Question

A compound contains 3.6gm of carbon and 1.2 gm of hydrogen only. Find its empirical formula?

Answer 1

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Answer 2

The Empirical Formula Is CH₄

GIVEN

mass of carbon = 3.6grams

mas of hydrogen = 1.2 grams

TO FIND

The empirical formula of the compound

SOLUTION:

The empirical formula of a compound is defined as the relative ratio of the atoms present in the compound.

To find the empirical formula we first need to calculate the mass % of all the elements in the compound.

The total mass of the compound = 3.6+1.2= 4.8 grams

$mass \: percentage \: of \: carbon \: = \frac{given \: weight \: of \: carbon}{mass \: of \: compound} \times 1 00$

$= \frac{3.6}{4.8} \times 100$

Mass% of carbon = 75%

Mass% of hydrogen = 100-75 = 25%

So, 100 grams of compound contains 75 grams of carbon and 25 grams of hydrogen.

Number Of Moles = Given Mass /Molar Mass

Moles of carbon = 75/12 = 6.2 moles

Mole of hydrogen = 25/1 = 25 moles

carbon has a lesser number of moles.

Now to find the Coefficient of carbon and hydrogen we will divide the moles of carbon by the number of moles of carbon

= 6.2/6.2 = 1

= 25/6.2 = 4.0

The coefficient calculated will become the subscript of in the chemical formula.

Hence, the empirical formula is CH₄

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