Question #2c86e

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Question #2c86e

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Answer 1 · 2017-05-08T12:09:24

The molecular formula will be $C_{6} H_{6}$ $C_6H_6$ ; no prizes for guessing what this molecule is......

Explanation:

As with all these problems, it is useful to assume that there is a $100 \cdot g$ $100*g$ mass of compound, and divide each elemental mass thru by the ATOMIC mass of each component.

And so..........

$moles of carbon \equiv \frac{92.5 \cdot g}{12.011 \cdot g \cdot m o l^{- 1}} = 7.70 \cdot m o l$ $"moles of carbon"-=(92.5*g)/(12.011*g*mol^-1)=7.70*mol$

$moles of hydrogen \equiv \frac{7.50 \cdot g}{1.00794 \cdot g \cdot m o l^{- 1}} = 7.50 \cdot m o l$ $"moles of hydrogen"-=(7.50*g)/(1.00794*g*mol^-1)=7.50*mol$

And if we divide thru by the LOWEST molar quantity we gets.....and empirical formula of $C H$ $CH$ .

But the molecular formula is always a whole number of the empirical formula:

$molecular formula = empirical formula \times n$ $"molecular formula"="empirical formula"xxn$

And so $78 \cdot g \cdot m o l^{- 1} = n \times (12.011 + 1.00794) \cdot g \cdot m o l^{- 1}$ $78*g*mol^-1=nxx(12.011+1.00794)*g*mol^-1$ ; clearly, $n = 6$ $n=6$ , and the $molecular formula$ $"molecular formula"$ is $C_{6} H_{6}$ $C_6H_6$ , which is what VERY common organic molecule?

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Question #2c86e

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