Match Column I with Column II for the given properties/applications mentioned therein.

Codes

           A         B           C           D

1.       4          3           2           1

2.       1          2           3           4

3.       1          4           3           2

4.       4          1           3           2

Match the terms in Column I with the relevant item in Column II.

Codes

          A          B          C           D        

 1.      3          1           2           4        

 2.      3          4           2           1       

 3.      1          4           3           2        

 4.      4          1           3           2        

Consider the reactions

(i) ${\mathrm{H}}_2{\mathrm{O}}_2+2\mathrm{HI}\to {\mathrm{I}}_2+2{\mathrm{H}}_2\mathrm{O}$

(ii) $\mathrm{HOCl}+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{Cl}}^{-}+{\mathrm{O}}_2$

Which of the following statements is correct about H₂O₂ with reference to these reactions? Hydrogen peroxide is ______.

1.  an oxidising agent in both (i) and (ii)

2.  an oxidisng agent in (i) and reducing agent in (ii)

3.  a reducing agent in (i) and oxidising agent in (ii)

4.  a reducing agent in both (i) and (ii)

The oxide that gives ${\mathrm{H}}_2{\mathrm{O}}_2$ on treatment with dilute ${\mathrm{H}}_2{\mathrm{SO}}_4$ is

1. ${\mathrm{PbO}}_2$

2. ${\mathrm{BaO}}_2.8{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3. ${\mathrm{MnO}}_2$

4. ${\mathrm{TiO}}_2$

Which of the following equations depict the oxidising nature of ${\mathrm{H}}_2{\mathrm{O}}_2$?

1. $2{\mathrm{MnO}}_4^{-}+6{\mathrm{H}}^{+}+5{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{Mn}}^{2+}+8{\mathrm{H}}_2\mathrm{O}+5{\mathrm{O}}_2$

2. $2{\mathrm{Fe}}^{3+}+2{\mathrm{H}}^{+}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{Fe}}^{2+}+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3. $2{\mathrm{I}}^{-}+2{\mathrm{H}}^{+}+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{I}}_2+2{\mathrm{H}}_2\mathrm{O}$

4. ${\mathrm{KIO}}_4+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{KIO}}_3+{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

Which of the following equation depicts reducing nature of ${\mathrm{H}}_2{\mathrm{O}}_2$?

1. $2{\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]}^{4-}+2{\mathrm{H}}^{+}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]}^{3-}+2{\mathrm{H}}_2\mathrm{O}$

2.  ${\mathrm{I}}_2+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{OH}}^{-}\to 2{\mathrm{I}}^{-}+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3.  ${\mathrm{Mn}}^{2+}+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{Mn}}^{4+}+2{\mathrm{OH}}^{-}$

4.  $\mathrm{PbS}+4{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{PbSO}}_4+4{\mathrm{H}}_2\mathrm{O}$

Hydrogen peroxide is-

1. an oxidising agent

2. a reducing agent

3. both an oxidising and a reducing agent

4. neither oxidising nor reducing agent.

When sodium peroxide is treated with dilute sulphuric acid, we get _____.

1.  Sodium sulphate and water

2.  Sodium sulphate and oxygen

3.  Sodium sulphate, hydrogen and oxygen

4.  Sodium sulphate and hydrogen peroxide