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Two liquids 'A' and 'B' form an ideal solution. At 300K, the vapour pressure of a solution containing 1 mol of A and 3 mol of B is 550 mm Hg. At the same temperature if one more mole of B is added to this solution, the vapour pressure of the solution increases by 10 mm Hg. Determine the vapour pressure of 'A' and 'B' in their pure states.

A
pA=400 mm Hg and pB=600 mm Hg
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B
pA=600 mm Hg and pB=400 mm Hg
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C
pA=300 mm Hg and pB=700 mm Hg
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D
pA=700 mm Hg and pB=300 mm Hg
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Solution

The correct option is A pA=400 mm Hg and pB=600 mm Hg

Let the vapour pressure of pure 'A' be pA and the vapour pressure of pure 'B' be pB
Initially,
Mole fraction of A, XA=14
Mole fraction of B, XB=34

Total vapour pressure of solution,
=XA.pA+XB.pB550=14pA+34pBor2200=pA+3pB ....eq(i)

After addition of 1 mol of B,
Total vapour pressure of solution
(1 mol of A + 4 mol B),
=15pA+45pB560=15pA+45pBor 2800=pA+4pB ....eq(ii)
Solving equations (i) and (ii), we get,
pB=600 mm Hg vapour pressure of pure 'B'
pA=400 mm Hg vapour pressure of pure 'A'

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