Imagine you are working on ways to improve the process by which Iron ore containing Fe2O3 is converted into Iron: Fe2O3 (s) + CO (g) Fe (s) + CO2 (g) If you start with 150g of Fe2O3 as the limiting reactant, what is the theoretical yield of Fe? If your actual yield is 87.9g, what is the percent yield?

Question

Chemistry

Eden Friedman

3 February, 10:59

Imagine you are working on ways to improve the process by which Iron ore containing Fe2O3 is converted into Iron: Fe2O3 (s) + CO (g) Fe (s) + CO2 (g) If you start with 150g of Fe2O3 as the limiting reactant, what is the theoretical yield of Fe? If your actual yield is 87.9g, what is the percent yield?

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Answers (1)

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Meredith Villegas · Answer 1

1. theoretical yield of Fe = 105g.

2. Percentage yield of Fe = 83.71%

Explanation:

Step 1:

Data obtained from the question. This includes:

The equation for the reaction:

Fe2O3 (s) + CO (g) - > Fe (s) + CO2 (g)

Mass of Fe2O3 = 150g

Actual yield of Fe = 87.9g

Theoretical yield of Fe = ?

Percentage yield of Fe =.?

Step 2:

Balancing the equation.

Fe2O3 (s) + CO (g) - > Fe (s) + CO2 (g)

The above equation can be balanced as follow:

There are 2 atoms of Fe on the left side and 1 atom on the right side. It can be balance by putting 2 in front of Fe as shown below:

Fe2O3 (s) + CO (g) - > 2Fe (s) + CO2 (g)

There are a total of 4 atoms of O on the left side and 2 atoms on the right side. It can be balance by putting 3 in front of CO and 3 in front of CO2 as shown below:

Fe2O3 (s) + 3CO (g) - > 2Fe (s) + 3CO2 (g)

Now the equation is balanced.

Step 3:

Determination of the mass of Fe2O3 that reacted and the mass of Fe produced from the balanced equation. This is illustrated below:

Fe2O3 (s) + 3CO (g) - > 2Fe (s) + 3CO2 (g)

Molar Mass of Fe2O3 = (56x2) + (16x3) = 112 + 48 = 160g/mol

Molar Mass of Fe = 56g/mol

Mass of Fe from the balanced equation = 2 x 56 = 112g

From the balanced equation,

160g of Fe2O3 reacted.

112g of Fe is produced.

Step 4:

Determination of the theoretical yield of Fe. This is illustrated below:

From the balanced equation,

160g of Fe2O3 produced 112g of Fe.

Therefore, 150g of Fe2O3 will produce = (150x112) / 160 = 105g of Fe.

Therefore, the theoretical yield of Fe is 105g.

Step 5:

Determination of the percentage yield of Fe. This is illustrated below:

Actual yield of Fe = 87.9g

Theoretical yield of Fe = 105g

Percentage yield of Fe =.?

Percentage yield = Actual yield/Theoretical yield x100

Percentage yield = 87.9/105 x 100

Percentage yield = 83.71%