Recall the **mass percent formula**:

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{mass}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{component}}{\mathbf{total}\mathbf{}\mathbf{mass}}{\mathbf{\times}}{\mathbf{100}}}$

**Assuming we have ****100-g sample**

$\mathbf{mass}\mathbf{\%}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{element}}{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{sample}}\mathbf{\times}\mathbf{100}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{mass}}{\mathbf{}}{\mathbf{element}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{\%}}{\mathbf{100}}{\mathbf{\times}}{\mathbf{mass}}{\mathbf{}}{\mathbf{of}}{\mathbf{}}{\mathbf{sample}}}$

**Percent H: 4.58%**

A compound isolated from the rind of lemons is found to be 88.14 % carbon and 11.86 % hydrogen by mass.

How many moles of H?

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