Question #4b3f0

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Question #4b3f0

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Answer 1 · 2017-02-09T16:43:15

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

Explanation:

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

$Moles of hydrogen:$ $"Moles of hydrogen:"$ $\frac{5.88 \cdot g}{1.00794 \cdot g \cdot m o l^{- 1}} = 5.83 \cdot m o l$ $(5.88*g)/(1.00794*g*mol^-1)=5.83*mol$

$Moles of oxygen:$ $"Moles of oxygen:"$ $\frac{94.12 \cdot g}{15.999 \cdot g \cdot m o l^{- 1}} = 5.88 \cdot m o l$ $(94.12*g)/(15.999*g*mol^-1)=5.88*mol$

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

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