Calculating Oxygen Volume for the Combustion of Carbon Disulfide

Understanding the chemistry behind the combustion of carbon disulfide (CS2) is crucial for various applications, including industrial processes. This article explains how to calculate the volume of oxygen required for the complete combustion of 1.5 moles of carbon disulfide. We will cover the necessary steps, the chemical equation, and the application of molar ratios to determine the required oxygen volume.

Chemical Equation for Combustion

The first step in determining the volume of oxygen needed is to write the balanced chemical equation for the combustion of carbon disulfide. The combustion of CS2 produces carbon dioxide (CO2) and sulfur dioxide (SO2).

CS2 O2 → CO2 SO2

To balance this equation, we need to ensure that the number of atoms of each element on both sides of the equation is equal. The balanced equation is:

2 CS2 5 O2 → 4 CO2 4 SO2

Understanding the Molar Ratios

The balanced equation indicates the molar ratio of CS2 to O2. From the equation, we can see that 2 moles of CS2 react with 5 moles of O2. This ratio can be used to find out the moles of O2 required for 1.5 moles of CS2.

Step 1: Determine the Moles of O2 Required

Using the molar ratio, we can set up the following proportion:

2 moles CS2 : 5 moles O2 1.5 moles CS2 : x moles O2

Solving for x, we get:

x (1.5 moles CS2) × (5 moles O2) / (2 moles CS2) 3.75 moles O2

Step 2: Convert Moles of O2 to Volume

The volume of a gas at standard room temperature and pressure (STP) is proportional to the number of moles of the gas. At STP, 1 mole of any gas occupies 24 dm3 of volume. Therefore, to find the volume of 3.75 moles of O2, we multiply the moles by 24 dm3 per mole:

Volume of O2 (3.75 moles) × (24 dm3/mole) 90 dm3

Conclusion

Therefore, the volume of oxygen required to burn 1.5 moles of carbon disulfide (CS2) is 90 dm3 at standard room temperature and pressure.

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