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A mixture of 169.9 g of Cl₂ and 37.1 g of P reacts completely to form PCl₃ and PCl₅. Find the mass of PCl₅.

Answer :

Final answer:

The exact mass of PCl₅ formed from a mixture of 169.9g of Cl₂ and 37.1g of phosphorus (P) can't be determined without additional information. The limiting reactant needs to be identified, which will determine the amount of PCl₅ produced. Both PCl₃ and PCl₅ react with water, yielding hydrogen chloride and their respective oxyacids.

Explanation:

The question involves a chemical reaction between chlorine (Cl₂) and phosphorus (P), which forms two compounds: phosphorus trichloride (PCl₃) and phosphorus pentachloride (PCl₅). Given that 169.9g of Cl₂ and 37.1g of P reacts completely, we first need to identify which compound is the limiting reactant in this mixture. Since we don't have any further information regarding the exact reaction process, we were not able to directly calculate the mass of PCl₅.

However, it's important to understand that in stoichiometric reactions, the limiting reactant determines the amount of product produced. Regarding the molecular structures, both PCl₃ and PCl₅ react with water to yield hydrogen chloride and an oxyacid: PCl₃ yields phosphorous acid, H₃PO₃, and PCl₅ yields phosphoric acid, H₃PO₄.

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