Stoichiometry and Molar Ratios

Oct 13, 2025 by wbrum.org 70 views

Introduction

Chemical reactions involve the transformation of one or more substances into new substances. In this article, we will explore a specific chemical reaction between carbon disulfide gas (CS2) and oxygen gas (O2) to form sulfur dioxide gas (SO2) and carbon dioxide gas (CO2). We will use the concept of stoichiometry to determine the volume of sulfur dioxide produced when 5.9 m³ of carbon disulfide is consumed.

The Chemical Reaction

The chemical reaction between carbon disulfide and oxygen can be represented by the following equation:

CS2 (g) + 3O2 (g) → SO2 (g) + CO2 (g)

In this reaction, one mole of carbon disulfide reacts with three moles of oxygen to produce one mole of sulfur dioxide and one mole of carbon dioxide.

Stoichiometry and Molar Ratios

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, we need to determine the molar ratio between carbon disulfide and sulfur dioxide.

From the balanced chemical equation, we can see that one mole of carbon disulfide produces one mole of sulfur dioxide. Therefore, the molar ratio between CS2 and SO2 is 1:1.

Calculating the Volume of Sulfur Dioxide

To calculate the volume of sulfur dioxide produced, we need to know the volume of carbon disulfide consumed. We are given that 5.9 m³ of carbon disulfide is consumed.

First, we need to convert the volume of carbon disulfide from cubic meters (m³) to moles. The molar volume of a gas is 22.4 liters per mole (L/mol) at standard temperature and pressure (STP). We can use this value to convert the volume of carbon disulfide to moles.

Converting Volume to Moles

To convert the volume of carbon disulfide from cubic meters (m³) to liters (L), we can multiply by 1000 (since 1 m³ = 1000 L).

5.9 m³ × 1000 L/m³ = 5900 L

Next, we can convert the volume of carbon disulfide from liters (L) to moles using the molar volume of a gas (22.4 L/mol).

5900 L ÷ 22.4 L/mol = 263.39 mol

Calculating the Volume of Sulfur Dioxide

Now that we have the number of moles of carbon disulfide consumed, we can use the molar ratio between CS2 and SO2 to determine the number of moles of sulfur dioxide produced.

Since the molar ratio between CS2 and SO2 is 1:1, the number of moles of sulfur dioxide produced is equal to the number of moles of carbon disulfide consumed.

263.39 mol CS2 × (1 mol SO2 / 1 mol CS2) = 263.39 mol SO2

Converting Moles to Volume

Finally, we can convert the number of moles of sulfur dioxide produced to volume using the molar volume of a gas (22.4 L/mol).

263.39 mol SO2 × 22.4 L/mol = 5915.36 L

To convert the volume of sulfur dioxide from liters (L) to cubic meters (m³), we can divide by 1000 (since 1 m³ = 1000 L).

5915.36 L ÷ 1000 L/m³ = 5.915 m³

Conclusion

In this article, we used the concept of stoichiometry to determine the volume of sulfur dioxide produced when 5.9 m³ of carbon disulfide is consumed. We first converted the volume of carbon disulfide from cubic meters (m³) to moles, and then used the molar ratio between CS2 and SO2 to determine the number of moles of sulfur dioxide produced. Finally, we converted the number of moles of sulfur dioxide produced to volume using the molar volume of a gas.

The volume of sulfur dioxide produced is 5.915 m³.

References

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling
Q&A: Understanding the Chemical Reaction and Stoichiometry =====================================================

Frequently Asked Questions

Q: What is the chemical reaction between carbon disulfide and oxygen? A: The chemical reaction between carbon disulfide and oxygen can be represented by the following equation:

CS2 (g) + 3O2 (g) → SO2 (g) + CO2 (g)

Q: What is stoichiometry? A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.

Q: What is the molar ratio between carbon disulfide and sulfur dioxide? A: The molar ratio between carbon disulfide and sulfur dioxide is 1:1, meaning that one mole of carbon disulfide produces one mole of sulfur dioxide.

Q: How do I convert the volume of carbon disulfide from cubic meters (m³) to moles? A: To convert the volume of carbon disulfide from cubic meters (m³) to moles, you need to know the molar volume of a gas, which is 22.4 liters per mole (L/mol) at standard temperature and pressure (STP). You can use the following formula:

moles = volume (L) ÷ molar volume (L/mol)

Q: How do I calculate the volume of sulfur dioxide produced? A: To calculate the volume of sulfur dioxide produced, you need to know the number of moles of carbon disulfide consumed and the molar ratio between CS2 and SO2. You can use the following formula:

moles SO2 = moles CS2 × (1 mol SO2 / 1 mol CS2)

Q: What is the volume of sulfur dioxide produced when 5.9 m³ of carbon disulfide is consumed? A: The volume of sulfur dioxide produced is 5.915 m³.

Q: What are the units of measurement for the volume of sulfur dioxide produced? A: The units of measurement for the volume of sulfur dioxide produced are cubic meters (m³).

Q: What is the significance of stoichiometry in chemistry? A: Stoichiometry is important in chemistry because it allows us to predict the amounts of reactants and products in a chemical reaction.

Q: How can I apply stoichiometry to real-world problems? A: You can apply stoichiometry to real-world problems by using the molar ratios between reactants and products to determine the amounts of substances involved in a chemical reaction.

Q: What are some common applications of stoichiometry? A: Some common applications of stoichiometry include:

Calculating the amounts of reactants and products in a chemical reaction
Determining the amounts of substances involved in a chemical reaction
Predicting the outcomes of chemical reactions
Designing chemical reactions and processes

Conclusion

In this Q&A article, we have discussed the chemical reaction between carbon disulfide and oxygen, stoichiometry, and the calculation of the volume of sulfur dioxide produced. We have also answered some frequently asked questions about stoichiometry and its applications.