The vapour pressure of two pure liquids A and B are 5 and 10 torr respectively. Calculate the total pressure of the solution (in torr) obtained by mixing 2 mole of A and 3 mole of B.
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The vapour pressure of two liquids P and Q are 80 torr and 60 torr respectively. The total vapour pressure obtained by mixing 3 mole of P and 2 mole of Q would be
100g of liquid A(molar mass 140"g mol"^(-1) ) was dissolved in 1000g of liquid B(molar mass 180"g mol"^(-1) ). The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 torr.
The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase. Apply Raoult's law P_(T)=P_(A)^(0)x_(A)+P_(B)^(0)x_(B)=P_(B)^(0)x_(A)+P_(B)^(0)(1-x_(A)) to calculate mole fraction of A(x_(A)) and B(x_(B)) . In vapour phase, partial pressure are used insted of number of moles.
Calculate the partial pressures N_2 and H_2 in a mixture of two moles of N_2 and two moles of H_2 at STP.
Vapour pressure of chloroform (CHCl_(3)) and dichloromethane (CH_(2)Cl_(2)) at 298 K are 200 mm Hg and 415 mm Hg respectively. (i) Calculate the vapour pressure of the solution prepared by mixing 25.5 g of CHCl_(3) and 40 g of CH_(2)Cl_(2) at 298 K and (ii) mole fractions of each component in vapour phase.
The vapour pressure of water is 12.3 k P_(a) at 300 K. Calculate the vapour pressure of 1 molal solution of a non-volatile solute in it.
The vapour pressure of a pure liquid A is 40 mm of Hg at 310K. The vapour pressure of its liquid in a solution with liquid B is 32 mm of Hg. Mole fraction of A in the solution, if it obeys Raoult's law is :
Vapour pressure of pure liquids P and Q are 700 and 450 mm Hg respectively at 330K. What is the composition of the liquid mixture at 330 K, if the total vapour pressure is 600 mm Hg?
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