A $9.48\mathrm{g}$ sample of potash alum, $\mathrm{KAl}(\mathrm{SO}{}_4){}_2\cdot 12\mathrm{H}{}_2\mathrm{O}$, is heated strongly until all water and all sulfur trioxide have been expelled, leaving a residue of $\mathrm{K}{}_2\mathrm{SO}{}_4$ and $\mathrm{Al}{}_2\mathrm{O}{}_3$ according to $2\mathrm{KAl}(\mathrm{SO}{}_4){}_2\to \mathrm{K}{}_2\mathrm{SO}{}_4+\mathrm{Al}{}_2\mathrm{O}{}_3+3\mathrm{SO}{}_3$. Using $\mathrm{K}=39$, $\mathrm{Al}=27$, $\mathrm{S}=32$, $\mathrm{O}=16$, $\mathrm{H}=1$, find the mass of the residue in grams, to two decimal places.

Numerical answer type, answer in g, tolerance 0.01.