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Vera_Pavlovna [14]
3 years ago
15

What is the empirical formula of a compound containing 5.03 grams carbon, 0.42 grams hydrogen, and 44.5 grams chlorine?

Chemistry
2 answers:
PtichkaEL [24]3 years ago
4 0

Answer:

The right choice is CHCl₃

Explanation:

  • <u>To find the empirical formula firstly, change the mass to moles.</u>

For Carbon :

no. of moles = (mass / molar mass) = (5.03 g / 12  g/mol )=  0.42 mol

<u><em>For Hydrogen  :</em></u>

no. of moles = (mass / molar mass) = (0.42 g / 1  g/mol )=  0.42 mol

<u><em>For Chlorine :</em></u>

no. of moles = (mass / molar mass) = (44.5 g / 35.5 g/mol )=  1.25 mol

The ratio for Carbon and Hydrogen is  1 : 1

0.42 mol / 042 mol =1.00

  • <u> Then find a ratio between the moles. </u>

The ratio of Chlorine to both Carbon and Hydrogen is 3:1

1.25 mol / 0.42 mol = 2.98 ≅ 3

So the ratio is 1 C : 1 H : 3 Cl.

So, the right choice is CHCl₃

Carbon usually forms four bonds one to Hydrogen and 3 to Chlorine atoms.

Chlorine usually forms one bond to Carbon atom.

Hydrogen usually forms one bond Carbon atom.

Anon25 [30]3 years ago
3 0

Answer:

CHCl₃

Explanation :

In order to deduce the empirical fomula of the compound, we first express the masses given as moles:

Elements C H Cl

Masses given(g) 5.03 0.42 44.5

Then divide through by their respective molar masses:

Molar mass 12 1 35.5

(g/mol)

Number of

Moles(mol) 0.42 0.42 1.254

Dividing by

the smallest(0.42) 1 1 3

The empirical formula of the compound is

CHCl₃

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