CBSE Questions for Class 11 Medical Chemistry Redox Reactions Quiz 13 - MCQExams.com

The oxidation number of carbon in $$CH_2F_2$$ is:
  • $$0$$
  • $$1$$
  • $$4$$
  • $$6$$
The sum of oxidation states of all atoms in $$ClO_4^-$$ is:
  • 0
  • -4
  • -1
  • +2
In which following compounds, phosphorous exhibits its highest oxidation state?
  • $$H_3PO_2$$
  • $$H_4P_2O_7$$
  • $$H_4P_2O_6$$
  • $$H_4P_2O_5$$
Oxidation number of chlorine atoms in $$CaOCl_2$$ are
  • $$0,0$$
  • $$-1, -1$$
  • $$-1, +1$$
  • $$-2,+7$$
Find the potential of a half-cell having reaction, $$Ag_{2}S+2e\rightarrow2Ag+S^{2-}$$ in a solution buffered
$$pH=3$$ and which is also saturated with $$0.1\ M\ H_{2}S$$. For $$H_{2}S:\ K_{1}=10^{-8}$$ and $$K_{2}=2\times 10^{-13},\ K_{sp}(Ag_{2}S)=2\times 10^{-48},\ E_{Ag,ag}^{o}=0.8$$
  • $$0.432\ V$$
  • $$1.658\ V$$
  • $$-0.245\ V$$
  • $$-0.144\ V$$
The number of mole of ferrous oxalate oxidized by one mole of $$ KMnO_{4}$$ in acidic medium is:​
  • 1.66
  • 5
  • 0.6
  • 2
The oxidation state of iron in chalco pyrite $$ (CuFeS_2) $$ is 
  • +1
  • +3
  • +2
  • +4
How many moles of $$KMnO_{4}$$ are required to oxidise one mole of $$SnCl_{2}$$ in acidic medium ?
  • $$\dfrac{1}{5}$$
  • $$\dfrac{2}{5}$$
  • $$\dfrac{3}{5}$$
  • $$\dfrac{4}{5}$$
In $$Zn|Zn^{+2}|| Ag^+|Ag$$, how will cell potential be affected if KI is added to $$Ag^{+}$$ half cell?
  • $$E_{cell}$$ will increase
  • $$E_{cell}$$ will decrease
  • $$E_{cell}$$ will remain unaffected
  • $$E_{cell}$$ is first increase then decrease
Which is a redox reaction ?
  • $${ 2CuI }_{ 2 }\rightarrow CuI+{ I }_{ 2 }$$
  • $$NaCl+AgNO_{ 3 }\rightarrow AgCl+NaNO_{ 3 }$$
  • $${ NH }_{ 4 }Cl+NaOH\rightarrow { NH }_{ 3 }+NaCl+H_{ 2 }O$$
  • $${ Cr }_{ 2 }{ \left( { SO }_{ 4 } \right) }_{ 3 }+6KOH\rightarrow 2Cr{ \left( OH \right) }_{ 3 }+{ 3K }_{ 2 }{ SO }_{ 4 }$$
When ethane is burnt in excess of oxygen, the oxidation number of carbon changes by
  • $$+8$$
  • $$+7$$
  • $$+3$$
  • $$+4$$
What is the sum of oxidation number of all carbon in $$C_6H_5CHO$$ ?
  • -4
  • 5
  • 6
  • 7
Which of the following is correct about oxidation number?
  • The O.N. of all atoms in elementary states is 0
  • Alkali and alkaline earth metals have +1 and +2 oxidation states respectively
  • The O.N. of a monoatomic ion is the same as its charge
  • All of the above
Average oxidation state of $${\rm{Fe}}$$ in $${\rm{F}}{{\rm{e}}_{\rm{3}}}{{\rm{O}}_{\rm{4}}}$$ is 
  • $$\frac{2}{3}$$
  • $$\frac{4}{5}$$
  • $$\frac{5}{4}$$
  • $$\frac{8}{3}$$
$${\text{2Fe}}{\left( {{\text{CO}}} \right)_{\text{5}}}\xrightarrow{{{\text{Photolysis}}}}{\text{Fe}}{\left( {{\text{CO}}} \right)_{\text{9}}}{\text{ + CO}}$$ Oxidation of $${\text{Fe}}$$ in $${\text{F}}{{\text{e}}_{\text{2}}}{\left( {{\text{CO}}} \right)_{\text{9}}}$$
  • $$4.5$$
  • $$2$$
  • $$3$$
  • $$0$$
Find out the values of a,b,c and d in the following equation:

