Liquid M and liquid N form an ideal solution. The vapour pressures of pure liquids M and N are 450 and 700 mm Hg, respectively, at the same temperature. Then correct statement is: (x_M= Mole fraction of M in solution; x_N= Mole fraction of N in solution; y_M= Mole fraction of M in vapour phase; y_N= Mole fraction of N in vapour phase)
xMxN>yMyN
xMxN<yMyN
xMxN=yMyN
(xM-yM)<(xN-yN)
Solution:
Correct option is C. xMxN>yMyN Since PNo > PMo, so N is more volatile than M. ∴ yN > xN and xM > yM Multiply we get yN × xM > xN × yM i.e. xMxN = yMyN