Consider the following unbalanced reaction: Fe2O3 (s) + CO (g) --> Fe (s) + CO2 (g) How many moles of carbon dioxide are produced per mole of iron (III) oxide reacted?
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You must balance the equation first.
Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g)
Now I see 3 mols CO2 per 1 mol Fe2O3.
To determine the number of moles of carbon dioxide produced per mole of iron (III) oxide, we need to balance the equation first.
The given unbalanced equation is: Fe2O3 (s) + CO (g) --> Fe (s) + CO2 (g)
Step 1: Balancing the number of iron atoms
Since there are two iron atoms on the left side and only one on the right side, we need to put a coefficient of 2 in front of Fe on the product side:
Fe2O3 (s) + CO (g) --> 2Fe (s) + CO2 (g)
Step 2: Balancing the number of oxygen atoms
There are three oxygen atoms on the left side from the Fe2O3 compound. To balance the equation, we put a coefficient of 3/2 in front of the oxygen-containing compound on the product side:
3/2 Fe2O3 (s) + CO (g) --> 2Fe (s) + CO2 (g)
Now, let's determine the ratio of moles of carbon dioxide (CO2) to moles of iron (III) oxide (Fe2O3) based on the balanced equation.
From the balanced equation:
1 mole of Fe2O3 reacts to produce 1 mole of CO2
Therefore, the ratio is 1:1. For every mole of iron (III) oxide reacted, one mole of carbon dioxide is produced.