
Concept explainers
Interpretation: The mass of iron (III) oxide produced on heating 1.25 g of iron and 0.0204 mole of oxygen gas needs to be calculated.
Concept introduction: The ratio of the mass of a substance to its molar mass is said to be the number of moles of that substance.

Answer to Problem 38A
The mass of iron (III) oxide produced on heating 1.25 g of iron and 0.0204 mole of oxygen gas is
Explanation of Solution
The chemical equation for the formation of iron(III) oxide from iron and oxygen gas is:
The above reaction is not balanced as the number of atoms of Fe and O is 1 and 2 on the reactant side and 2 and 3 on the product side.So in order to balance the reaction, coefficient 4 and 3 are written before Fe and O2 respectively on the reactant side and coefficient 2 is written before Fe2O3 on the product side. Thus, the balanced equation is:
The mass of iron (III) oxide produced will be calculated after determining the limiting reagent (The reagent in a reaction that controls the amount of product formed is termed as limiting reagent. After completion of
Calculating the moles of iron as:
The molar mass of iron is 55.845 g/mol. The number of moles of ironwill be:
The given mole of oxygen gas is 0.0204 mol.
In the above-balanced reaction, 4.0 mol of
Since, the required moles of
From the balanced chemical reaction, the mole ratio of
Now, the mass of iron(III) oxide produced is calculated as:
The molar mass of iron(III) oxide is 159.69 g/mol. So,
Hence, the mass of iron (III) oxide produced on heating 1.25 g of iron and 0.0204 mole of oxygen gas is
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