At `300 K`, the vapour pressure of an ideal solution containing one mole of `A` and `3` mole of `B` is `550 mm` of `Hg`. At the same temperature, if one mole of `B` is added to this solution, the vapour pressure of solution increases by `10 mm` of `Hg`. Calculate the `V.P.` of `A` and `B` in their pure state.

At `300 K`, the vapour pressure of an ideal solution containing one mo

1.	At `300 K`, the vapour pressure of an ideal solution containing one mole of `A` and `3` mole of `B` is `550 mm` of `Hg`. At the same temperature, if one mole of `B` is added to this solution, the vapour pressure of solution increases by `10 mm` of `Hg`. Calculate the `V.P.` of `A` and `B` in their pure state.
Answer» Correct Answer - `V.P.` of `A = 400 mm`, `V.P.` of `B = 600 mm`;

Discussion

No Comment Found

Related InterviewSolutions

1000 g of 1 molal aqueous solution of sucrose is cooled and maintained at `-3.534^(@)C`. Find out how much ice will separate out at this temperature. `(K_(f)` for water `=1.86 k m^(-1)`)
Art what temperature `(s)` a `5%` solution `(w//V)` of glucose will develop an osmotic pressure of `7 atm`?A. `273 K`B. `306.94 K`C. `33.94^(@)C`D. `33.94 K`
What will be the osmotic pressure of `0.1 M` monobasic acid its `pH` is `2` at `25^(@)C`?
Chloroacetic acid has `K_(a) = 1.36 xx 10^(-3)`. Calculate the concentration of each ion and freezing point of `0.1 M` its solution, assuming molarity and malality same. `(K_(f) "for"H_(2)O = 1.86 K "molality"^(-1))`
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 ratio by weight of `NaF` and `NaI` which when dissolved in water produces the same osmotic effects as `0.1` molar solution of urea in water at same temperature? The weight of residue obtained on evaporation of the salt solution is `0.48` gram per `100mL` of solution evaporated. Assume complete dissociation of the salts.
Among `0.1 M` solution of `NH_(2)CONH_(2), Na_(2)PO_(4)` and `Al_(2)(SO_(4))_(3)`:A. The `V.P.` and freezing point are the highest for urea.B. The elevation in boiling point is the highest for `Al_(2)(SO_(4))_(3)`C. The `V.P.` and freezing point is the lowest for ureaD. The depression in freezing point in the highest for the `Al_(2)(SO_(4))_(3)`
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.
Vapour pressure of `C_(6)H_(6)` and `C_(7)H_(8)` mixture at `50^(circ)C` are given by `P=179X_(B)+92`, where `X_(B)` is mole fraction of `C_(6)H_(6)`. Calculate (in `mm`): (a) Vapour pressure of pure liquids. (b) Vapour pressure of liquid mixture obtained by mixing `936g C_(6)H_(6)` and `736g` toluene. ( c) If the vapours are removed and condensed into liquid and again brought to the temperature of `50^(circ)C`, what would be mole fraction of `C_(6)H_(6)` in vapour state ?
An aqueous solution of an acid is so weak that it can be assumed to be practically unionised, boiled at `100.4^(circ)C`. `25 mL` of this solution was neutralised by `38.5 mL` of `1N` solution of `NaOH`. Calculate basicity of the acid if `K_(b)` for water is `0.52 K mol^(-1) kg`. Assume molality equal to molarity.

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment