Question

How many grams of iron metal can be produced from the reaction of 14.2 g of CO gas with 21.0 g of Fe2O3

Answer 1

14.7 grams of Fe

Step-by-step explanation

Given:

Mass of CO = 14.2 g

Mass of Fe₂O₃ = 21.0 g

What to find:

The grams of iron metal (Fe) produced.

Step-by-step solution;

The first step is to write a balanced chemical equation for the reaction:

`Fe_2CO_3+3CO\rightarrow2Fe+3CO_2`

The second step is to determine the limiting reactant

From the Periodic Table:

1 mol CO = 28.01 g

1 mol Fe₂O₃ = 159.69 g

1 mol Fe = 55.85 g

From the balanced equation;

3 mol x 28.01 g/mol = 84.03 g CO reacts with 1 mol x 159.69 g/mol = 159.69 g Fe₂O₃

So 14.2 g CO will react with

This implies that the given 14.2 g of CO will require 27.0 g Fe₂O₃. Note that the given mass of Fe₂O₃ that reacted is 21.0 g, hence Fe₂O₃ is the limiting reactant.

The final step is to use the limiting reactant to calculate the grams of Fe metal produced.

If from the balanced equation, 159.96 g Fe₂O₃ produced 2 x 55.85 g = 111.7 g Fe,

Therefore, 21.0 g Fe₂O₃ will produce:

Hence, 14.7 grams of iron metal can be produced from the reaction of 14.2 g of CO gas with 21.0 g of Fe₂O₃