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elena55 [62]
3 years ago
5

A 19.13 gram sample of chromium is heated in the presence of excess bromine. A metal bromide is formed with a mass of 77.92 g. D

etermine the empirical formula of the metal bromide.
Chemistry
1 answer:
vova2212 [387]3 years ago
6 0

Answer:

The empirical formula of the compound is CrBr_2.

Explanation:

Mass of chromium = 19.13 g

Mass metal bromide formed = 77.92 g

Mass of bromine in metal bromide = 77.92 g - 19.13 g = 58.79 g

Moles of chromium metal :

=\frac{19.13 g}{52 g/mol}=0.3679 mol

Moles of bromine:

=\frac{58.79 g}{80 g/mol}=0.7349 mol

For empirical formula divide the smallest number of moles of element from the all the moles of elements:

chromium : \frac{0.3679 mol}{0.3679}=1

bromine : \frac{0.7349 mol}{0.3679}=2

The empirical formula of the compound is CrBr_2.

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