The total vapour pressure of an ideal binary solution containing two volatile liquids, X and Y, is given by the equation P = 250 - 110 x_ X (in torr), where x_ X is the mole fraction of X in the liquid phase. The vapour pressures of pure X and pure Y, and the identity of the more volatile component, respectively, are:

Step-by-step solution

The total vapour pressure of an ideal binary solution is given by Raoult's law: P = P_ X ^ x_ X + P_ Y ^ x_ Y Since x_ X + x_ Y = 1 , we can substitute x_ Y = 1 - x_ X : P = P_ X ^ x_ X + P_ Y ^ (1 - x_ X ) P = P_ Y ^ + (P_ X ^ - P_ Y ^ ) x_ X Comparing this with the given equation P = 250 - 110 x_ X : 1) The intercept corresponds to the vapour pressure of pure Y: P_ Y ^ = 250 torr 2) The slope corresponds to the difference in pure vapour pressures: P_ X ^ - P_ Y ^ = -110 P_ X ^ - 250 = -110 P_ X ^ = 140 torr Alter