$\mathrm{n}$ factor of nitrobenzene in this process is

The reducing agent in the given reaction is

${\mathrm{Fe}}_2{\mathrm{O}}_3+2\mathrm{Al}\to {\mathrm{Al}}_2{\mathrm{O}}_3+2\mathrm{Fe}$

Consider the given reaction as balanced equation in acidic medium

$\mathrm{aCr}{\left(\mathrm{OH}\right)}_3+{\mathrm{blO}}_3^{-}+{\mathrm{cOH}}^{-}\to {\mathrm{dl}}^{-}+{\mathrm{aCrO}}_4^{2-}+{\mathrm{eH}}_2\mathrm{O}$.

The ratio of $\mathrm{b}$ to $\mathrm{a}$ is

The oxidation number of $\mathrm{C}$ marked as (1) and (2) in the compound

$\begin{array}{cccccc}\mathrm{O}& =& \mathrm{C}& =& \mathrm{C}& =\\ & & \left(1\right)& & \left(2\right)& \end{array}\begin{array}{ccc}\mathrm{C}& =& \mathrm{O}\\ \left(3\right)& & \end{array}$, respectively are

Consider the given reaction

$\mathrm{Zn}+{\mathrm{NO}}_3^{-}\to {\mathrm{Zn}}^{2+}+{\mathrm{NH}}_4^{+}$ (Basic medium)

The balanced equation for the given reaction is

The oxidant in the given reaction is

$2{\mathrm{FeCl}}_3\left(\mathrm{aq}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2{\mathrm{FeCl}}_2\left(\mathrm{aq}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)$