In $\mathrm{Fe}\left(\mathrm{II}\right)-{\mathrm{MnO}}_4^{-}$ titration, ${\mathrm{HNO}}_3$, is not used because :

1. it oxidises ${\mathrm{Mn}}^{2+}$

2. it reduces ${\mathrm{MnO}}_4^{-}$

3. it oxidises ${\mathrm{Fe}}^{2+}$

4. it reduces ${\mathrm{Fe}}^{3+}$ formed

Which species are oxidized and reduced in the given reaction?

${\mathrm{FeC}}_2{\mathrm{O}}_4+{\mathrm{KMnO}}_4\to {\mathrm{Fe}}^{3+}+{\mathrm{CO}}_2+{\mathrm{Mn}}^{2+}$

1. Oxidised : Fe,C ; Reduced : Mn

2. Oxidised : Fe; Reduced : Mn

3. Reduced : Fe,Mn ; Oxidised : C

4. Reduced : C; Oxidised : Mn,Fe

Reaction that shows ${\mathrm{H}}_2{\mathrm{O}}_2$ as a reducing agent is -

1. ${\mathrm{SO}}_2+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{H}}_2{\mathrm{SO}}_4$

2. $2\mathrm{KI}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2\mathrm{KOH}+{\mathrm{I}}_2$

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

4. ${\mathrm{Ag}}_2\mathrm{O}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2\mathrm{Ag}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

The following reaction describes the rusting of iron. 

$4\mathrm{Fe}+3{\mathrm{O}}_2\to 4{\mathrm{Fe}}^{3+}+6{\mathrm{O}}^{2-}$

Which one of the following statements is incorrect?

1. This is an example of a redox reaction

2. Metallic iron is reduced to ${\mathrm{Fe}}^{3+}$

3. ${\mathrm{Fe}}^{3+}$ is an oxidising agent

4. Metallic iron is a reducing agent

Which of the following reactions does not involve disproportionation process?

1. ${\mathrm{Cl}}_2+{\mathrm{OH}}^{-}\to {\mathrm{Cl}}^{-}+{\mathrm{ClO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}$

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

3. $2{\mathrm{Cu}}^{+}\to {\mathrm{Cu}}^{2+}+\mathrm{Cu}$

4. ${\left({\mathrm{NH}}_4\right)}_{2}C{r}_2{O}_7\to {\mathrm{N}}_2+{\mathrm{Cr}}_2{\mathrm{O}}_3+4{\mathrm{H}}_2\mathrm{O}$

Which of the following is a redox reaction?

1. ${\mathrm{H}}_2{\mathrm{SO}}_4$ with NaOH

2. Formation of ${\mathrm{O}}_3$ in the atmosphere

3. Evaporation of ${\mathrm{H}}_2\mathrm{O}$

4. Oxides of nitrogen forming nitrogen & oxygen from lightening

Which of the following is a redox reaction ?

1. $2\mathrm{Na}\left[\mathrm{Ag}{\left(\mathrm{CN}\right)}_2\right]+\mathrm{Zn}\to {\mathrm{Na}}_2\left[\mathrm{Zn}{\left(\mathrm{CN}\right)}_4\right]+2\mathrm{Ag}$

2. ${\mathrm{BaO}}_2+{\mathrm{H}}_2{\mathrm{SO}}_4\to {\mathrm{BaSO}}_4+{\mathrm{H}}_2{\mathrm{O}}_2$

3. ${\mathrm{N}}_2{\mathrm{O}}_5+{\mathrm{H}}_2\mathrm{O}\to 2{\mathrm{HNO}}_3$

4. ${\mathrm{AgNO}}_3+\mathrm{KI}\to \mathrm{AgI}+{\mathrm{KNO}}_3$

For the redox reaction, ${\mathrm{MnO}}_4^{-}+{\mathrm{C}}_2{\mathrm{O}}_4^{2-}+{\mathrm{H}}^{+}\to {\mathrm{Mn}}^{2+}+{\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}$, the correct coefficients of the reactants for the balanced reaction are respectively ${\mathrm{MnO}}_4^{-},{\mathrm{C}}_2{\mathrm{O}}_4^{-},{\mathrm{H}}^{+}$:

1. 2,5,16

2. 16,3,12

3. 15,16,12

4. 2,16,5

The sum of the coefficients of the reactants in the following reaction is :

$....{\mathrm{CS}}_2+.....{\mathrm{Cl}}_2\to {\mathrm{CCl}}_4+....{\mathrm{S}}_2{\mathrm{Cl}}_2$

1. 5

2. 3

3. 6

4. 4

Balance the following equation and choose the quantity that is the sum of the coefficients of reactants and products :

$...{\mathrm{PtCl}}_4+...{\mathrm{XeF}}_2\to {\mathrm{PtF}}_6+....\mathrm{ClF}+...\mathrm{Xe}$

1. 16

2. 13

3. 18

4. 12