Final answer:
To calculate the volume of CO₂ formed and unused O₂ in the given reaction, we use the stoichiometric ratio and molar volume. The volume of CO₂ formed is approximately 1.14 liters, and the unused O₂ is approximately 2 liters.
Step-by-step explanation:
The given chemical equation is:
2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O
From the equation, we can see that 2 moles of C₂H₆ reacts with 7 moles of O₂ to produce 4 moles of CO₂ and 6 moles of H₂O.
To calculate the volume of O₂ burned, we can use the concept of molar volume. At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, to find the volume of O₂, we need to calculate the number of moles of O₂ used and then multiply it by the molar volume.
Given that 2000 cc of O₂ was burnt, we can convert it to liters by dividing by 1000: 2000 cc ÷ 1000 = 2 liters.
So, the number of moles of O₂ used can be calculated as follows:
Moless of O₂ = Volume of O₂ (in liters) / Molar Volume
Moless of O₂ = 2 L / 22.4 L/mol = 0.089 mol
Since the stoichiometric ratio between O₂ and CO₂ is 7:4, we can use this to find the moles of CO₂ produced:
Moless of CO₂ = Moless of O₂ × (Moles of CO₂ / Moles of O₂)
Moless of CO₂ = 0.089 mol × (4 mol CO₂ / 7 mol O₂) = 0.051 mol
To convert the moles of CO₂ to volume, we can use the molar volume:
Volume of CO₂ = Moless of CO₂ × Molar Volume
Volume of CO₂ = 0.051 mol × 22.4 L/mol = 1.14 liters
Therefore, the volume of CO₂ formed is approximately 1.14 liters and the unused O₂ is approximately 2 liters.