For the following reaction, 6.80 grams of hydrochloric acid are mixed with excess iron. The reaction yields 8.51 grams of iron(II) chloride. iron (s) + hydrochloric acid (aq) rightarrow iron(II) chloride (aq) + hydrogen (g) a. What is the theoretical yield of iron(II) chloride? grams b. What is the percent yield for this reaction?

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%

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