Pure water freezes at 273 K and 1 bar. The addition of 34.5 g of ethanol to 500 g of water changes the freezing point of the solution. Use the freezing point depression constant of water as 2 K kg mol^(-1).The figures shown below represent plots of vapour pressure (V.P.) versus temperature (T). [molecular weight of ethanol is 46 g mol^(-1) Among the following, the option representing change in the freezing point is

Pure water freezes at 273 K and 1 bar. The addition of 34.5 g of ethan

1.	Pure water freezes at 273 K and 1 bar. The addition of 34.5 g of ethanol to 500 g of water changes the freezing point of the solution. Use the freezing point depression constant of water as 2 K kg mol^(-1).The figures shown below represent plots of vapour pressure (V.P.) versus temperature (T). [molecular weight of ethanol is 46 g mol^(-1) Among the following, the option representing change in the freezing point is
Answer» Solution :MOLE of `C_(2)H_(5)OH=34.5/46` `m=34.5/46xx1000/500` `DeltaT_(f)=34.5/46xx1000/500xx2=3` `T_(f)^(@)-T_(f)=273-T_(f)=3` `T_(f)=273-3=270K`