You have a 1 L container of F2 at 20 degrees C and 1 atm. Subtract the weight of the container , what is the mass of the gas
You can use PV = nRT
Plug in 1 atm and 1 L and 298 for T, calculate n, then n = g/molar mass to calculate grams.
To find the mass of the gas, we need to know the density of F2 at the given temperature and pressure.
1. Start by finding the molar mass of F2. The molar mass of F2 is the sum of the atomic masses of fluorine (F), which is approximately 19.0 g/mol.
2. Next, 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.
3. Convert the given temperature from degrees Celsius to Kelvin by adding 273.15: 20 degrees C + 273.15 = 293.15 K.
4. Convert the given pressure from atm to Pascal using the conversion factor: 1 atm = 101325 Pa.
5. Rearrange the ideal gas law equation to solve for n (number of moles): n = PV / RT.
6. Plug in the values into the equation: n = (1 atm * 101325 Pa/atm) * (1 L) / (0.0821 L * atm / mol * K * 293.15 K).
7. Calculate n to find the number of moles of F2.
8. Finally, multiply the number of moles by the molar mass of F2 to get the mass of the gas: mass = n * molar mass of F2.
By following these steps, you can determine the mass of the gas in a 1 L container of F2 at 20 degrees C and 1 atm pressure.