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Question

At 300 K, the vapour pressure of an ideal solution containing 1 mole of A and 3 moles of B is 500 mm Hg. At the same temperature, 2 moles of B are added to this solution. The vapour pressure of the solution increases by 10% of the original vapour pressure. The correct statement(s) about the vapour pressure are :
  1. The vapour pressure of A in the pure state is 1300 mm Hg
  2. The vapour pressure of B in the pure state is 650 mm Hg
  3. The ratio of the final vapour pressure to the initial vapour pressure is 2 : 1
  4. The ratio of the vapour pressure of pure B to the vapour pressure of pure A is 13 : 1 


Solution

The correct options are
B The vapour pressure of B in the pure state is 650 mm Hg
D The ratio of the vapour pressure of pure B to the vapour pressure of pure A is 13 : 1 
nA = 1; nB = 3; PT = 500 mm Hg
When 2 moles of B is added 
nA = 1; nB = 5
As it is given that vapour pressure increases by 10%,
PT=500+500×10100=550
500 = PA(11+3)+PB(31+3)
2000 = PA+3PB(1)
550 = PA(16)+PB(56)
3300 = PA+5PB(2)
Solving (1) and (2)  we get,
 PA=50 mm Hg PB=650 mm Hg
PAPB=65050=13:1
 

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