A beaker filled with an equimolar liquid mixture of ethyl alcohol and ethyl acetate evaporates

s we know the Raoult's law states that : For an ideal solution, the equilibrium partial pressure pA of a constituent at a fixed temperature equals the product of its vapor pressure PA and its mole fraction in the liquid XA. Let A as Ethyl alcohal an

Raolt' s law
Pp = partial pressure = Pv *x here
Pp = partial pressure and
Pv = vapour pressure
x = mole fraction of the fluid no of moles of liquid ethyl alcohol =0.5 no of moles of liquid

ethyl acetate =0.5 temperature of liquid mixture = 0 oc ( T =273 ok ) and P = 1 atm = 101 Kpa Pp = Pv.* x= 3,23 *0.5 =1.615 kpa ( for ethyl acetate)
Pp = Pv*x =1.62 *0.5 =0.81 kpa ( for ethyl alcohal )
Pt = Pp + Pp = 1.615 +0.81 = 2.425 kpa molecular
wt of ethyl alcohol = C2H5OH = 12*2 +6*1 +16*1 =24 +6 +16 =46 kg /kmol molecular wt of ethyl acetate = C2H5C00CH3=4*12 +2*16 +8*1 =48 +32+8 =88 kg/kmol mass of ethyl acetate = 88 *0.5 = 44 kg mass of ethyl alcohal = 46 *0.5 = 23 kg now, y1 = mol fraction of vapour of ethyl acetate here Pt =101 kpa y1 *Pt = Pp .x1 y1 = 3.23*0.5 /101 =0.015 y2 = mole fraction of ethyl alcohall
y2*Pt =Pp* x= y2 =Pp*x/Pt= 1.62 *0.5/ 101 y2 =0.008 by ideal gas law- P.V =n.R.T N =n = P.V/R.T N = 1*22.4.