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A 45.2 mg sample of phosphorus reacts with selenium to form 131.6 mg of the phosphorus selenide. determine the empirical formula of phosphorus selenide. what will be the simplest molecular formula of this compound

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barnuts

Phosphorus:

mass = 45.2 mg

molar mass = 30.97 mg / mmol

moles = 45.2 mg / (30.97 mg / mmol) = 1.46 mmol ≈ 1.5

 

Selenium:

mass = 131.6 mg – 45.2 mg = 86.4 mg

molar mass = 78.96 mg / mmol

moles = 86.4 mg / (78.96 mg / mmol) = 1.10 mmol ≈ 1

 

P1.5Se1

To get the empirical formula, we multiply with 2 to get whole numbers:

P3Se2

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