The density of chlorine gas at 0.970 atm and 54.1 °C is ________ g/L.
To find the density of chlorine gas at these conditions, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (0.970 atm)
V = volume (unknown, since we are calculating density in g/L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature in Kelvin (54.1 + 273 = 327.1 K)
First, we need to calculate the number of moles using the ideal gas law:
n = (PV) / (RT)
n = (0.970 atm) / (0.0821 L.atm/mol.K * 327.1 K)
n ≈ 0.0328 moles
Next, we need to calculate the mass of chlorine gas using the molar mass of chlorine gas (Cl₂ = 70.91 g/mol):
mass = n * molar mass
mass = 0.0328 moles * 70.91 g/mol
mass ≈ 2.33 g
Finally, we can calculate the density of chlorine gas at these conditions:
density = mass / volume
density = 2.33 g / V
Since we don't know the volume (V), we won't be able to provide the exact density without this information.