction ?
  • $$H_{2}+Br_{2} \rightarrow 2HBr$$
  • $$2NaCl+H_{2}SO_{4} \rightarrow Na_{2}SO_{4}+2HCl$$
  • $$HCl+AgNO_{3} \rightarrow AgCl+HNO_{3}$$
  • $$NaOH+HCl \rightarrow NaCl+H_{2}O$$
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