Final answer:
The number of moles of fluorine gas in the given conditions is approximately 0.183 moles, not matching any of the provided options. The number of fluorine atoms would be double that amount, approximately 0.366 moles, as each molecule of F2 contains two atoms.
Step-by-step explanation:
The number of moles of fluorine gas contained in a 3.01 L vessel at 27°C with a pressure of 1.50 atm can be calculated using the ideal gas law PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(K·mol)), and T is the temperature in kelvins.
To find the number of moles (n), rearrange the ideal gas equation: n = PV / RT. Convert the temperature to kelvins by adding 273.15 to the Celsius temperature: T = 27 + 273.15 = 300.15 K. Now plug the values into the equation:
n = (1.50 atm × 3.01 L) / (0.0821 L·atm/(K·mol) × 300.15 K) which yields approximately 0.183 moles, an answer not listed in the options provided.
If we calculate the number of fluorine atoms in the sample, it will be twice the number of moles of the F2 molecule because each molecule contains two fluorine atoms: 0.183 moles × 2 = 0.366 moles of fluorine atoms.