Question

Diethyl ether, C4H10O was a widely used anesthetic in the early days of surgery. It has a vapor pressure of 537 torr at 25 oC. A 10.00 mL sample (D = 0.708 g/mL) is placed in a sealed 0.205 L flask. What is the maximum volume in liters the flask can have if equilibrium is to be maintained between liquid and vapor?

Answer 1

`V=3.32 L`

Step-by-step explanation:

Moles in the sample:

`n=10 mL*(0.708g)/(mL)*(1mol)/(74g)`

`n=0.096mol`

Max. volume to be in equilibrium:

`V=(n*R*T)/(P)`

`V=(0.096mol*0.082 atm*L*mol^(-1)*K^(-1)*298K)/(0.707atm)`

`V=3.32 L`

If the volume is higher, the pressure will be less than the vapour pressure and the sample will be all gas and not L-V equilibrium.