Question

how do i find delta T of benzoic acid? as well as delta T of unknown and the experimental molar mass of unknown??

Pure solvent Mass of Lauric acid TFP (pure solvent) (Trial 1) (Typ freezing point temperature from graph) 8.03g 1200 42.00 42.00 42.6°C TFP (pure solvent) (Trial 2) Average TFP (pure solvent) Unknown code Benzoic acid (2 pts.) Mass of benzoic acid TFP (solution) (Trial 1) TFP (solution) (Trial 2) 1.05g (2 pes 360.04C 38.00 366.6C_(2 pts.) Mass of Lauric acid Mass of unknown TFP (solution) (Trial 1) TFP (solution) (Trial 2) ORT_12 pes) 8.034_(2 pts.) 1.069 12 pes) 36.0°C 36.00 36.0°C 12 pes) Average TFP (solution) Average TFP (solution) ATbenzoic acid AT unknown Experimental Molar Mass of benzoic acid 122129100ks pos) Experimental Molar Mass of unknown (3 pts.)

also what would the equation be?

Answer 1

Date DAT benzoic CIBA Tre (Golvent - TFP (BA) acid = 42°C -38°C 2 4°C = Trp coolvent) - Trp (solution) I unknown 42 °C - 36°C Вибут kg of lauric and - 3.9°C. kglmal At = mokf > m=AL Kf Where, m = molality 6c 3,9% Kglmol 1.538 mollkg - m= no.oh moles wgt. of solvent (kg) 1.538 mollkg & no. of moles

Uaail) Date / no. of moles a 0.002 mol We know, no. of moles - mass of unknown Molecular wogt of unitine = 0.012 ma 1606g ць! - ugt => Mol. wat = 1.069 ooola mol = 88.33 glmol. i. Malembt Holecular weight of unknown = 88.33 gimola