The percent yield for the following reaction carried out in carbon tetrachloride $\left({\mathrm{CCl}}_4\right)$ solution is $80\%$.

${\mathrm{Br}}_2+{\mathrm{Cl}}_2⟶2\mathrm{BrCl}$

(a) What amount of $\mathrm{BrCl}$ would be formed from the reaction of $0.025 \mathrm{mol} {\mathrm{Br}}_2$ and $0.025 \mathrm{mol} {\mathrm{Cl}}_2$?
(b) What amount of ${\mathrm{Br}}_2$ is left unchanged?

${\mathrm{KCIO}}_3$ decomposes by two parallel reactions,

($i$) $2{\mathrm{KClO}}_3\stackrel{\Delta }{⟶}2\mathrm{KCl}+3{\mathrm{O}}_2$  ($ii$) $4{\mathrm{KClO}}_3\stackrel{\Delta }{⟶}3{\mathrm{KClO}}_4+\mathrm{KCl}$

If $3$ moles of ${\mathrm{O}}_2$ and$1\mathrm{mol}$ of ${\mathrm{KClO}}_4$ is produced along with other products, then determine the initial moles of ${\mathrm{KClO}}_3$.

Find the ${\mathrm{Cl}}^{-}$ concentration in solution which is obtained by mixing one mole each of ${\mathrm{BaCl}}_2,\mathrm{NaCl}$ and $\mathrm{HCl}$ in  $500\mathrm{ml}$ water.

What volume of water should be added to $50\mathrm{ml}$ of ${\mathrm{HNO}}_3$ having density $1.5{\mathrm{gml}}^{-1}$ and $63.0\%$ by weight to have one molar solution?