Final answer:
To find the mass of fluorine gas produced from 0.67 L of HF at STP, use the given reaction stoichiometry and the volume of gas at STP to calculate moles and then convert to mass using the molar mass of fluorine.
Step-by-step explanation:
To calculate the mass of fluorine gas (F2) produced from 0.67 L of hydrogen fluoride (HF) at Standard Temperature and Pressure (STP), we will use the reaction:
4HF + O2 → 2F2 + 2H2O.
At STP, 1 mole of gas occupies 22.414 L. So the number of moles of HF in 0.67 L can be calculated by the formula:
Moles of HF = Volume of HF / Volume of 1 mole at STP = 0.67 L / 22.414 L/mol
Then, from the reaction stoichiometry, the moles of F2 produced is half the moles of HF since 4 moles of HF produce 2 moles of F2.
Moles of F2 = Moles of HF / 2
To find the mass of F2, we multiply the moles of F2 by its molar mass (approximately 38.00 g/mol):
Mass of F2 = Moles of F2 × Molar Mass of F2
Following the calculations, the answer will be the mass of fluorine gas produced from the reaction.