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Problem: Iron(III) oxide reacts with carbon monoxide according to the equation:Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2 (g)A reaction mixture initially contains 22.55 g Fe2O3 and 14.00 g CO.Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

🤓 Based on our data, we think this question is relevant for Professor Ferguson's class at LEHIGH.

FREE Expert Solution

The reaction is:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)


Molar masses:

Fe2O3(s) = 159.69 g/mol

CO(g) = 28.01 g/mol

Fe(s) = 55.85 g/mol


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Problem Details

Iron(III) oxide reacts with carbon monoxide according to the equation:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2 (g)

A reaction mixture initially contains 22.55 g Fe2O3 and 14.00 g CO.

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ferguson's class at LEHIGH.