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

Ch.6 Chemical Reactions: Mole and Mass Relationships

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McMurry 8th Edition

Ch.6 Chemical Reactions: Mole and Mass Relationships

문제 73b

6장, 문제 73b

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

검증된 단계별 안내

Step 1: Write the balanced chemical equation for the reaction. Pyrite (FeS2) reacts with oxygen (O2) to produce sulfur dioxide (SO2) and iron(III) oxide (Fe2O3). The balanced equation is: 4FeS2 + 11O2 → 8SO2 + 2Fe2O3.

Step 2: Convert the mass of pyrite (1.0 kg) into grams, since molar mass is typically expressed in grams per mole. Use the conversion factor: 1 kg = 1000 g.

Step 3: Calculate the molar mass of pyrite (FeS2). Add the atomic masses of iron (Fe) and sulfur (S) from the periodic table: Molar mass of FeS2 = (1 × atomic mass of Fe) + (2 × atomic mass of S).

Step 4: Determine the number of moles of pyrite by dividing the mass of pyrite (in grams) by its molar mass. Use the formula: \( \text{moles of FeS}_2 = \frac{\text{mass of FeS}_2}{\text{molar mass of FeS}_2} \).

Step 5: Use the stoichiometric ratio from the balanced equation to calculate the moles of SO2 produced. From the equation, 4 moles of FeS2 produce 8 moles of SO2. Use the ratio \( \text{moles of SO}_2 = \text{moles of FeS}_2 \times \frac{8}{4} \).

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주요 개념

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the 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 solve the question, one must first calculate the molar mass of pyrite (FeS2) to determine how many moles correspond to 1.0 kg.

Chemical Reaction of Pyrite

The chemical reaction of pyrite (FeS2) typically involves its oxidation to produce sulfur dioxide (SO2). The balanced equation for this reaction is essential for understanding how many moles of SO2 can be generated from a specific amount of pyrite. Knowing the stoichiometric coefficients in the reaction allows for accurate calculations of product formation.