One commercial system removes ${\mathrm{SO}}_2$ emission from smoke at $95°C$ by the following set of reactions :

$\begin{array}{l}{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶{\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right) ...\left(\mathrm{i}\right)\\ {\mathrm{SO}}_2{\mathrm{Cl}}_2+2{\mathrm{H}}_2\mathrm{O}⟶{\mathrm{H}}_2{\mathrm{SO}}_4+2\mathrm{HCl} ...\left(\mathrm{ii}\right)\\ {\mathrm{H}}_2{\mathrm{SO}}_4+\mathrm{Ca}(\mathrm{HO}{)}_2⟶{\mathrm{CaSO}}_4+2{\mathrm{H}}_2\mathrm{O} ...(\mathrm{iii})\end{array}$

Assuming the process to be $95\%$ efficient, how many moles of ${\mathrm{CaSO}}_4$ may be produced from $128g$${\mathrm{SO}}_2?[\mathrm{Ca}=40,\mathrm{S}=32,\mathrm{O}=16]$