The oxidation number of phosphorus in $\mathrm{Ba}{\left({\mathrm{H}}_2{\mathrm{PO}}_2\right)}_2$ is-

2 mole of ${\mathrm{N}}_2{\mathrm{H}}_4$ loses 16 mole of electron is being converted to a new compound X. Assuming that all of the N appears in the new compound. What is the oxidation state of 'N' in X ?

When ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ is converted to ${\mathrm{K}}_2{\mathrm{CrO}}_4$, the change in the oxidation state of chromium is :

When a manganous salt is fused with a mixture of ${\mathrm{KNO}}_3$ and solid NaOH, the oxidation number of Mn changes from +2 to :

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

Which species are oxidized and reduced in the reaction ?

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

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

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 statement is incorrect ?

Which of the following reactions does not represent auto redox or disproportionation?

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 ${\mathrm{MnO}}_4^{-},{\mathrm{C}}_2{\mathrm{O}}_4^{-},{\mathrm{H}}^{+}$;

The sum of the coefficients of the reactants for the given reaction is -

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

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

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

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 :

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

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

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

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

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

The oxidation state of Cr in ${\mathrm{CrO}}_6$ is -

The standard electrode potential (E$°$) value of ${\mathrm{Al}}^{3+}/\mathrm{Al}, {\mathrm{Ag}}^{+}/\mathrm{Ag}, {\mathrm{K}}^{+}/\mathrm{K, }\mathrm{and} {\mathrm{Cr}}^{3+}/\mathrm{Cr}$ are -1.66V, 0.80 V, -2.93 V, & -0.79 V respectively. The correct decreasing order of the reducing power of the metal is-

The species that does not contain peroxide ions is: