\(0.4 \mathrm{~g}\) of dihydrogen is made to react with \(7.4 \mathrm{~g}\) of dichlorine to form hydrogen chloride. The volume of hydrogen chloride formed at \(273 \mathrm{~K}\) and 1 bar pressure is

\(71 \mathrm{~g} \mathrm{Cl}_{2}\) requires \(2 \mathrm{~g} \mathrm{H}_{2}\), than \(7.4 \mathrm{~g} \mathrm{Cl}_{2}\) will require, how much gram \(\mathrm{H}_{2}\).
\(\therefore \mathrm{H}_{2} \text { required }=\frac{2 \times 7.4}{71}=0.208 \mathrm{gm}\)
\(\therefore \mathrm{Cl}_{2}\) is limiting reagent \(\left[\because \mathrm{H}_{2}\right.\) is in excess \(]\)
\(\therefore\) Amount of \(\mathrm{HCl}\) formed will depend on \(\mathrm{Cl}_{2}\) gas
\(\begin{array}{rlr}
& 71 \mathrm{gm} \mathrm{Cl}_{2} & 44.8 \mathrm{~L} \mathrm{HCl} \\
& 7.4 \mathrm{gm} \mathrm{Cl}_{2} & x \mathrm{~L} \mathrm{HCl} \\
\therefore \quad & x=\frac{7.4 \times 44.8}{71} \\
& x=4.67 \mathrm{~L} \text { of } \mathrm{HCl} \text { gas is formed. }
\end{array}\)