A quantity of $6\mathrm{.}75g$ of $S{O}_{2}C{l}_2$ was placed in a $2\mathrm{.}00L$ flask. At $648K,$ there is $0\mathrm{.}0345$ mole of $S{O}_2$ present. Calculate $K_c$ for the reaction below. Round your answer to $2$ significant digits.

$S{O}_{2}C{l}_2(g)S{O}_2(g)+C{l}_2(g)$

$10$