Determining the Minimum Mass of Oxygen for Butane Combustion

In this article, we will explore the process of determining the minimum mass of oxygen required for the complete combustion of 100 kg of butane (C4H10). This is a fundamental concept in chemical engineering and combustion science, with practical applications in various industries, including fuel technology, energy production, and environmental management.

Step-by-Step Guide: Calculating the Oxygen Requirement

The first step in this process is to write a balanced chemical equation for the combustion of butane:

2 C4H10 13 O2 → 8 CO2 10 H2O

This equation represents the complete combustion of butane, where two molecules of butane react with 13 molecules of oxygen to produce eight molecules of carbon dioxide and ten molecules of water.

Calculating the Molar Mass of Butane

Next, we need to determine the molar mass of butane (C4H10). Given:

Molar mass of Carbon (C) 12.01 g/mol Molar mass of Hydrogen (H) 1.008 g/mol Molar mass of Butane (C4H10) 4 × 12.01 10 × 1.008 48.04 10.08 58.12 g/mol

Converting Butane Mass to Moles

Now we will convert the mass of butane to moles:

Moles of butane (mass of butane) / (molar mass)

100,000 g / 58.12 g/mol 1716.3 moles

Using Stoichiometry to Determine the Oxygen Requirement

From the balanced equation, we know that 2 moles of butane react with 13 moles of oxygen:

13 moles O2 / 2 moles C4H10 6.5 moles O2 per mole of C4H10

Therefore, for 1716.3 moles of butane:

Moles of O2 1716.3 moles × 6.5 11164.0 moles

Converting Moles of Oxygen to Mass

The molar mass of oxygen (O2) is 2 × 16.00 g/mol 32.00 g/mol. Thus:

Mass of O2 (moles of O2) × (molar mass of O2) 11164.0 moles × 32.00 g/mol 356,000 g 356 kg

Conclusion

The minimum mass of oxygen needed for the complete combustion of 100 kg of butane is approximately 356 kg. This shows how stoichiometry and chemical equations play a crucial role in understanding the exact requirements for chemical reactions, particularly in contexts involving combustion processes.

Further Exploration

To further your understanding of this topic, you can explore more detailed calculations and applications of chemical reactions, such as thermodynamic analysis and the environmental implications of butane combustion. Additionally, studying the stoichiometry of other hydrocarbons can provide a broader perspective on fuel combustion and energy production processes.