${\mathrm{KMnO}}_4$ is a strong oxidising agent in acidic medium. To provide acidic medium, ${\mathrm{H}}_2{\mathrm{SO}}_4$ is used instead of HCl. This is because

1. ${\mathrm{H}}_2{\mathrm{SO}}_4$ is stronger acid than HCl
2. HCl is oxidised by ${\mathrm{KMnO}}_4$ to ${\mathrm{Cl}}_2$
3. ${\mathrm{H}}_2{\mathrm{SO}}_4$ is dibasic acid
4. Rate is faster in the presence of ${\mathrm{H}}_2{\mathrm{SO}}_4$

What is the stoichiometric coefficient of sulfur (\(S\)) in the balanced equation for the following reaction in acidic medium?
\(\mathrm{H}_2 \mathrm{~S}(a q)+\mathrm{HNO}_3(a q) \rightarrow \mathrm{NO}(g)+\mathrm{S}(s)+\mathrm{H}_2 \mathrm{O}(l)\)

1. 1

2. 2

3. 3

4. 4

Equal volumes of 1M each of KMnO${}_4$ and ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ are used to oxidise Fe(II) solution in acidic medium.
The amount of Fe oxidised will be

1. More with KMnO${}_4$

2. More with ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$

3. Equal with both oxidising agents

4. Cannot be determined

The oxidation number of Pt in ${\left[\mathrm{Pt}\left({\mathrm{C}}_2{\mathrm{H}}_4\right){\mathrm{Cl}}_3\right]}^{-}$ is:

1. +1

2. +2

3. +3

4. +4

Oxidation state of nitrogen is incorrectly given for:      

A, B and C are three elements forming a part of
compound in oxidation states of +2, +5 and –2
respectively. What could be the compounds?

1. ${\mathrm{A}}_2{\left(\mathrm{BC}\right)}_2$

2. ${\mathrm{A}}_2{\left({\mathrm{BC}}_4\right)}_3$

3. ${\mathrm{A}}_3{\left({\mathrm{BC}}_4\right)}_2$

4. ABC

Consider the following reaction :

${\mathrm{xMnO}}_4^{-} + {\mathrm{yC}}_2{\mathrm{O}}_4^{2-} + {\mathrm{zH}}^{+} \to {\mathrm{xMn}}^{2+} +\hspace{0.17em}2{\mathrm{yCO}}_2 +\hspace{0.17em}\frac{\mathrm{z}}{2}{\mathrm{H}}_2\mathrm{O}$

The values of x, y and z in the reaction are
respectively :

1. 2, 5 and 16

2. 5, 2 and 8

3. 5, 2 and 16

4. 2, 5 and 8

Valency factor $\left({\mathrm{V}}_t\right)$ for following redox reaction is respectively.

a. ${\mathrm{As}}_2{\mathrm{S}}_3 \to {\mathrm{AsO}}_4^{-3}+{\mathrm{SO}}_4^{2-}$

b. ${\mathrm{I}}_2 \to {\mathrm{I}}^{-}+{\mathrm{IO}}_3^{-}$

c. ${\mathrm{H}}_3{\mathrm{PO}}_2 \to {\mathrm{PH}}_3+{\mathrm{H}}_3{\mathrm{PO}}_3$

1. $28, \frac{5}{3},\frac{4}{3}$

2. $28,\frac{4}{3},\frac{5}{3}$

3. $6, 4, 7$

4. 4, 3, 9

The oxidation number of phosphorus in Ba(H₂PO₂)₂ is:

1. +3

2. +2

3. +1

4. -1

The oxidation state of Cr in [Cr(NH₃)₄Cl₂]⁺ is:

1. +3

2. +2

3. +1

4. 0