In the following redox reaction, 

${\mathrm{xFe}}^{2+}+{\mathrm{yCr}}_2{\mathrm{O}}_7^{2-}+14{\mathrm{H}}^{+}\to 6{\mathrm{Fe}}^{3+}+2{\mathrm{Cr}}^{3+}+{\mathrm{zH}}_2\mathrm{O}$

The value of x,y,z are :

1. x = 6, y = 1, z = 7

2. x = 3, y = 6, z = 8

3. x = 6, y = 2, z = 7

4. x = 4, y = 6, z = 7

Balance the following reaction and find the values of a, b and g, respectively

\(aKMnO_4 + bH_2O_2 + 3H_2SO_4 \rightarrow \)
\( dMnSO_4 + eK_2SO_4 + fO_2 + gH_2O\)

1. 2, 4, 8

2. 2, 5, 8

3. 10, 4, 16

4. 8, 5, 2

0.1 Mole of ${\mathrm{H}}_3{\mathrm{PO}}_{\mathrm{x}}$ is completely neutralised by 5.6 g KOH then thr true statement is :

1. x = 3 and given acid is dibasic

2. x = 4 and given acid has not P-H linkage

3. x = 2 and given acid does not form acid salt

4. All of these

When potassium permangante is titrated against ferrous ammonium sulphate in acidic medium, the equivalent weight of potassium permanganate is :

1. $\frac{\mathrm{molecular} \mathrm{weight}}{3}$

2. $\frac{\mathrm{molecular} \mathrm{weight}}{5}$

3. $\frac{\mathrm{molecular} \mathrm{weight}}{2}$

4. $\frac{\mathrm{molecular} \mathrm{weight}}{10}$

Equivalent weight of ${\mathrm{FeS}}_2$ in the half reaction, ${\mathrm{FeS}}_2\to {\mathrm{Fe}}_2{\mathrm{O}}_3+{\mathrm{SO}}_2$ is :

1. M/10

2. M/11

3. M/6

4. M/1

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

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

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

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

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