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2 years ago

What is the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen

1 answer:

6 0

Carbon(C):
number of moles= mass/molar mass(Mr)
=65.5/12
=5.5 moles

Hydrogen(H):
number of moles=mass/molar mass (Mr)
=5.5/1
=5.5 moles

Oxygen (O):
number of moles = mass/molar mass (Mr)
=29.0/16
=1.8 moles

EF= lowest number of moles over each of the elements

So,
C= 5.5/1.8 = 3
H= 5.5/1.8 = 3
O= 1.8/1.8 = 1

Therefore Emperical formula= C3H3O

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The moles of reactant and product in a chemical reaction to the whole number ratio is given by the stoichiometric coefficient of the balanced chemical equation.

<h3>Computation for the moles of oxygen</h3>

The balanced chemical equation for the reaction is :

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From the balanced chemical equation, the 2 moles of acetylene react with 5 moles of oxygen.

The moles of oxygen react with 1 mole of acetylene are:

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The moles of oxygen required to completely react with 1-mole acetylene is 2.5 mol.

Learn more about moles reacted, here:

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