The vapour pressure of pure liquid `M & N` are `700mm` of `Hg` and `450mm` of `Hg` respectively. Which of the following option is correct ? Given : `X_(N),X_(M)=` mole fraction of `N & M` in liquid phase `Y_(N),Y_(M)=` mole fraction of `N & M` in vapour phase
Liquid ‘M’ and liquid ‘N’ form an ideal solution. The vapour pressures of pure liquids ‘M’ and ‘N’ are 450 and 700 mmHg, respectively, at the same temperature. Then correct statement is: ( x_(M)= Mole fraction of ‘M’ in solutions , " " 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)
For an ideal liquid solution with P_A^(@)gtP_A^(@) , which relation between X_(A) ((mole fraction of A in liquid phase) and Y_(A) (mole fraction of A in vapour phase) is correct ?
For an ideal binary liquid solution with p_(A)^(@) gt p_(B)^(@) which of the following relations between x_(A) (mole fraction of A in liquid phase) and y_(A) (mole fraction of A in vapour phase) is correctly represented?
Vapour pressure of pure liquid A & B are 21 & 18 mm of Hg respectively. Determine vapour pressure of a solution obeying Raoult's law containing 1 mole of A& 2mole of B
For an ideal binary liquid solutions with P_(A)^(@)gtP_(B)^(@) , which relation between X_(A) (mole fraction of A in liquid phase) and Y_(A) (mole fraction of A in vapour phase) is correct:
At 300 K the vapour pressure of two pure liquids, A and B are 100 and 500 mm Hg, respectively. If in a mixture of a and B, the vapoure is 300 mm Hg, the mole fractions of a in the vapour phase, respectively, are -
