Calculate the density of sulfur hexafluoride gas at 800 torr and 35
density=mass/volume=( moles/molmass )/volume
moles/volume from PV=nRT n/v=P/RT
density= P/RTV
From PV = nRT = (mass/f.wt)RT => (mass/Volume) = P(f.wt.)/RT = Density
P = 800 Torr = 1.053 Atm (must convert Torr to Atm b/c R-value units = L∙Atm/mole∙K)
f.wt = S + 6F = [32 + 6(19)] g/mol = 146 g/mol
R = 0.08206 L∙Atm/mole∙K
T = 35ᵒC + 273 = 308 K
D = (1.053-Atm)(146 g/mol)/(0.08206 L∙Atm/mole∙K)(308 K) = 6.08 g/L
To calculate the density of a gas, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant
T = temperature of the gas in Kelvin
First, we need to convert the given values into the correct units:
800 torr = 800/760 atm (since 1 atm = 760 torr)
35°C = 35 + 273.15 = 308.15 K
Next, we need to determine the molar mass of sulfur hexafluoride (SF6). The molar mass of sulfur (S) is 32.06 g/mol, and the molar mass of fluorine (F) is 18.998 g/mol. Since there are six fluorine atoms in one SF6 molecule, the molar mass of SF6 is:
6(18.998 g/mol) + 32.06 g/mol = 146.06 g/mol
Now we can calculate the density. Rearranging the ideal gas law equation, we have:
n = PV / (RT)
Since we want to calculate the density, which is mass per unit volume, we can substitute the molar mass (M) of SF6:
density = (PM) / (RT)
Substituting the values into the equation, we get:
density = ((800/760) atm) * (146.06 g/mol) / ((0.0821 L * atm/(mol * K)) * 308.15 K)
Simplifying the equation gives the density of sulfur hexafluoride gas at the given conditions.