Pyrite, also known as fool's gold, is used commercially to produce SO2 used in the production of paper products. How many moles of SO2 can be produced from 1.0 kg of pyrite?

Verified step by step guidance

1. Identify the chemical formula of pyrite, which is FeS2.
2. Write the balanced chemical equation for the reaction of pyrite with oxygen to produce sulfur dioxide (SO2): 4FeS2 + 11O2 -> 2Fe2O3 + 8SO2.
3. Calculate the molar mass of FeS2 by adding the atomic masses of iron (Fe) and sulfur (S).
4. Convert the mass of pyrite (1.0 kg) to grams, then use the molar mass of FeS2 to convert grams to moles of FeS2.
5. Use the stoichiometry from the balanced equation to convert moles of FeS2 to moles of SO2.

Key Concepts

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to calculate how much of a substance is needed or produced based on the balanced chemical equation. Understanding stoichiometry is essential for determining the moles of SO2 produced from a given mass of pyrite.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles. To find out how many moles of SO2 can be produced from 1.0 kg of pyrite, one must first calculate the molar mass of pyrite and then use it in stoichiometric calculations.

Chemical Reaction of Pyrite

The chemical reaction of pyrite (FeS2) involves its oxidation to produce sulfur dioxide (SO2) and iron oxides. The balanced equation for this reaction is essential for determining the mole ratio between pyrite and SO2. Knowing this ratio allows for accurate calculations of how many moles of SO2 can be generated from a specific amount of pyrite.