Chemical Reaction Stoichiometry: Finding the Grams of CO2 Produced

How many grams of CO2 is produced when excess CS2 reacts with 4 mols of O2? The mass of CO2 produced when excess CS2 reacts with 4 mols of O2 can be calculated using stoichiometry principles. Let's break down the process step by step. Given reaction: CS2 + 3O2 -> CO2 + 2SO2 Molar ratio of CO2 to O2 is 1:3 based on the balanced chemical equation. This means for every 1 mol of CO2 produced, 3 mols of O2 are consumed. Since O2 is the limiting reactant in this case, we will use it to determine the amount of CO2 produced. First, calculate the amount of CO2 in mols that will be produced by 4 mols of O2: Mols of CO2 = (4 mols O2) x (1 mol CO2 / 3 mols O2) = 4/3 mols CO2 Next, convert mols of CO2 to grams using the molar mass of CO2 (44 g/mol): Mass of CO2 = (4/3 mols CO2) x (44 g/mol) = 58.67 grams Therefore, when excess CS2 reacts with 4 mols of O2, 58.67 grams of CO2 will be produced.

Stoichiometry is a branch of chemistry that deals with the calculation of quantitative relationships in chemical reactions. It allows us to determine the amount of products formed in a chemical reaction based on the amount of reactants consumed.

Steps to Solve the Problem:

1. Write down the balanced chemical equation for the reaction. In this case, the reaction is between CS2 and O2 producing CO2 and SO2.

2. Identify the limiting reactant, which is the reactant that will be completely consumed first and determines the amount of product formed.

3. Use the molar ratio from the balanced equation to relate the amount of the limiting reactant to the amount of product formed.

4. Calculate the amount of product formed in mols and then convert it to grams if necessary using the molar mass of the product.

Key Concepts:

- Molar ratio: The ratio of mols of one substance to another in a balanced chemical equation.

- Limiting reactant: The reactant that limits the amount of product formed in a chemical reaction.

- Molar mass: The mass of one mole of a substance, expressed in grams per mole.

By following these steps and understanding these key concepts, you can solve stoichiometry problems like the one presented here and determine the amount of product formed in a chemical reaction.
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