${\mathrm{Cl}}_2+\mathrm{KOH}\stackrel{60\%}{⟶}\mathrm{KCl}+\mathrm{KClO}+{\mathrm{H}}_2\mathrm{O}$

$\mathrm{KClO}\stackrel{50\%}{⟶}\mathrm{KCl}+{\mathrm{KClO}}_3$

${\mathrm{KClO}}_3\stackrel{80\%}{⟶}{\mathrm{KClO}}_4+\mathrm{KCl}$

$112\mathrm{L} {\mathrm{Cl}}_2$ gas at $\mathrm{STP}$ is passed in$10\mathrm{L} \mathrm{KOH}$ solution, containing $1$ mole of potassium hydroxide per litre.

Calculate the total moles of $\mathrm{KCl}$ produced, rounding it off to nearest whole number. (Yield of chemical reactions are written above the arrow$(\to )$ of respective reaction).

If $240 \mathrm{g}$ of carbon is taken in a container to convert it completely to ${\mathrm{CO}}_2$ but in industry it has been found that $280 \mathrm{g}$ of $\mathrm{CO}$ was also formed along with ${\mathrm{CO}}_2$. Find the mole percentage yield of ${\mathrm{CO}}_2$. The reactions occurring are:

$\mathrm{C}+{\mathrm{O}}_2⟶{\mathrm{CO}}_2;\mathrm{C}+\frac{1}{2}{\mathrm{O}}_2⟶\mathrm{CO}$

$92 \mathrm{g}$ mixture of ${\mathrm{CaCO}}_3$, and ${\mathrm{MgCO}}_3$ heated strongly in an open vessel. After complete decomposition of the carbonates it was found that the weight of residue left behind is $48 \mathrm{g}$. Find the mass of ${\mathrm{MgCO}}_3$ in grams in the mixture.