Home
Class 12
CHEMISTRY
A solution containing 0.1 mole of naphth...

A solution containing `0.1` mole of naphthalene and `0.9` mole of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed upto `353K` where its vapour pressure was found to be `670` torr. The freezing point and and boiling point of benzene are `278.5K` and `353K` respectively and its enthalpy of fusion is `10.67 Lk "mol"^(-1)`. Calculate the temperature to which the solution was cooled originally and the amount of benzene that must have frozen out. Assume ideal behavious.

Text Solution

Verified by Experts

The correct Answer is:
`8.11 K`
Thus, original solution must have ben cooled to `278.5-8.11=270.39K`
Promotional Banner

Topper's Solved these Questions

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) level-I|55 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) level-II|30 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SUBJECTIVE) level-I (NUMERICAL BASED PROBLEMS)|8 Videos

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise SINGLE INTEGER ANSWER QUESTIONS|4 Videos

  • NUCLEIC ACID AND VITAMIN

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE)|15 Videos

Similar Questions

Explore conceptually related problems

A solution containing 0.1 mol of naphthalene and 0.9 mol of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed upto 353 K where its vapour pressure was found to be 670 mm . The freezing point and boiling point of benzene are 278.5 K and 353 K respectively, and its enthalpy of fusion is 10.67 KJ "mol"^(-1) . Calculate the temperature to which the solution was cooled originally and the amount of benzene that must have frozen out. Assume ideal behaviour.

What is the freezing of 0.4 molal solution of acetic acid in benzene in which it dimerises to the extent of Freezing point of benzene is 278.K and its molar heat of fusion is 10-042KJ mol^(-1)

The freezing point of 0.02 mole fraction acetic acid in benzene is 277.4 K . Acetic acid exists partly as dimer. Calculate the equilibrium constant for dimerization. The freezing point of benzene is 278.4 K and the heat the fusion of benzene is 10.042 kJ mol^(-1) . Assume molarity and molality same.

The vapour pressure of pure benzene and toluene at 40^(@)C are 184.0 torr and 59.0 torr, respectively. Calculate the partial presure of benzene and toluene, the total vapour pressure of the solution and the mole fraction of benzene in the vapour above the solution that has 0.40 mole fraction of benzene. Assume that the solution is ideal.

The freezing point depression constant of benzene is 5.12 K kg mol^(-1) . The freezing point depression for the solution of molality 0.078m containing a non-electrolyte solute in benzene is