A solution prepared by dissolving a 2.50 g sample of an unknown compound dissolved in `34.0` g on benzene , `C_(6)H_(6)` , boils `1.38^(@) C ` higher than pure benzene . Which expression gives the molar mass of the unknown compound ?

A solution prepared by dissolving a 2.50g sample of a unknown compound dissolved in 34.0g of benzene C_(6)H_(6) boils at 1.38^(@)C higher than pure benzene. Which expression gives the molar mass of the unknown compound? {:("Compound",K_(b)),(C_(6)H_(6),2.53^(@)Cm^(-1)):}

A solution prepared by dissolving a 2.50g sample of a unknown compound dissolved in 34.0g of benzene C_(6)H_(6) boils at 1.38^(@)C higher than pure benzene. Which expression gives the molar mass of the unknown compound? {:("Compound",K_(b)),(C_(6)H_(6),2.53^(@)Cm^(-1)):}

A solution prepared by dissolving 1.25 g of oil of winter green (methyl s.ilicylate) in 99.0 g of benzene has a boiling po . int of 80.31^(@) C , Determine the molar mass of this compound. (B.P. of pure benzene = 80.10^(@) C and K_(b) for benzene = 2.53^(@) C " Kg " mol^(-1) )

1.02 g of urea when dissolved in 98.5 g of certain solvent decreases its freezing point by 0.211 K . 1.60 g of unknown compound when dissolved in 86.0 g of the same solvent depresses the freezing point by 0.34 K . Calculate the molar mass of the unknown compound (Molar mass of urea = 60 g mol^(-1) ).

A solution prepared by dissolving 1.25g of oil of winter green (methyl sallicylate) in 99.0g of benzene has a boiling point of 80.31^(@)C . Determine the molar mass of this compound. ( B.P. of pure benzene =80.10^(@)C and K_(b) for benzene =2.53^(@)C kg "mol".1 )

A solution prepared by dissolving 1.25g of oil of winter green (methyl sallicylate) in 99.0g of benzene has a boiling point of 80.31^(@)C . Determine the molar mass of this compound. ( B.P. of pure benzene =80.10^(@)C and K_(b) for benzene =2.53^(@)C kg "mol".1 )

1.02 g of urea when dissolved in 98.5 g of certain solvent decreases its freezing point by 0.211K. 1.609 g of unknown compound when dissolved in 86 g of the same solvent depresses the freezing point by 0.34 K. Calculate the molar mass of the unknown compound.(molar mass of urea = 60 g/mol )