CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 10 - MCQExams.com

Oxidation number of carbon in chloroform $$(CHCl_3)$$ is :
  • $$+2$$
  • $$\frac{+4}{3}$$
  • $$+3$$
  • $$+4$$
In the following redox equation,
$$xUO^{+2}+Cr_2O_7^{2-}\rightarrow aUO_2 ^{2+}+zCR^{+3}+bH_2O$$
The values of coefficients x, y and z respectively are:
  • 3,8,2
  • 3,8,7
  • 3,2,4
  • None of the above
Oxidation number of osmium (Os) in $$OsO_4$$ is 
  • +8
  • +6
  • +7
  • +4
In which of the following reactions, there is no change valency ?
  • $${ 4KClO }_{ 3 }\rightarrow { 3KClO }_{ 4 }+KCl$$
  • $${ SO }_{ 2 }+{ 2H }_{ 2 }S\rightarrow { 2H }_{ 2 }O+3S$$
  • $${ BaO }_{ 2 }+{ H }_{ 2 }{ SO }_{ 4 }\rightarrow { BaSO }_{ 4 }+H_{2}O_{2}$$
  • $$2BaO +{ O }_{ 2 }\rightarrow { 2BaO }_{ 2 }$$
In the reaction, $$Fe_2O_3 + 3C \rightarrow 2Fe + 3CO$$, oxidation number of $$C$$:
  • increases by 3 per atom
  • decreases by 3 per atom
  • increases by 2 per atom
  • no change
To a 25 ml $$ H_2O_2 $$ solution excess acidified solution of $$KI$$ was added. The iodine liberated required 20 ml of 0.3 N sodium thiosulphate solution. Use these data to choose the correct statement from the following
  • The weight of $$ H_2O_2 $$ present in 25 ml solution is 0.102 g.
  • The molarity of $$ H_2O_2 $$ solution is 0.12 M.
  • The weight of $$ H_2O_2 $$ present in 1 L of the solution is 0.816 g.
  • The volume strength of $$ H_2O_2 $$ is 1.344 L.
Oxidation number of $$Cl$$ in $$CaOC{l_2}$$ (bleaching powder is)
  • Zero , since it contains $$C{l_2}$$
  • -1 , since it contains $$C{l^ - }$$
  • +1 , since it contains $$Cl{O^ - }$$
  • +1 and -1 since it contains $$Cl{O^ - }$$ and $$C{l^ - }$$
In the reaction $$MnO_{4}^{-}+SO_{3}^{-2}+H^{+}\longrightarrow SO_{4}^{2+}+Mn^{2+}+H_{2}O$$
  • $$MnO_{4}^{-}$$ and $$H^{+}$$ both are reduced.
  • $$MnO_{4}^{-}$$ is reduced and $$H^{+}$$ is oxidised.
  • $$MnO_{4}^{-}$$ is reduced and $$SO_{3}^{2-}$$ is oxidised.
  • $$MnO_{4}^{-}$$ is oxidised and $$SO_{3}^{2-}$$ is reduced.
In the fluorite structure, the oxidation number of $$Ca$$ is:
  • +2
  • +6
  • +8
  • +3
The oxidation number of oxygen in $$O_2F_2$$ is:
  • +2
  • -2
  • +1
  • -1
If the following half cells have the $$E^o$$ values as
$$Fe^{+3} + e^- \rightarrow Fe^{+2}$$; $$E^o= +0.77V$$ and $${Fe}^{+2}+2 {e}^{-} \longrightarrow {Fe}$$ ; $$E^o= -0.44 V$$ The $$E^o$$ of the half cell is $$Fe^{+3} + 3e^- \rightarrow Fe$$ will be:
  • $$0.33$$ V
  • $$1.21$$ V
  • $$0.04$$ V
  • $$0.605$$ V
Which compound contains two different elements with identical oxidation states?
