In the given balanced chemical reaction,


\(\mathrm{IO}_3^{-}+\mathrm{aI}^{-}+\mathrm{bH}^{+} \rightarrow \mathrm{cH}_2 \mathrm{O}+\mathrm{dI}_2\)

The values of a, b, c, and d respectively are-

1. 5, 6, 3, 3

2. 5, 3, 6, 3

3. 3, 5, 3, 6

4. 5, 6, 5, 5

Subtopic:  Balancing of Equations |
 80%
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The standard electrode potential (E°) values of  Al3+/ Al,  Ag+ / Ag, K+ / K,  and Cr3+ / Cr are –1.66 V, 0.80 V, –2.93 V, & –0.79 V respectively. The correct decreasing order of the reducing power of the metal is:

1. Ag > Cr > Al > K 2. K > Al > Cr > Ag
3. K > Al > Ag > Cr 4. Al > K > Ag > Cr
Subtopic:  Emf & Electrode Potential |
 73%
From NCERT
NEET - 2019
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Balance the following equation and choose the quantity that is the sum of the coefficients of reactants and products :

...PtCl4+...XeF2PtF6+....ClF+...Xe

1. 16

2. 13

3. 18

4. 12

Subtopic:  Balancing of Equations |
 69%
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The reaction that does not represent auto redox or disproportionation is: 

1. Cl2+OH-Cl-+ClO3-+H2O

2. 2H2O2H2O+O2

3. 2Cu+Cu2++Cu

4. NH42Cr2O7N2+Cr2O3+4H2O

Subtopic:  Introduction to Redox and Oxidation Number |
 75%
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Among the following the correct order of acidity is-

1. HClO < HClO2< HClO3< HClO4
2. HClO2< HClO < HClO3< HClO4
3. HClO4< HClO2< HClO < HClO3
4. HClO3< HClO4< HClO2< HClO

Subtopic:  Oxidizing & Reducing Agents |
 85%
From NCERT
NEET - 2016
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What is the alteration in the oxidation state of carbon in the given reaction?

\(\mathrm{{CH_4}_{(g)} + 4{Cl_2}_{(g)} \rightarrow {CCl_4}_{(l)} + 4 HCl_{(g)}}\)

1. 0 to +4

2. –4 to +4

3. 0 to –4

4. +4 to +4

Subtopic:  Oxidizing & Reducing Agents |
 82%
From NCERT
NEET - 2020
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The change in oxidation number of chlorine when Cl2 gas reacts with hot and concentrated sodium hydroxide solution is:

1. Zero to +1 and Zero to –5

2. Zero to –1 and Zero to +5

3. Zero to –1 and Zero to +3

4. Zero to +1 and Zero to –3

Subtopic:  Oxidizing & Reducing Agents |
 69%
From NCERT
AIPMT - 2012
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For the redox reaction,
 aMnO4-+bC2O42-+cH+dMn2++eCO2+fH2O
the correct stoichiometric coefficients of the reactants a, b, and c respectively for the balanced equation are: 

1. 16, 5, 2
2. 2, 5, 16
3. 2, 16, 5
4. 5, 16, 2

Subtopic:  Balancing of Equations |
 79%
From NCERT
NEET - 2018
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MnO42- undergoes disproportionation reaction in acidic medium but MnO4- does not. It is:

1.  Due to the highest oxidation state of Mn in  MnO42-
2.  Due to the highest oxidation state of Mn in  MnO4-
3.  Due to the endothermic nature of the disproportionation reaction.
4.  Due to the exothermic nature of the disproportionation reaction.

Subtopic:  Introduction to Redox and Oxidation Number |
 81%
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(a) \(E_{k^+/K}^o = - 2.93\ V\); \(E_{Ag^+/Ag}^o = 0.80\ V\)
(b) \(E_{Hg^{2+}/Hg}^o = 0.79\ V\); \(E_{Mg^{2+}/Mg}^o = - 2.37\ V\)  
(c) \(E_{Cr^{3+}/Cr}^o = -0.74\ V\)

Based on standard electrode potentials given above, the correct arrangement for increasing order of reducing power of
elements is: 

1. \(\mathrm{Ag}<\mathrm{Hg}<\mathrm{Cr}<\mathrm{Mg}<\mathrm{K} \)
2. \(\mathrm{Ag}>\mathrm{Cr}>\mathrm{Mg}>\mathrm{Hg}>\mathrm{K}\)
3. \(\mathrm{K}>\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}>\mathrm{Ag} \)
4. \(\mathrm{K}<\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}<\mathrm{Ag}\)
Subtopic:  Emf & Electrode Potential |
 74%
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