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scZoUnD [109]
2 years ago
9

Determine the empirical formula for a compound that contains 48.6%C, 8.2% H, and 43.2% S by mass.

Chemistry
1 answer:
vagabundo [1.1K]2 years ago
4 0

The empirical formula for a compound that contains 48.6%C, 8.2% H, and 43.2% S by mass is C_3H_6S.

<h3>What is the empirical formula?</h3>

An empirical formula tells us the relative ratios of different atoms in a compound.

We need to calculate the number of moles

Number of a mole of carbon =

48.6 g X (\frac{1 mole }{ 12.0107 g}) =4.05 mole

Number of a mole of hydrogen =

8.2g X (\frac{1 mole}{.00784g}) =8.14 mole

Number of moles of sulphur =

43.2g X (\frac{ mole}{32.065g}) = 1.35 mole

Dividing each mole using the smallest number that is divided by 1.35 moles.

Carbon= \frac{4.05 mole }{1.35 mole} =3

Oxygen= \frac{8.14 mole}{1.35 mole} =6

Sulfur= \frac{1.35 mole}{1.35 mole} =1

Empirical formula is C_3H_6S

Learn more about empirical formula here:

brainly.com/question/14044066

#SPJ1

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How many MOLES of boron tribromide are present in 3.20 grams of this compound ?
Dmitriy789 [7]

Answer:

1) There are 0.0128 moles of BBr3 present in 3.20 grams of this compound

2) There are 909.35 grams of BBr3 present in 3.63 moles of this compound

Explanation:

<u>Step 1: </u>Given data

Boron tribromide = BBr3

Molar mass of Boron = 10.81 g/mole

Molar mass of Bromide = 79.9 g/mole

Molar mass of Boron tribromide = 10.81 + 3*79.9 = 250.51 g/mole

<u>Step 2:</u> Calculating number of moles

Number of moles = mass / molar mass

Number of moles of BBr3 = 3.20 grams / 250.51 g/mole

Number of moles of BBr3 = 0.0128 moles

<u>Step 3:</u> Calculating mass

If we have 3.63 moles of boron tribromide (= BBr3)

Mass of BBr3 = number of moles of BBr3 * Molar mass of BBr3

Mass of BBr3 = 3.63 moles * 250.51 g/mole

Mass of BBr3 = 909.35 grams

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