  • HClO
  • $$Mg(OH)_2$$
  • $$Na_2SO_4$$
  • $$NH_4Cl$$
In the reaction, $$MnO^{-}_{4(aq)}+Br^{-}_{(aq)}\rightarrow MnO_{2(s)}+BrO^{-}_{3(aq)}$$, the correct change in oxidation number of the species involved is:
  • $$Br^{5+}$$ to $$Br^{-}$$
  • $$Mn^{7+}$$ to $$Mn^{2+}$$
  • $$Mn^{7+}$$ to $$Mn^{3+}$$
  • $$Br^{-}$$ to $$Br^{5+}$$
Balance the following redox equations in basic medium by oxidation number method :
  • $$\mathrm { Zn } _ { ( \mathrm { s } ) } + \mathrm { NO } _ { 3 ( \mathrm { aq } ) } ^ { - } \longrightarrow \mathrm { NH } _ { 3 ( \mathrm { aq } ) } + \mathrm { Zn } ( \mathrm { OH } ) _ { 6 ( \mathrm { aq } ) } ^ { 2 - }$$
  • $$\mathrm { MnCl } _ { 2 ( \mathrm { aq } ) } + \mathrm { HO } _ { 2 ( \mathrm { aq } ) } ^ { - } \longrightarrow \mathrm { Mn } ( \mathrm { OH } ) _ { 3 ( \mathrm { s } ) } + \mathrm { Cl } _ { ( \mathrm { aq } ) } ^ { - }$$
  • $$\mathrm { Mn } _ { ( \mathrm { aq } ) } ^ { 2 + } + \mathrm { H } _ { 2 } \mathrm { O } _ { 2 ( \mathrm { aq } ) } \longrightarrow \mathrm { MnO } _ { 2 ( \mathrm { s } ) } + \mathrm { H } _ { 2 } \mathrm { O } _ { ( l ) }$$
  • $$\mathrm { Cu } ( \mathrm { OH } ) _ { 2 ( \mathrm { s } ) } + \mathrm { N } _ { 2 } \mathrm { H } _ { 4 } ( \mathrm { aq } ) \longrightarrow \mathrm { Cu } _ { ( \mathrm { s } ) } + \mathrm { N } _ { 2 ( \mathrm { g } ) }$$
In the compounds $$KMnO_4$$ and $$K_2Cr_2O_7$$, the lowest oxidation state is of:
  • potassium
  • chromium
  • oxygen
  • manganese
The compound of Xe and F is found to have 53.5% Xe. What is oxidation number of Xe in this compound? (Xe = 131)
  • -4
  • 0
  • +4
  • +6
Which reaction is not a redox reaction?
  • $$Mg+2HNO_3\rightarrow Mg(NO_3)_2+H_2$$
  • $$2Mg(NO_3)_2\rightarrow 2MgO+4NO_2+O_2$$
  • $$SO_2+NO_2\rightarrow SO_3+NO$$
  • $$SO_3+H_2O\rightarrow H_2SO_4$$
Oxidation number of sodium in sodium amalgam is :
  • +2
  • +1
  • -2
  • zero
The order of the oxidation state of the phosphorus atom in $$ H_{3}PO_{2} $$, $$ H_{3}PO_{4} $$, $$ H_{3}PO_{3} $$ and $$ H_{4}P_{2}O_{6} $$
  • $$ H_{3}PO_{4} > H_{3}PO_{2}> H_{3}PO_{3}>H_{4}P_{2}O_{6} $$
  • $$ H_{3}PO_{4} >H_{4}P_{2}O_{6}> H_{3}PO_{3}> H_{3}PO_{2} $$
  • $$ H_{3}PO_{2}> H_{3}PO_{3}> H_{2}P_{2}O_{6}> H_{3}PO_{4} $$
  • $$ H_{3}PO_{3}>H_{3}PO_{2} > H_{3}PO_{4}> H_{2}P_{2}O_{6} $$
The oxidation states of Cr in  $$  \left [Cr(H_{2}O_{6})  \right ] Cl_{3} $$, $$ \left [ Cr(C_{6}H_{6})_{2} \right ] $$ and $$ K_{2}\left [ Cr(CN)_{2}(O_{2})(O_{2})(NH_{3}) \right ] $$ respectively are
  • +3,0 and +4
  • +3,+4 and +6
  • +3,+2 and +4
  • +3,+0 and +6
Which of the following reaction is an example of redox reactions
  • $$ XeF_{4}+O_{2}F_{2}\rightarrow XF_{6} +O_{2} $$
  • $$ XeF_{2}+PF_{5}\rightarrow \left [ XeF \right ]^{+}PF_{6}^{-} $$
  • $$ XeF_{6}+H_{2}O\rightarrow XeoF_{4}+2HF $$
