A compound containing only carbon and hydrogen is analyzed, and is found to contain 20.11% hydrogen on a mass basis. How can the empirical formula of the compound be calculated?

Md Ariful Islam

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Md Ariful Islam

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In 100 g hydrocarbon, there are $(20.11*g)/(1.00794*g*mol^(-1)) = 19.95$ $mol$ $H$, and $(79.89*g)/(12.011*g*mol^(-1)) = 19.95$ $mol$ $C=6.65*mol$ $C$.

We then divide thru by the lowest ratio to give the empirical formula, $CH_3$.

How did I know that $%C$ was $79.89$?

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