As is typical with these questions, we assume $100*g$ of unknown compound, and work out the MOLAR quantities of each element present:
$" moles of C":$ $(15.8*g)/(12.011*g*mol^-1)=1.32*mol$
$" moles of K":$ $(52.8*g)/(39.10*g*mol^-1)=1.35*mol$
$" moles of O":$ $(32.1*g)/(15.999*g*mol^-1)=2.00*mol$
Now if we divide thru by the lowest molar quantity, we get $CKO_(1.5)$; if we multiply this preiminary formula by $2$ we get whole numbers:
$C_2K_2O_3$ is the empirical formula.
But $"(empirical formula)"xxn$ $=$ $"molecular formula"$
Thus, solving for $n$:
$150.22*g*mol^-1=nxx(2xx12.011+2xx39.1+3xx15.999)*g*mol^-1$
Clearly, $n=1$, and the molecular formula is $C_2O_3K_2$
This corresponds to no reasonable formula I know; $C_2O_4K_2$ would be reasonable. It is possible that you have been given duff values.