Answer:
A. 11.83g
B. 71.9%
Explanation:
We'll begin by writing the balanced for the reaction. This is shown below:
Fe + 2HCl —> FeCl2 + H2
A. Step 1
Determination of the mass of HCl that reacted and the mass of FeCl2 produced from the balanced equation. This is illustrated below:
Molar Mass of HCl = 1 + 35.5 = 36.5g/mol
Mass of HCl from the balanced equation = 2 x 36.5 = 73g
Molar Mass of FeCl2 = 56 + (35.5x2) = 56 + 71 = 127g
Summary:
From the balanced equation above,
73g of HCl produced 127g of FeCl2.
A. Step 2:
Determination of the theoretical yield of FeCl2.
The theoretical yield of FeCl2 can be obtained as follow:
Fe + 2HCl —> FeCl2 + H2
From the balanced equation above,
73g of HCl produced 127g of FeCl2.
Therefore, 6.80g of HCl will produce = (6.80 x 127)/73 = 11.83g of FeCl2.
Therefore, the theoretical yield of FeCl2 is 11.83g
B. Determination of the percentage yield.
Actual yield = 8.51g
Theoretical yield = 11.83g
Percentage yield =?
Percentage yield = Actual yield/Theoretical yield x100
Percentage yield = 8.51/11.83 x100
Percentage yield = 71.9%
Therefore, the percentage yield of FeCl2 is 71.9%
