The molal freezing point depression constant of benzene is 5.07 K kg/mol. A .45% solution of monoclinic sulfur in benzene freezes .088K below the freezing point of pure benzene. Find the molecular formula of sulfur in benzene. Can someone tell me if the answer is S2 ? I guess I'm not 100% sure about what exactly I'm looking for. What I did was say that if there was 100g of solution, then 100g *(.45)*(1/32.1)=1.402 moles of sulfur 100g *(.55)*(1/78.1)=0.704 moles of benzene then divided them which gave about 2 moles of sulfur per benzene. But 1) I never used the molality from the freezing point depression which makes me think I'm definitely wrong and 2) I'm just not sure if it makes sense to find moles of sulfur per moles of benzene. any insight? This was on my quiz today and I won't rest until I know how wrong I was! lol.