$${IO_{3}}^{-}+aI^{-}+bH^{+}$$$$\rightarrow$$ $$ cH_{2}O+dI_{2}$$
  • a=3, b=2, c=1, d=1
  • a=5, b=6, c=3, d=3
  • a=5, b=6, c=3, d=6
  • a=10, b=12, c=6, d=6
Following reaction describes the rusting of iron $$4{\text{Fe}} + 3{{\text{O}}_2} \to 4{\text{F}}{{\text{e}}^{3 + }} + {60^{2 - }}$$, which one of the following statement is incorrect?
  • This is an example of a redox reaction
  • Metallic iron is reduced to $${\text{F}}{{\text{e}}^{{\text{3 + }}}}$$
  • $${\text{F}}{{\text{e}}^{{\text{3 + }}}}$$ is an oxidizing agent
  • Metallic iron is a reducing agent
Of the following transition metals, the maximum number of oxidation states is shown by
  • $$Cr$$
  • $$Mn$$
  • $$Fe$$
  • $$Ti$$
Which of the following is a redox:
  • $$2NaAg{(CN)}_{2}+Zn\longrightarrow {Na}_{2}Zn{(CN)}_{4}+2Ag$$
  • $$Ba{O}_{2}+{H}_{2}{SO}_{4}\longrightarrow Ba{SO}_{4}+{H}_{2}O$$
  • $${N}_{2}{O}_{5}+{H}_{2}O\longrightarrow 2H{NO}_{3}$$
  • $$Ag{NO}_{3}+KI\longrightarrow AGI+K{NO}_{3}$$
Consider the half-cell reaction(s)
$${Cu}^{2+}+{e}^{-}\rightarrow {Cu}^{+};{E}^{o}=0.15V$$
$${Cu}^{2+}+2{e}^{-}\rightarrow {Cu};{E}^{o}=0.33V$$
$${E}^{o}$$ for the half-cell reaction: $${Cu}^{+}+{e}^{-}\rightarrow Cu$$ will be:
  • $$0.48V$$
  • $$0.18V$$
  • $$0.31V$$
  • $$0.51V$$
What is the oxidation state of iodine when it is oxidized in the form $${{\text{I}}^{\text{ - }}}$$ in neutral medium by permanganate ion
  • $$ + 5$$
  • $$ + 7$$
  • $$ + 3$$
  • $$ + 1$$
A compound contains atoms $$\mathrm { A } , \mathrm { B }$$ and $$\mathrm { C }$$ . The oxidation number of $$\mathrm { A }$$ is $$+ 2 ,$$ of $$\mathrm { B }$$ is $$+ 5$$ and of $$\mathrm { C }$$ is $$- 2 .$$ The possible formula of the compound is:
  • $$A B C _ { 2 }$$
  • $$\mathrm { A } _ { 2 } \left( \mathrm { BC } _ { 3 } \right) _ { 2 }$$
  • $$A_3(BC_4)_2$$
  • $$\mathrm { A } _ { 3 } \left( \mathrm { B } _ { 4 } \mathrm { C } \right) _ { 2 }$$
An element A in a compound ABD has oxidation number -n. It is oxidized by $${\text{C}}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{7}}}^{{\text{2 - }}}$$ in acid medium. In the experiment, $$1.68 \times {10^{ - 3}}$$ moles of $$\;{{\text{K}}_{\text{2}}}{\text{C}}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{7}}}$$ were used for $$1.68 \times {10^{ - 3}}$$ mole ABD. The new oxidation number of A after oxidation is :
  • 3
  • 3 - n
  • n - 3
  • + n
In the reaction $$Cu + {H_2}S{O_4} \to CuS{O_4} + {H_2}O + S{O_2}$$
  • $${{\text{H}}^{\text{ + }}}$$ is the oxidising agent
  • $${\text{S}}{{\text{O}}_{{\text{2  }}}}$$ is the oxidising agent
  • Both $$\left( {\text{A}} \right)$$ and $$\left( {\text{B}} \right)$$ are correct
  • None of the above is correct
What is the oxidation number of $$N$$ in $$NH_2OH$$? 
  • -2
  • -1
  • 0
  • +1
Which of the following arrangement represents increasing O.N. of 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 oxidation states of the most electronegative element in the product of the reaction of $$Ba{ O }_{ 2 }$$ with dilute $${ H }_{ 2 }{ SO }_{ 4 }$$ are:
  • +1 and +2
  • -1 and +2
  • -2 and -2
  • -2 and -1
The oxidation number of $$P$$ in $$Mg{ NH }_{ 4 }{ PO }_{ 4 }$$ is 
  • +3
  • +5
  • +2
  • +7
Match List I and List-II and select the correct answer using the codes given below the lists:
List-I (compound)List-II ( oxidation states of N ) 
(A)$$ NO_2 $$(1)+5
(B)$$ HNO_2 $$(2)-3
(C)$$ NH_3 $$(3)+4
(D)$$ N_2O_5 $$(4)+3
The oxidation number of ''V'' in the complex $${\text{R}}{{\text{b}}_{\text{4}}}{\text{Na}}\left[ {{\text{H}}{{\text{V}}_{{\text{10}}}}{{\text{O}}_{{\text{28}}}}} \right]$$ is 
  • +3
  • +5
  • +7
  • +6
Oxidation numbers of sulphur in $$H_2S_3$$ molecule are
