Chemical Reaction Limiting Reagent Calculation

When it comes to chemical reactions, it is crucial to determine the limiting reagent. In the case of the reaction between carbon disulfide (CS2) and oxygen (O2) to form carbon dioxide (CO2) and sulfur (S), it is important to identify which reactant will be completely consumed first, thus limiting the amount of product formed.

Given that 100 grams of CS2 reacts with 38 grams of O2, we first need to convert these masses into moles to determine the limiting reagent. Using the molar masses of CS2 (76.15 g/mol) and O2 (32 g/mol), we find that there are 1.3132 moles of CS2 and 1.1875 moles of O2.

The balanced chemical reaction shows that the mole ratio of CS2 to O2 is 1:1. Since there are more moles of CS2 (1.3132 moles) than O2 (1.1875 moles), it means that O2 will be completely consumed first, making it the limiting reagent in this reaction.

By understanding the concept of limiting reagents in chemical reactions, we can predict the amount of product that can be formed and optimize the reaction conditions for better efficiency. Identifying the limiting reagent allows us to control the reaction and maximize the yield of the desired products.