When phosphorus reacts with chlorine, phosphorus trichloride is formed according to the following equation: ___P₄(s)+ ___Cl₂(g)→ ___PCl₃(l)(unbalanced)Balance the equation and determine how many grams of phosphorus reactant would be required to produce 75.0 g of phosphorus trichloride, assuming there is sufficient chlorine available.

Question

Quizplus · Accepted Answer

The balanced equation is P4 + 6Cl2 → 4PCl3. The molar mass of PCl3 is 137.33 g/mol, so 75.0 g of PCl3 is 0.546 mol. From the balanced equation, 1 mol of P4 produces 4 mol of PCl3, so 0.546 mol of PCl3 requires 0.1365 mol of P4. The molar mass of P4 is 123.88 g/mol, so 0.1365 mol of P4 is 16.9 g.

When Phosphorus Reacts with Chlorine, Phosphorus Trichloride Is Formed According