What is the molecular formula of each compound if the empirical formula is CH and the actual molar mass of compound is 78 g/mole?

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What is the molecular formula of each compound if the empirical formula is CH and the actual molar mass of compound is 78 g/mole?

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Answer 1 · 2018-03-02T08:42:09

The molecular formula is $C_{6} H_{6}$ $C_6H_6$ .

Explanation:

First, calculate the molar mass of the empirical formula, $C H$ $CH$ by adding the molar mass of carbon and hydrogen.

$12 + 1 = 13 l g$ $12 + 1 = 13color(white)(l)g$ / $m o l l C H$ $molcolor(white)(l)CH$

Now, divide the molar mass of the molecular compound (actual molar mass) by the molar mass of $C H$ $CH$ to see how many times more massive the actual compound is.

$\frac{78}{13} = 6$ $78/13=6$ times more massive

After multiplying each atom in the empirical formula by 6, we know the molecular formula is $C_{6} H_{6}$ $C_6H_6$ .

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What is the molecular formula of each compound if the empirical formula is CH and the actual molar mass of compound is 78 g/mole?

1 Answer

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