How do you determine the empirical formula of a compound that has the following composition: 92.3 percent C and 7.7 percent H?

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How do you determine the empirical formula of a compound that has the following composition: 92.3 percent C and 7.7 percent H?

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Answer 1 · 2016-11-07T09:08:38

As with all these problems, we assume that there are $100 \cdot g$ $100*g$ of unknown compound........to give an empirical formula of $C H$ $CH$ .

Explanation:

And then we work out the molar composition.

Thus $Moles of carbon$ $"Moles of carbon"$ $=$ $=$ $\frac{92.3 \cdot g}{12.011 \cdot g \cdot m o l^{- 1}} = 7.68 \cdot m o l$ $(92.3*g)/(12.011*g*mol^-1)=7.68*mol$ .

And $Moles of hydrogen$ $"Moles of hydrogen"$ $=$ $=$ $\frac{7.7 \cdot g}{1.00794 \cdot g \cdot m o l^{- 1}} = 7.64 \cdot m o l$ $(7.7*g)/(1.00794*g*mol^-1)=7.64*mol$ .

Clearly, there is $1 : 1$ $1:1$ molar equivalence with respect to $C : H$ $C:H$ .

The molecular formula is a multiple of the empirical formula, but we have no handle on that here.

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How do you determine the empirical formula of a compound that has the following composition: 92.3 percent C and 7.7 percent H?

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Explanation:

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