By using the molar masses of the products obtained in the reaction, we can calculate that the mass P₄O₆ formed is 125.1 g, and the mass of P₄O₁₀ formed is 162.2 g.
If the phosphorus (P) and oxygen (O₂) react completely, then the total mass of the reactants will be equal to the total mass of the products. So, if we label the mass of P₄O₆ as X, and the mass of P₄O₁₀ as Y, we know that:
X + Y = m(P) + m(O₂)
X + Y = 141.3 g + 146.0 g
X + Y = 287.3 g
X = 287.3 g - Y
Now, all the phosphorus has been used in the oxidation reaction. So, if we wanted to calculate the mass of phosphorus in P₄O₆, we would use its molar mass (M = 220 g/mol):
4 * 31 g : 220 g = mass of P in P₄O₆ : X
mass of P in P₄O₆ = 124 * X / 220
mass of P in P₄O₆ = 0.5636 * X
We can do the same for the mass of phosphorus in P₄O₁₀ (M = 284 g/mol):
4 * 31 g : 284 g = mass of P in P₄O₁₀ : Y
mass of P in P₄O₁₀ = 124 * Y / 284
mass of P in P₄O₁₀ = 0.4366 * Y
We know that the total mass of P used is 141.3 g, so:
mass of P in P₄O₆ + mass of P in P₄O₁₀ = 141.3 g
0.5636 * X + 0.4366 * Y = 141.3 g
If we substitute X from the first set of unknowns, we get:
0.5636 * (287.3 g - Y) + 0.4366 * Y = 141.3 g
161.9 g - 0.5636 * Y + 0.4366 * Y = 141.3 g
20.6 g = 0.127 * Y
Y = 20.6 g / 0.127
Y = 162.2 g
X = 287.3 g - 162.2 g
X = 125.1 g
You can learn more about the molar mass here:
brainly.com/question/12127540
#SPJ4
