Posted by Dave on .
In a solution with carbon tetrachloride as the solvent, the compound VCl4 undergoes dimerization:
2VCl4 <-> V2Cl8
When 6.6834 g VCl4 is dissolved in 100.0 g of carbon tetrachloride, the freezing point is lowered by 5.97*C/ Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm^3. and Kf = 29.8*C kg/mol for CCl4.)
It's an "integrative problem", and I'm unsure as to where to start... /:
Chemistry - Chemical Equilibrium -