Eight moles of chlorine $\left({\mathrm{Cl}}_2\right)$ undergo a loss and gain of $14$$\mathrm{moles}$ of electrons to form two oxidation states of chlorine ($\mathrm{Cl}$). Write down the two half reactions and equation for disproportionation of chlorine, (${\mathrm{Cl}}_2$).

The values of$\mathrm{p}, \mathrm{q}, \mathrm{r}, \mathrm{s}$ and $\mathrm{t}$ in the following redox reaction are:

${\mathrm{pBr}}_2+{\mathrm{qOH}}^{-} \stackrel{}{\to } {\mathrm{rBr}}^{-}+{\mathrm{sBrO}}_3^{-}+{\mathrm{tH}}_2\mathrm{O}$

${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}+6{\mathrm{I}}^{-}+14{\mathrm{H}}^{+}⟶6{\mathrm{I}}_2+2{\mathrm{Cr}}^{3+}+7{\mathrm{H}}_2\mathrm{O}$

Which are not in balanced position?

What is the molecular state of sulphur as a reactant in the following reaction:

$\mathrm{Sulphur} +12{\mathrm{OH}}^{-}⟶4{\mathrm{S}}^{2-}+2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+3{\mathrm{H}}_2\mathrm{O}$

In balancing the half-reaction,

${\mathrm{CN}}^{-}⟶{\mathrm{CNO}}^{-}$ (skeletal) 

the number of electrons that must be added are:

In the following reaction (unbalanced), equivalent weight of ${\mathrm{As}}_2{\mathrm{S}}_3$ is related to molecular weight $\mathrm{M}$ by,

${\mathrm{As}}_2{\mathrm{S}}_3+{\mathrm{H}}^{+}+{\mathrm{NO}}_3^{-}⟶\mathrm{NO}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{AsO}}_4^{3-}+{\mathrm{SO}}_4^{2-}$

In the following unbalanced redox reaction,

${\mathrm{Cu}}_3\mathrm{P}+{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}⟶{\mathrm{Cu}}^{2+}+{\mathrm{H}}_3{\mathrm{PO}}_4+{\mathrm{Cr}}^{3+}$

The equivalent weight of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is: