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(C) Calculate the moles of each element present in $116 \ g$ of the substance:Moles of $H = \frac{7.5 \ g}{1 \ g/mol} = 7.5 \ mol$Moles of $O = \frac{

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$2$

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(C) Calculate the moles of each element present in $116 \ g$ of the substance:Moles of $H = \frac{7.5 \ g}{1 \ g/mol} = 7.5 \ mol$Moles of $O = \frac{60 \ g}{16 \ g/mol} = 3.75 \ mol$Moles of $C = \frac{48.5 \ g}{12 \ g/mol} \approx 4.04 \ mol$Dividing by the smallest value $(3.75)$:$H: \frac{7.5}{3.75} = 2$$O: \frac{3.75}{3.75} = 1$$C: \frac{4.04}{3.75} \approx 1.08 \approx 1$The empirical formula is $CH_2O$.Now,check the given options for the empirical formula $CH_2O$:$(A)$ $CH_3COOH$ is $C_2H_4O_2$,which simplifies to $CH_2O$.$(B)$ $HCHO$ is $CH_2O$,which simplifies to $CH_2O$.$(C)$ $CH_3OOCH_3$ is $C_2H_6O_2$,which does not simplify to $CH_2O$.$(D)$ $CH_3CHO$ is $C_2H_4O$,which does not simplify to $CH_2O$.Thus,$2$ formulae ($A$ and $B$) agree with the empirical formula $CH_2O$.

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