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What is the empirical formula of a compound that contains 32.39 percent sodium 22.53 percent sulfur and 45.07 percent oxygen?
Wiki User
∙ 6y ago
First assume you have 100 g of the substance & then convert to moles using the molecular weight of each element:
Na: 32.39 g / (22.99 g/mol) = 1.409 mol Na
S : 22.53 g / (32.07 g/mol) = 0.703 mol S
O : 45.07 g / (16.00 g/mol) = 2.817 mol O
Next divide each mole amount by the smallest one of the group, in this case sulfur. This gives you the ratio of each element in the compound.
Na: 1.409 mol / 0.703 mol = 2.00
S : 0.703 mol/0.703 mol = 1.00
O: 2.817 mol/0.703 mol = 4.01
Round to the nearest whole number & you get the formula: Na2SO4 (sodium sulfate)
Wiki User
∙ 6y ago
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Percent composition can be used to calculate the percentage of an element/compound in a mixture. From the percent composition, you can also find the empirical formula. And from the empirical formula you can find the actual molecular weight.
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