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:

( = Mole fraction of

Question

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:

( = Mole fraction of 'M' in solution;  = Mole fraction of 'N' in solution;  = Mole fraction of 'M' in vapour phase;  = Mole fraction of 'N' in vapour phase;)

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Strategy:
 For an ideal solution, the vapour is enriched in the more volatile component (Konovalov's Rule). Relate the liquid phase ratios to the vapour phase ratios using pure state vapour pressures.

Step 1: Identify the more volatile component
 and .
N is more volatile.

Step 2: Relate the ratios

Dividing the two:

Step 3: Analyze the inequality
Since :

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