When phosphorus reacts with chlorine, phosphorus trichloride is formed according to the following equation: ___P₄(s) + ___Cl₂(g)$\rightarrow$___PCl₃(l) (unbalanced) Balance the equation and determine how many grams of chlorine would be required to react with 21.2 g of phosphorus.

Question

Quizplus · Accepted Answer

The balanced equation is P4 + 6Cl2 → 4PCl3. The molar mass of P is 30.97 g/mol, so 21.2 g of P is 0.684 mol. According to the balanced equation, 6 moles of Cl2 are needed for every mole of P4, which means 1.026 moles of Cl2 are needed. The molar mass of Cl2 is 70.90 g/mol, so 1.026 moles of Cl2 is 72.8 g.

When Phosphorus Reacts with Chlorine, Phosphorus Trichloride Is Formed According →\rightarrow→

When Phosphorus Reacts with Chlorine, Phosphorus Trichloride Is Formed According $\rightarrow$