When phosphorus reacts with chlorine, phosphorus trichloride is formed according to the equation: ___P₄(s)+ ___Cl₂(g)→ ___PCl₃(l)(unbalanced)Balance the equation and determine how many grams of chlorine would be required to react with 10.6 g of phosphorus.

Question

Quizplus · Accepted Answer

The balanced equation is P4 + 6Cl2 → 4PCl3. The molar mass of P4 is 123.88 g/mol, and Cl2 is 70.90 g/mol. 10.6 g of phosphorus is 0.0855 mol. According to the balanced equation, 6 moles of Cl2 are needed for 1 mole of P4, so 0.0855 mol of P4 requires 0.513 mol of Cl2. This is equivalent to 36.4 g of Cl2.

When Phosphorus Reacts with Chlorine, Phosphorus Trichloride Is Formed According