Write a balanced chemical equation, assuming that the iron was oxidized to iron

Question

Write a balanced chemical equation, assuming that the iron was oxidized to iron (III) Include phases. Use this equation for calculations 2-5. Fe_(5) + CuCl_2(ag) rightarrow Cu(s) + FeCl_2 (ag) Model#1: Based on the masses of the starting materials (lines Band C), what is the theoretical yield of copper? CuCl_2 (s) = 1.87 g 3.6594_g Fe (1 mol Fe/55.845_g Fe) (1 mol FeCoCl_2/1 mol Fe) (190.30 g FeCuCl_2/1 mol Fe CuCl_2) Fe(s) = 3.6594g 1.87 gCuCl_2 (1 mol CuCl_2/134.45 g Cucl_2)(1 mol r x n/1 mol CuCl_2) = 0.0139 mol.

Explanation / Answer

1. The balanced chemical reaction for the process is given below :-   

2Fe(s) + 3CuCl2(aq) -----------> 3Cu(s) + 2FeCl3(aq)

Molar mass of CuCl2=134.45.

molar mass of fe = 55.84.

Moles of CuCl2 = 1.87/134.45 = 0.0139 gmol.

Moles of iron = 3.6599/55.84 = 0.0655 gmol.

According to the balanced reaction, 3 moles of CuCl2 will react with 2 moles of iron to give 3 moles of copper.

This means that 1 mol of CuCl2 will require 2/3 (0.66) mol of iron to give 1 mol of copper.

CuCl2 is the limiting reagent.

So 0.0139 gmol of CuCl2 will react to give 0.0139 gmol of copper.

Amount of copper produced = moles X molar mass

= 0.0139 X 63.54

= 0.883206 g.

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