A molecular compound containing only phosphorus and oxygen has the formula. A sample of the compound is found to contain 0.161 g of phosphorus and 0.290 g of oxygen. Theempirical formulaof the compound isP₁O₃, and the subscript of oxygen (y) in the formula is3.To determine the empirical formula of the compound, we need to find the simplestwhole-numberratio between the moles of phosphorus (P) and oxygen (O) in the sample.First, let's calculate the number ofmolesof each element:Molar mass of phosphorus (P) = 30.97 g/molMolar mass of oxygen (O) = 16.00 g/molMoles of phosphorus (P) = 0.161 g / 30.97 g/mol ≈ 0.0052 molMoles of oxygen (O) = 0.290 g / 16.00 g/mol ≈ 0.0181 molNext, we need to find theratioof moles between phosphorus and oxygen:Moles ratio: P:O = 0.0052 mol : 0.0181 molTo simplify this ratio, we can divide both values by the smallest value (0.0052 mol):P:O ≈ 1 : 3.48Since we are looking for the simplest whole-number ratio, we can round the ratio to thenearestwhole number:P:O = 1 : 3Therefore, the empirical formula of thecompoundis P₁O₃, and the subscript of oxygen (y) in the formula is 3.To know more aboutempirical formulaherebrainly.com/question/32125056#SPJ4...

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