`0.75 g` of a non-electrolyte was dissolved in `87.9 g` of benzene. This raised the boiling point of benzene by `0.25^(@)C`. If the molecular mass of non-electrolyte is `103`, calculate the molal elevation constant for bezene.

0.90g of a non-electolyte was dissolved in 87.9 g of benzene. This reised the boiling point of benzene by 0.25^(@)C . If the molecular mass of the non-electrolyte is 103.0 g mol^(-1) , calculate the molal elecation constant for benzene.

0.90g of a non-electrolyte was dissolved in 90 g of benzene. This raised the boiling point of benzene by 0.25^(@)C . If the molecular mass of the non-electrolyte is 100.0 g mol^(-1) , calculate the molar elevation constant for benzene.

0.90g of a non-electrolyte was dissolved in 90 g of benzene. This raised the boiling point of benzene by 0.25^(@)C . If the molecular mass of the non-electrolyte is 100.0 g mol^(-1) , calculate the molar elevation constant for benzene.

2g of a non-electrolyte solute dissolved in 100g of benzene lowered the freezing point of benzene by 0.40 K. find the molar mass of the solute.

If 10.0 g of a non-electrolyte dissolved in 100 g of water lowers the freezing point of water by 1.86^(@)C , the molar mass of the non-electrolyte is ( K_(f)=1.86 Km^(-1) )

1.0 g of non - electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.4 K. Find the molar mass of the solute. [Given : Freezing point depression constant of benzene = 5.12 K. kg mol].