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» 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: