[tex]\boxed{\begin{array}{c|c|c|c|c|c|c}\boxed{\bf{Element}} &\boxed{\bf{Percentage}} &{\boxed{\bf{Atomic\:mass}} &\boxed{\bf{Constant\:in\:Sample}} &\boxed{\bf No\:of\:moles} &\boxed{\bf{Sample\:Ratio}} &\boxed{\bf{Sample\:whole\:no\:ratio}}\\ &&&&&& \\ \sf C &\sf 50.84 &\sf 12 &\sf 50.84g &\sf{\dfrac{50.84}{12}=4.2} &\sf {\dfrac{4.2}{3.6}=1.16} &\sf 1 \\ &&&&&&\\ \sf H &\sf 8.53 &\sf 1 &\sf 8.53g &\sf{\dfrac{8.53}{1}=8.53} &\sf{$\dfrac{8.53}{3.6}$}=2.37} &\sf 2 \\&&&&&&\\ \sf O &\sf 57.69 &\sf 16 &\sf 57.69g &\sf{\dfrac{57.69}{16}=3.6} &\sf{\dfrac{3.6}{3.6}=1} &\sf 1\end{array}}[/tex]
Now
Empirical formula is
[tex]\\ \sf\bull\longmapsto C_1H_2O_1[/tex]
[tex]\\ \sf\bull\longmapsto CH_2O[/tex]
