Determining the Oxygen Required for the Complete Combustion of Sulfur

Understanding the chemical reactions and stoichiometry is essential in the field of chemistry, particularly when it comes to understanding how elements react with each other. One such reaction is the combustion of sulfur, a process that is both fundamental and illustrative of basic chemical principles. This article aims to explain the amount of oxygen required to completely burn 640 grams of sulfur, providing a step-by-step guide to solving this problem and offering insights into the importance of stoichiometry in chemical reactions.

Chemical Reaction and Stoichiometry

The combustion of sulfur can be described by the following balanced chemical equation:

S (s) O? (g) → SO? (g)

This equation tells us that one mole of sulfur (S) reacts with one mole of oxygen (O?) to produce one mole of sulfur dioxide (SO?). This fundamental relationship is key to determining the amount of oxygen required for the combustion of sulfur.

Understanding Molarity and Molar Mass

To properly understand the stoichiometry of this reaction, we need to understand the concept of molar mass. The molar mass of a substance is the mass per mole of that substance. For oxygen (O?), the molar mass is 16 g/mol for each oxygen atom, so the molar mass of O? is:

Molar mass of O? 16 g/mol × 2 32 g/mol

Calculation of Moles of Oxygen Required

Given 640 grams of sulfur (S), we need to determine how many moles of oxygen (O?) are required to completely burn all the sulfur. We start by calculating the number of moles of sulfur present in 640 grams:

Moles of S 640 g / (32 g/mol) 20 mol

From the balanced chemical equation, we know that 1 mole of sulfur reacts with 1 mole of oxygen. Therefore, to completely burn 20 moles of sulfur, we need 20 moles of oxygen. This can be expressed in the following steps:

Moles of O? Moles of S 20 mol

Hence, 20 moles of oxygen are required to completely burn 640 grams of sulfur.

Implications of the Reactant Stoichiometry in Chemical Reactions

The result of this calculation highlights the importance of understanding the reactant stoichiometry in chemical reactions. It demonstrates how the balanced chemical equation directly translates into the required quantities of reactants, making it a practical tool in both theoretical and real-world applications. For chemists and engineers, this knowledge is crucial for designing reactions, calculating yields, and ensuring the efficient use of resources.

Conclusion

In conclusion, the complete combustion of 640 grams of sulfur requires 20 moles of oxygen. This process is governed by the balanced chemical equation, where the stoichiometry of sulfur to oxygen is 1:1. Understanding these principles not only aids in solving specific problems but also deepens the understanding of chemical reactions and their practical applications.

Keywords

oxygen combustion, sulfur reaction, stoichiometry, molar mass, balanced chemical equation