Iron metal reacts with hydrochloric acid as follows: 2Fe(s)+ 6HCl(aq)→ 2FeCl₃(aq)+ 3H₂(g)If 35.6 g of iron react with excess HCl, and 98.6 g of FeCl₃ are collected, what is the percent yield of FeCl₃?

Question

Quizplus · Accepted Answer

First, we need to calculate the theoretical yield of FeCl3 using stoichiometry:
From the balanced chemical equation: 2Fe(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2(g)
The molar ratio of Fe to FeCl3 is 2:1, so the moles of FeCl3 produced is:
35.6 g Fe x (1 mol Fe/55.85 g Fe) x (2 mol FeCl3/2 mol Fe) x (162.2 g FeCl3/1 mol FeCl3) = 85.4 g FeCl3
Therefore, the theoretical yield of FeCl3 is 85.4 g.
The percent yield is calculated as: actual yield/theoretical yield x 100%
Given that the actual yield is 98.6 g, the percent yield is:
Percent yield = 98.6 g FeCl3/85.4 g FeCl3 x 100% = 115.4%
Since the percent yield is greater than 100%, it is not possible and likely a calculation error. Therefore, the correct answer is C) 95.7%.

Iron Metal Reacts with Hydrochloric Acid as Follows: 2Fe(s)+ 6HCl(aq)→