Question #4b3f0

Feb 9, 2017

$H O$.........I wonder what it could be......?

Explanation:

As with all these empirical formulae problems, we assume a mass of $100 \cdot g$, and then we work out the atomic composition:

$\text{Moles of hydrogen:}$ $\frac{5.88 \cdot g}{1.00794 \cdot g \cdot m o {l}^{-} 1} = 5.83 \cdot m o l$

$\text{Moles of oxygen:}$ $\frac{94.12 \cdot g}{15.999 \cdot g \cdot m o {l}^{-} 1} = 5.88 \cdot m o l$

This is near enuff to equality with respect to moles. The empirical formula of the compound is thus $O H$. The likely molecule is $\text{hydrogen peroxide}$, $H O - O H$. How is this consistent with the empirical formula?