According to the following reaction, how many moles of Fe(OH) ₂ can form from 175.0 mL of 0.227 mol L^-1 LiOH solution? Assume that there is excess FeCl₂.
FeCl₂(aq) + 2LiOH(aq) → Fe(OH) ₂(s) + 2LiCl(aq)

Question

Quizplus · Accepted Answer

First, we need to find the number of moles of LiOH we have: 0.227 mol/L x 0.175 L = 0.0396 mol LiOH According to the balanced equation, we need 2 moles of LiOH to form 1 mole of Fe(OH)2. Therefore, the number of moles of Fe(OH)2 that can form is: 0.0396 mol LiOH x (1 mol Fe(OH)2 / 2 mol LiOH) = 0.0198 mol Fe(OH)2 However, the question asks for the number of moles of Fe(OH)₂, which has a molar mass of 89.87 g/mol. We can use the following formula to convert moles to grams: moles = mass (g) / molar mass (g/mol) Rearranging the formula gives us: mass (g) = moles x molar mass (g/mol) Therefore, mass (Fe(OH)2) = 0.0198 mol x 89.87 g/mol = 1.78 g So approximately 1.78g is formed. Therefore, the answer is C: 1.99 × 10^-2 moles

According to the Following Reaction, How Many Moles of Fe(OH)2

According to the Following Reaction, How Many Moles of Fe(OH)₂