An aqueous solution of urea has a freezing point of `-0.515^(@)C`. Predict the osmotic pressure (in atm) of the same solution at `37^(@)C`.

An aqueous solution of urea has freezing point of -0.604^(@)C & At 27^(@)C . The osmatic pressure of the same solution is ____________atm . (assume molality and molarity are same)

An aqueous solution of urea has a freezing point of -0.52^(@)C . Assuming molarity same for the solution, the osmotic pressure of solution at 37^(@)C would be : (K_(f) of H_(2)O=1.86 K molarity .^(-1) )

Calculate osmotic pressure of 0.1M urea aqueous solution at 300K .

Calculate osmotic pressure of 0.1M urea aqueous solution at 300K .

An aqueous solution of urea has freezing point of -0.52^(@)C . If molarity and molality are same and K'_(f) for H_(2)O = 1.86 K "molality"^(-1) the osmotic pressure of solution would be:

The depression in feezing point is 0.93^(@)C then the osmotic pressure of aqueous solution of the given non-electrolyte at 27^(@)C is