  • -1, -1 and -1
  • -1, +1 and +1
  • -1, 0 and -1
  • +1, 0 and -1
Oxidation number of oxygen in $$NaO_{ 3 }, { KO }_{ 2 }$$ respectively are:
  • 3, 2
  • 1, 0
  • 0, 1
  • -0.33, -0.5
The oxidation number of nitrogen in $$NC{l_3}$$ is 
  • +3
  • -3
  • zero
  • -1/3
When $$ Cl_2 $$ gas reacts with hot and concentrated sodium hydroxide solution, the oxidation number of chlorine changes from____ 
  • zero to +1 and zero to -5
  • zero to -1 and zero to +5
  • zero to -1 and zero to +3
  • zero to +1 and zero to +3
Which of the following is a non - redox process ?
  • $$ SO_{4}^{2-}\rightarrow SO_{3} $$
  • $$ Cr_{2}O_{7}^{2-}\rightarrow CrO_{4}^{2-} $$
  • $$ PO_{4}^{3-}\rightarrow P_{2}O_{7}^{4-} $$
  • $$ C_{2}O_{4}^{-2}\rightarrow CO_{2} $$
Balance the following redou reaction
$$x M n O _ { 4 } ^ { - } + y F e ^ { + 2 } + z H ^ { + } \rightarrow a M n ^ { + 2 } + b F e ^ { + 3 } + c H _ { 2 } O$$
What is the ratio of $$( x + y + z ) / ( a + b + c ) ?$$
  • $$5 : 7$$
  • $$7 : 5$$
  • $$4 : 7$$
  • $$7 : 4$$
Which of the following reaction is non-redox?
  • $$2NaNO_{3}\rightarrow 2NaNO_{2}+O_{2}$$
  • $$CaO+SiO_{2}\rightarrow CaSiO_{3}$$
  • $$Fe+H_{2}SO_{4}\rightarrow FeSO_{4}+H_{2}$$
  • $$4Ag+8CN^{-}+O_{2}+2H_{2}O\rightarrow 4[Ag(CN)_{2}]^{-}+4OH^{-}$$
$$HOCl(aq)$$ is the molecule that kills bacteria wen chlorine is added to water. 
The following reaction produces this molecule
$${Cl}_{2}(g)+{H}_{2}O(l)\rightleftharpoons HOCl(aq)+{H}^{+}(aq)+{Cl}^{-}(aq)$$
Which statement about this reaction is correct?
  • Chlorine is both oxidised and reduced
  • Chlorine is oxidised but not reduced
  • Hydrogen is both oxidised and reduced
  • Hydrogen is oxidised but not reduced
Oxidation number of oxygen in ozone $$\left( \mathrm { O } _ { 3 } \right)$$ is:
  • $$+ 3$$
  • $$- 3$$
  • $$- 2$$
  • 0
The oxidation state of A, B, and C in a compound are +2, +5, and -2, respectively. The correct formula for the compound is:
  • $${ A }_{ 2 }\left( BC \right) _{ 2 }$$
  • $${ A }_{ 2 }\left( BC \right) _{ 3 }$$
  • $${ A }_{ 3 }\left( BC_{ 4 } \right) _{ 2 }$$
  • $${ A }_{ 2 }\left( BC_{ 4 } \right) _{ 3 }$$
Which of the following carbonyl compounds undergoes self redox reaction in presence of concentrated base?
  • 3-Methylpentanal
  • 2-Chlorobutanal
  • 2,2-Dimethylpropanal
  • tert-butyl methyl ketone.
Which of the following statement is correct?
  • $$ MnO^-_4 $$ is very good oxidant in acidic medium and liberates iodine when added to $$KI$$ solution by forming $$ MnO_2 $$.
  • $$ MnO^-_4 $$ is a very good oxidant in basic medium and liberates iodine when added to $$KI$$ solution by forming $$ MnO_2 $$.
  • $$ MnO^-_4 $$ is very good oxidant in acidic medium and liberates iodine when added to $$KI$$ solution by forming $$ Mn^{2+} $$.
  • $$ MnO^-_4 $$ is very good oxidant in basic medium and liberates iodine when added to $$KI$$ solution by forming $$ Mn^{2+} $$.
What is the molar concentration of the triiodide solution, $$KI_3$$(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a $$0.200\ mol/L$$, thiosulphate solution, $$K_2S_2O_3$$(aq) ?
The chemical equation for the reaction is:
$$2S_2O_3^{2-}(aq) + I_3^-(aq)\rightarrow S_4O_6^{2-} (aq)+3 I^-(aq)$$
  • 0.0333 M
  • 0.12 M
  • 0.0833 M
  • 0.00012 M
Balance the following redox reaction
$$xMnO_{4}^{-} + yFe^{+2} + zH^{+} \rightarrow aMn^{+2} + bFe^{+3} + cH_2O$$
What is the ratio of $$(x + y + z)/ (a + b + c)$$?
  • $$5 : 7$$
  • $$7 : 5$$
  • $$4 : 7$$
  • $$7 : 4$$
The dissociation constant for $$CH_{3}COOH$$ is $$1.8\times 10^{-5}$$ at $$298\ K$$. The electrode potential for the half-cell: $$Pt|H_{2}\ (1\ bar)\|0.5\ M\ CH_{3}COOH$$, at $$298\ K$$ is:

$$(log\ 2 = 0.3\ ;\ log\ 3 = 0.48\ ;\ 2.303\ RT/F = 0.06)$$
  • $$-0.3024\ V$$
  • $$-0.1512\ V$$
  • $$+0.3024\ V$$
  • $$+0.1512\ V$$
From the following $$E^{\circ}$$ values for the half-cells:


$$(i)\ D\rightarrow D^{2+}+2e^{-};E^{\circ}=-1.5V$$

$$(ii)\ B^{+}+e^{-}\rightarrow B;E^{\circ}=-0.5V$$

$$(iii)\ A^{3-}\rightarrow A^{2-}+e^{-};E^{\circ}=1.5V$$

$$(iv)\ C^{2+}+e^{-}\rightarrow C^{+};E^{\circ}= +0.5V$$

Which combination of two half-cells would result in a cell with the largest potential?
  • $$(i)$$ and $$(iii)$$
  • $$(i)$$ and $$(iv)$$
  • $$(iii)$$ and $$(iv)$$
  • $$(ii)$$ and $$(iv)$$
The value of $$n$$ in the reaction is:

$$Cr_{2}O_{7}^{2-}+14H^{+}+nFe^{2+}\rightarrow 2Cr^{3+}+nFe^{3+}+7H_{2}O$$
  • $$2$$
  • $$3$$
  • $$6$$
  • $$7$$
The atomic number of an element isThe highest oxidation state exhibited by it in its compounds is 
  • 1
  • 2
  • 3
  • 4
For the feasibility of a redox reaction in a cell, the emf should be 
  • Positive
  • Fixed
  • Zero
  • Negative
When $$ KMnO_4 $$ is reduced with oxalic acid in acidic solution, the oxidation number of Mn changes from
  • 7 to 4
  • 6 to 4
  • 7 to 2
  • 4 to 2
0:0:1


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