Given the reaction: P₄(l)+ 6 Cl₂(g)→ 4 PCl₃(l) If the percent yield is 82%,what mass of P₄ is required to obtain 2.30 g PCl₃ (Cl₂ in excess)? A)0.63 g B)0.52 g C)0.43 g D)0.16 g E)0.95 g

Question

Quizplus · Accepted Answer

First, identify the molar masses of the compounds involved: $ P_4S_{10} $ (Molar mass = 444.56 g/mol) and $ PCl_3 $ (Molar mass = 137.33 g/mol). Given the reaction, 1 mole of $ P_4S_{10} $ produces 4 moles of $ PCl_3 $. To find the theoretical yield of $ PCl_3 $ from 1 mole of $ P_4S_{10} $, we use the stoichiometry of the reaction. Since the actual yield is 82% of the theoretical yield, we calculate the mass of $ P_4S_{10} $ needed to produce 2.30 g of $ PCl_3 $ at this yield. The calculation involves converting the mass of $ PCl_3 $ to moles, using the stoichiometry to find the moles of $ P_4S_{10} $ needed, and then converting this back to grams, taking into account the percent yield. The correct calculation leads to approximately 0.63 g of $ P_4S_{10} $ needed.

Given the Reaction: P4(l)+ 6 Cl2(g)→ 4 PCl3(l)

Given the Reaction: P₄(l)+ 6 Cl₂(g)→ 4 PCl₃(l)