Volume (V) = 329.5 cm3 = 0.3295 Liters
Pressure (P) = 1 atm
Temperature (T) = 20 oC = 293.15 K
Gas constant (R) = 0.0821 L atm mol-1 K-1
PV = nRT
No. of moles (n) = PV / RT = (1 atm x 0.3295 L) / (0.0821 L atm mol-1 K-1 x 293.15 K) = 0.0137 mol
Moles = weight / molar mass
molar mass = weight / moles = (2 g) / (0.0137 mol) = 146 g/mol
Given compound is: SX6
(32 g/mol) + (6 x molar mass of X) = 146 g/mol
molar mass of X = (114 / 6) = 19 g/mol
molar mass having 19 g/mol = Fluorine
So;
the compound is: SF6
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