Calculating the Mass of Carbon Dioxide Produced from Propane Combustion
How can we calculate the mass of carbon dioxide produced from the complete combustion of propane?
Given data: The density of liquid propane in the tank is 0.621 g/mL
Answer:
To calculate the mass of carbon dioxide produced from the complete combustion of propane, we can utilize stoichiometry, the ideal gas law, and the given density of the liquid propane in the tank. This involves converting the given volume of propane into its mass and then determining the moles of propane to find the mass of carbon dioxide produced.
When calculating the mass of carbon dioxide generated from the complete combustion of propane, it is essential to follow a systematic approach. First, we need to consider the balanced chemical equation for the combustion of propane, which reveals the stoichiometric ratio between propane and carbon dioxide.
In this case, the balanced equation is: C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
From the balanced equation, we can see that 1 mole of propane (C₃H₈) produces 3 moles of carbon dioxide (CO₂). This information is crucial for determining the amount of carbon dioxide generated.
Given that the density of liquid propane in the tank is 0.621 g/mL, we can convert the provided volume of propane to its mass using the density formula: density = mass/volume. By rearranging the formula, we can find the mass of propane in grams.
Once we have the mass of propane, we can then convert it to moles by using the molar mass of propane (44.1 g/mol). This step is necessary for applying the stoichiometric ratio to determine the moles of carbon dioxide produced.
The molar mass of carbon dioxide (CO₂) is approximately 44.01 g/mol. By using the 3:1 stoichiometric ratio from the balanced equation, we can calculate the moles of carbon dioxide generated from the combustion of propane.
Finally, to obtain the mass of carbon dioxide in kilograms, we convert the moles of carbon dioxide to grams and then to kilograms. This comprehensive approach allows us to accurately determine the mass of carbon dioxide produced from the combustion of a given volume of propane.
Understanding the principles of stoichiometry, gas laws, and chemical reactions is crucial in solving complex chemistry problems related to reactants and products. By applying these concepts, we can analyze the relationships between substances in a chemical reaction and make precise calculations based on the given data.