Final answer:
To determine the mass of oxygen gas consumed in the reaction with 5.52 g of ethanol, we use the balanced chemical equation and molar masses to find that 3.84 g of oxygen gas is consumed.
Step-by-step explanation:
To calculate the mass of oxygen gas consumed by the reaction of 5.52 g of ethanol, we first need to write down the balanced chemical equation for the reaction:
C₂H₅OH + O₂ → CH₃COOH + H₂O
However, this equation is not balanced. The balanced equation is:
C₂H₅OH + O₂ → 2CH₃COOH + 2H₂O
Next, we will calculate the moles of ethanol (C₂H₅OH) using its molar mass:
Molar mass of C₂H₅OH = 46.07 g/mol
Moles of ethanol = mass / molar mass = 5.52 g / 46.07 g/mol = 0.12 moles
According to the balanced equation, 1 mole of ethanol reacts with 1 mole of oxygen gas. Therefore, 0.12 moles of ethanol will react with 0.12 moles of oxygen. Now, we will calculate the mass of oxygen gas using its molar mass:
Molar mass of O₂ = 32.00 g/mol
The mass of oxygen gas used = moles of oxygen * molar mass = 0.12 moles * 32.00 g/mol = 3.84 g
The mass of oxygen gas consumed by the reaction of 5.52 g of ethanol is therefore 3.84 g.