  • $$ XeF_{6}+2H_{2}O\rightarrow Xeo_{2}F_{2}+4HF $$
The oxidation numbers of $$S$$ in $$S_{8},\ S_{2}F_{2}$$ and $$H_{2}S$$ respectively are
  • $$0,\ +1$$ & $$-2$$
  • $$+2,\ +1$$ & $$-2$$
  • $$0,\ +1$$ & $$+2$$
  • $$-2,\ +1$$ & $$-2$$
Oxidation number of $$N$$ in $${({NH}_{4})}_{2}{SO}_{4}$$ is
  • $$-1/3$$
  • $$-1$$
  • $$+1$$
  • $$-3$$
If $$H{NO}_{3}$$ changes into $${N}_{2}O$$, the oxidation number is changed by
  • $$+2$$
  • $$-1$$
  • $$0$$
  • $$+4$$
The oxidation number of $$C$$ in $${CO}_{2}$$ is
  • $$-2$$
  • $$+2$$
  • $$-4$$
  • $$+4$$
Oxidation number of osmiium $$(Os)$$ in $$Os{O}_{4}$$ is
  • $$+4$$
  • $$+6$$
  • $$+7$$
  • $$+8$$
The oxidation states of the most electronegative element in the products of the reaction of $$Ba{O}_{2}$$ with dilute $${H}_{2}{SO}_{4}$$ are
  • $$0$$ and $$-1$$
  • $$-1$$ and $$-2$$
  • $$-2$$ and $$0$$
  • $$-2$$ and $$+1$$
The oxidation number of $$Fe$$ and $$S$$ in iron pyrites are
  • $$4$$, $$-2$$
  • $$2$$, $$-1$$
  • $$3$$, $$-1.5$$
  • $$3$$, $$-1$$
The oxidation number of $$Ba$$ in barium peroxide is
  • $$+6$$
  • $$+2$$
  • $$1$$
  • $$+4$$
$${Sn}^{2+}$$ loses two electrons in a reaction. What will be the oxidation number of tin after the reaction?
  • $$+2$$
  • zero
  • $$+4$$
  • $$-2$$
The sum of the oxidation numbers of all the carbons in $${C}_{6}{H}_{5}CHO$$ is
  • $$+2$$
  • $$0$$
  • $$+4$$
  • $$-4$$
In which of the following compounds the oxidation number of carbon is maximum?
  • $$HCHO$$
  • $$CH{Cl}_{3}$$
  • $${CH}_{3}OH$$
  • $${C}_{12}{H}_{22}{O}_{11}$$
In which of the following pair of compounds, oxidation number of chromium is same?
  • $$K_2CrO_4$$ and $$KCrO_2$$
  • $$KCrO_2$$ and $$Cr(CO)_6$$
  • $$K_2Cr_2O_7$$ and $$Cr(CO)_4$$
  • $$K_2Cr_2O_7$$ and $$K_2CrO_4$$
Balance the following equation and choose the quantity which is the sum of the coefficients of reactants and products:
             ......... $$ PtCl_4 $$ + ........... $$ XeF_4 \rightarrow PtF_{6} $$ +  ....$$ClF $$ + ....$$Xe $$ 
  • $$16$$
  • $$13$$
  • $$18$$
  • $$12$$
The value of coefficients to balance the following reaction are
$$Cr(OH)_3+ClO^-+OH^- \rightarrow CrO_4^{2-}+Cl^-+H_2O$$
  • $$Cr(OH)_3\ 2,\ ClO^-\ 3,\ CrO_4^{2-}\ 3,\ Cl^-\ 3$$
  • $$Cr(OH)_3\ 2,\ ClO^-\ 4,\ CrO_4^{2-}\ 3,\ Cl^-\ 2$$
  • $$Cr(OH)_3\ 2,\ ClO^-\ 4,\ CrO_4^{2-}\ 4,\ Cl^-\ 2$$
  • $$Cr(OH)_3\ 2,\ ClO^-\ 3,\ CrO_4^{2-}\ 2,\ Cl^-\ 3$$
The oxidation number of $$ \mathrm{N} $$ in $$ \mathrm{NF}_{3} $$ is $$ +3 . $$
  • True
  • False
The oxidation number of sulphur in $$ \mathrm{S}_{8}, \mathrm{S}_{2} \mathrm{F}_{2}, \mathrm{H}_{2} \mathrm{S} $$ respectively, are
  • $$ 0,+1 $$ and -2
  • $$ +2,+1 $$ and -2
  • $$ 0,+1 $$ and +2
  • $$ -2,+1 $$ and -2
Which of the following statements is correct?
