A 26 L flask at 273 K and 17 Torr contains nitrogen . What mass of the nitrogen is present? Answerand units of g.
To calculate the mass of nitrogen present in the flask, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in atmospheres (Torrs can be converted to atm by dividing by 760)
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin
First, let's convert the pressure from Torr to atm:
17 Torr / 760 Torr/atm = 0.02237 atm
Now let's rearrange the ideal gas law equation to solve for the number of moles:
n = PV / RT
Plug the values into the equation:
n = (0.02237 atm) * (26 L) / (0.0821 L·atm/mol·K * 273 K)
Perform the calculations:
n = 0.2217 mol
Now, to calculate the mass of nitrogen, we need to know its molar mass. The molar mass of nitrogen (N₂) is approximately 28 g/mol.
Finally, we can use the number of moles and the molar mass to calculate the mass of nitrogen:
Mass = n * Molar Mass
Mass = 0.2217 mol * 28 g/mol
Perform the calculations:
Mass = 6.2046 g
Therefore, the mass of nitrogen present in the flask is approximately 6.2046 grams.
PV = nRT and solve for n = number of mols.
Then n = grams/molar mass. You know molar mass and n, solve for grams.