Final answer:
To find the mass of a sample of fluorine gas at STP, we use the ideal gas law equation PV = nRT. Given a volume of 12.7 L, we can calculate the number of moles using the ideal gas law equation n = PV / RT. The molar mass of fluorine gas is 38.00 g/mol, so the mass of the sample is approximately 21.7 g.
Step-by-step explanation:
To find the mass of a sample of fluorine gas at STP, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. At STP, the pressure is 1 atm and the temperature is 273 K. We can rearrange the equation to solve for the mass, m = n × M, where m is the mass, n is the number of moles, and M is the molar mass of fluorine gas. The molar mass of fluorine gas (F2) is 38.00 g/mol.
Given the volume of 12.7 L, we can calculate the number of moles using the ideal gas law equation: n = PV / RT. Plugging in the values, we have n = (1 atm) × (12.7 L) / (0.0821 L.atm/K.mol) × (273 K). Solving for n gives us approximately 0.571 moles.
Finally, we can calculate the mass using the equation m = n × M. Plugging in the values, we have m = (0.571 mol) × (38.00 g/mol) = 21.7 g.