  • Hydrogen has the same ionization potential as alkali metals
  • $$H^-$$ has more electronegativity as halogens
  • $$H^-$$ has oxidation number of $$-1$$
  • $$H^-$$ will Dot be liberated at the anode.
Oxidation state of Osmium (Os) in $$ \mathrm{OsO}_{4} $$ is
  • $$ +7 $$
  • $$ +6 $$
  • $$ +4 $$
  • $$ +8 $$
The reaction, $$ 3 \mathrm{ClO}^{-}(a q) \rightarrow $$ $$ \mathrm{ClO}_{3}^{-}(a q)+2 \mathrm{Cl}^{-}(a q) $$ is an example of
  • Oxidation reaction
  • Reduction reaction
  • Disproportionation reaction
  • Decomposition reaction.
A metal ion $$ M^{3+} $$ loses 3 electrons, its oxidation number will be
  • $$ +3 $$
  • $$ +6 $$
  • $$ 0 $$
  • $$ -3 $$
The oxidation number of carbon in $$ \mathrm{CH}_{2} \mathrm{Cl}_{2} $$ is
  • 0
  • 2
  • 3
  • 5
Oxidation states of the metal in the minerals haematite and magnetite, respectively are:
  • II, III in haematite and III in magnetite
  • II, III in haematite and II in magnetite
  • II in haematite and II, III in magnetite
  • III in haematite and II, III in magnetite
The number of moles of $$KMnO_{4}$$ that will be needed to react completely with one mole of ferrour oxalate $$Fe(C_{2}O_{4})$$ in acidic solution is :
  • $$1$$
  • $$\dfrac{2}{5}$$
  • $$\dfrac{3}{5}$$
  • $$\dfrac{4}{5}$$
What is the oxidation state of Fe in the product formed when acidified potassium ferrocyanide $$(K_{4}[Fe(CN)_{6}])$$ is treated with hydrogen peroxide?
  • $$+2$$
  • $$+3$$
  • $$+1$$
  • $$+6$$
One gas bleaches the colour of flowers by reduction while the other gas by oxidation. The two gases are, respectively:
  • $$CO$$ & $$Cl_{2}$$
  • $$H_{2}S$$ & $$Br_{2}$$
  • $$SO_{2}$$ & $$Cl_{2}$$
  • $$NH_{3}$$ & $$SO_{3}$$
When $$K_{2}Cr_{2}O_{7}$$ is mixed with $$H_{2}SO_{4}$$ and thoroughly shaken with $$H_{2}O_{2}$$ in presence of ether, then a floated blue coloured complex $$X$$ is formed. The change in oxidation state and the percentage of $$Cr$$ in the complex $$X$$ is:
  • $$+6, 49.4$$
  • $$+4, 39.4$$
  • $$0, 39.4$$
  • $$+4, 59.4$$
The oxidation number of $$Cr$$ in $$CrO_{5}$$ is:
  • $$+10$$
  • $$+8$$
  • $$+6$$
  • $$+4$$
Which ordering of compounds is according to the decreasing order of the oxidation state of nitrogen?
  • $$HNO_3, NH_4Cl, NO, N_2$$
  • $$HNO_3, NO, NH_4Cl, N_2 $$
  • $$HNO_3, NO, N_2, NH_4Cl$$
  • $$NO, HNO_3, NH_4Cl, N_2$$
$$1$$ mol of ferric oxalate is oxidised completely by $$x$$ mol of $$MnO_{4}^{-}$$ in acidic medium. Then, $$x$$ is :
  • $$1.2$$
  • $$1.6$$
  • $$1.8$$
  • $$1.5$$
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