Which element exhibits both positive and negative oxidation states?

The balanced equation for the reaction between chlorine and sulphur dioxide in water is-

The set of metals that can show disproportionation reaction is -

The maximum weight of nitric oxide that can be obtained starting only with 10.00 g of ammonia and 20.00 g of oxygen is -

In Fe_0.90O , Fe is present in +2 and +3 oxidation state. What is the mole fraction  of Fe³⁺ in the compound ? 

The correct decreasing order of following metals in which they displace each other from the solution of their salts is: 
           Al, Cu, Fe, Mg and Zn.

1) Al> Zn > Fe > Cu > Mg

2) Zn > Fe > Cu > Mg > Al

3) Mg > Al > Zn > Fe > Cu

4) Fe > Mg > Zn > Al > Cu

The correct statement about the electrolysis of an aqueous solution of ${\mathrm{AgNO}}_3$ with Ag electrode is-

The reactions of electrolysis for a dilute solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$ with platinum electrode are-

The correct statement about electrolysis of an aqueous solution of ${\mathrm{CuCl}}_2$ with Pt electrode is-

The oxidizing agent and reducing agent in the given reaction are

$$\begin{gathered} 3{\mathrm{N}}_2{\mathrm{H}}_{4\left(\mathrm{l}\right)}+4{\mathrm{ClO}}_{3\left(\mathrm{aq}\right)}^{-}\to \\ 6{\mathrm{NO}}_{\left(\mathrm{g}\right)}+4{\mathrm{Cl}}_{\left(\mathrm{aq}\right)}^{-}+6{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} \end{gathered}$$

The oxidising agent and reducing agent in the given reaction are

$$\begin{gathered} {\mathrm{Cl}}_2{\mathrm{O}}_{7\left(\mathrm{g}\right)}+4{\mathrm{H}}_2{\mathrm{O}}_{2\left(\mathrm{aq}\right)}+2{\mathrm{OH}}_{\left(\mathrm{aq}\right)}^{-}\to \\ 2{\mathrm{ClO}}_{2\left(\mathrm{aq}\right)}^{-}+4{\mathrm{O}}_{2\left(\mathrm{g}\right)}+5{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} \end{gathered}$$

Given a galvanic cell with the following reaction

${\mathrm{Zn}}_{\left(\mathrm{s}\right) } + 2{{\mathrm{Ag}}^{+}}_{\left(\mathrm{aq}\right)} \to {{\mathrm{Zn}}^{+2}}_{\left(\mathrm{aq}\right)} + {\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

The negatively charged electrode will be-

The oxidation states of the central atom in the given species are, respectively:

${\mathrm{H}}_4{\mathrm{P}}_2{\mathrm{O}}_7 \mathrm{and} {\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7$

${\mathrm{KI}}_3 , {\mathrm{H}}_2{\mathrm{S}}_4{\mathrm{O}}_6$

The oxidation numbers of iodine and sulphur in the above compounds are, respectively?

 $$\begin{gathered} 1. \frac{1}{3}; 4 \\ 2. 2.5; \frac{1}{3} \\ 3. \frac{1}{3}; 2.5 \\ 4. 2.5; 3 \end{gathered}$$

The metal displacement reaction among the following is -

2 Na(s) + H₂(g) → 2 NaH (s)
The incorrect statement among the following regarding above mentioned reaction is-

2Cu₂O(s) + Cu₂S(s) → 6Cu(s) + SO₂(g)
The correct statement among the following regarding above mentioned reaction is-

The species among the following that does not show a disproportionation reaction is-

ClO^–, ClO₂^–, \(ClO_{3}^{-}\) and ClO₄^–