The normal boiling point of diethyl ether is 34.5 C. A solution containing a nonvolatile solute...

The normal boiling point of diethyl ether is 34.5 C. A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698 torr at 34.5 C. What is the mole fraction of diethyl ether in this solution?

Solutions

Expert Solution

Total pressure of the system will be room temperature pressure which is 760 mmHg

Since normal boiling point of ether is 34.5 oC. the vapour pressure of diethyl ether must equal to that of the total pressure.

Hence Vapour pressure of diethyl ether = 760 mmHg

Since a non-volatile solute is now added .the vapour pressure of ether has went down

Vapour pressure of ether after addition of non volatile solute

We will apply roults law

YiP_t=P = Xi Psat

where P is partial pressure of the solution

Xi is the mole fraction in liquid state

Psat is the vapour pressure of the pure solvent.

In our case P = 698 Torr, Psat = 760 Torr

substituting this in the above equation,

698 = Xi*760

Xi =0.9184

Hence, mole fraction of diethyl in this solution is 0.9184

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

1. The boiling point of diethyl ether CH3CH2OCH2CH3 is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte...

1. The boiling point of diethyl ether CH3CH2OCH2CH3 is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is cholesterol . How many grams of cholesterol, C27H46O (386.6 g/mol), must be dissolved in 247.0 grams of diethyl ether to raise the boiling point by 0.450 °C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene...

Estimate the heat of vaporization of diethyl ether at its normal boiling point using Trouton’s rule...

Estimate the heat of vaporization of diethyl ether at its normal boiling point using Trouton’s rule and Chen’s rule and compare the results with a tabulated value of this quantity. Calculate the percentage error that results from using each estimation. Then estimate ΔH^v at 100°C using Watson’s correlation.

Diethyl ether (C4H10O) has a vapor pressure of 379.6 torr at 20.0 °C. If diethyl ether...

Diethyl ether (C4H10O) has a vapor pressure of 379.6 torr at 20.0 °C. If diethyl ether is place in a 10.0 L container at atmospheric pressure and sealed once equilibrium has been established, what will the mass percent of diethyl ether in the gas-phase be (assume air has an average molecular mass of 28.97 g/mol and diethyl ether liquid has a negligible volume).

How is a solution freezing point and boiling point affected by addition of a dissolved solute?

Calculate the freezing point and boiling point in each solution,assuming complete dissociation of the solute....

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. A. Calculate the freezing point of a solution containing 10.7 g FeCl3 in 164 g water. B. Calculate the boiling point of the solution above C. Calculate the freezing point of a solution containing 3.7 % KCl by mass (in water). D. Calculate the boiling point of the solution above.

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute....

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. 1) Calculate the freezing point of a solution containing 10.6 g FeCl3 in 151 g water. 2) Calculate the boiling point of a solution above. 3) Calculate the freezing point of a solution containing 6.2% KCl by mass (in water). Express your answer using two significant figures. 4) Calculate the boiling point of a solution above 5) Calculate the freezing point of a solution...

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute....

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. a.Calculate the freezing point of a solution containing 13.0 g FeCl3 in 164 g water. b.Calculate the boiling point of a solution above. c.Calculate the freezing point of a solution containing 3.9 % KCl by mass (in water). Express your answer using two significant figures. d.Calculate the boiling point of a solution above. e.Calculate the freezing point of a solution containing 0.162 m MgF2....

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute....

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. a) Calculate the freezing point of a solution containing 12.2 g FeCl3 in 158 g water. b) Calculate the boiling point of a solution above. c) Calculate the freezing point of a solution containing 4.5 % KCl by mass (in water). d) Calculate the boiling point of a solution above. e) Calculate the freezing point of a solution containing 0.170 m MgF2. f) Calculate...

The boiling point of chloroform CHCl3 is 61.70°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves...

The boiling point of chloroform CHCl3 is 61.70°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin . How many grams of aspirin, C9H8O4 (180.1 g/mol), must be dissolved in 293.0 grams of chloroform to raise the boiling point by 0.450 °C ? _________g aspirin.

The boiling point of ethanol CH3CH2OH is 78.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves...

The boiling point of ethanol CH3CH2OH is 78.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen (estradiol). How many grams of estrogen, C18H24O2 (272.4 g/mol), must be dissolved in 265.0 grams of ethanol to raise the boiling point by 0.500 °C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl...

Subjects