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What Is The Empirical Formula Of A Compound Containing 43.66% Phosphorus And 56.34% Oxygen?

April 26, 2017compound containing empirical Formula oxygen Phosphorus

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What Is The Empirical Formula Of A Compound Containing 43.66% Phosphorus And 56.34% Oxygen?

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Let us assume the total mass is 100 grams and percentage of each element is their respective mass out of the total. P = 43.66 g O = 56.34 g 1. Convert the mass of each element to moles by using molar mass according to the periodic table: P = 43.66 g x 1 mol / 31 g = 1.4 (‘g’ gets crossed out) O = 56.34 g x 1 mol / 16 g = 3.52 2. Divide each mole value by the smallest mole value obtained: P = 1.4 / 1.4 = 1 O = 3.52 / 1.4 = 2.5 3.