At 298 K, 500cm^{3} H_{2}O dissolved 15.30 cm^{3} CH_{4}(STP) under a partial pressure of methane of one atm. If Henery's law holds, what pressure is required to cause 0.001 mole methane to dissolve in 300cm^{3} water ?

(a) 0.286 atm

(b) 2.486 atm

(c) 1.286 atm

(d) 3.111 atm

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Dalton’s Law of Partial Pressure/ Henry"s law

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The partial pressure of ethane over a saturated solution containing 6.56 X 10^{-2} g of ethane is 1 bar. If the solution contains 5.00 X 10^{-2} g of ethane, then what shall be the partial pressure of the gas.

(a) 0.76 bar

(b) 0.16 bar

(c) 1.16 bar

(d) 3.12 bar

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Dalton’s Law of Partial Pressure/ Henry"s law

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How much oxygen is dissolved in 100ml water at 298K if partial pressure of oxygen is 0.5 atm and K_{H}=1.4X10^{-3} M/atm ?

(1) 22.4 mg

(2) 22.4 g

(3) 2.24 g

(4) 2.24 mg

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Dalton’s Law of Partial Pressure/ Henry"s law

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The total vapour of a solution of liquid A and liquid b is 600 torr. The mole fraction of component A in liquid phase is 0.7. The vapour pressure of pure A and B are respectively

(1) 300 torr, 130 torr

(2) 1300 torr, 130 torr

(3) 300 torr, 1300 torr

(4) 300 torr, 300 torr

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Dalton’s Law of Partial Pressure/ Henry"s law

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The vapour pressure of water at room temperature is 30 mm of Hg. If the mole fraction of the water is 0.9, the vapour pressure of solution will be

(1) 30 mm of Hg

(2) 24 mm of HG

(3) 21 mm of Hg

(4) 27 mm of Hg

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Dalton’s Law of Partial Pressure/ Henry"s law

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p_{A} and p_{B}, are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution.If x, represents the mole fraction of component A, the total pressure of the solution will be.

(a) p_{A} + x_{A}(p_{B}-p_{A})

(b) p_{A} + x_{A}(p_{A}-p_{B})

(c) p_{B} + x_{A}(p_{B}-p_{A})

(d) p_{B} + x_{A}(p_{A}-p_{B})

NEET - 2012

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Dalton’s Law of Partial Pressure/ Henry"s law

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An ideal mixture of liquids A and B with 2 moles of A and 2 moles of B has a total vapour pressure of 1 atm at a certain temperature. Another mixture with 1 mole of A and 3 moles of B has a vapour pressure greater than 1 atm. But if 4 moles of C are added to the second mixture, the vapour pressure comes down to 1 atm. Vapour pressure of C, P_{c}° = 0.8 atm. Calculate the vapour pressures of pure A and pure B.

(1) P_{A}° = 1.4 atm, P_{B}° = 0.7 atm

(2) PA = 1.2 atm, P_{B}° = 0.6 atm

(3) PA = 1.4 atm, P_{B}° = 0.6 atm

(4) P_{A}° = 0.6 atm, P_{B}° = 1.4 atm

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Dalton’s Law of Partial Pressure/ Henry"s law

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The vapor pressures of benzene, toluene and a xylene are 75 Torr, 22 Torrand 10 Torr at 20°C. Which of the following is not a possible value of the vapor pressure of an equimolar binary/ternary solution of these at 20°C ? Assume all form ideal solution with each other.

(1) 48$\frac{1}{2}$

(2) 16

(3) $35\frac{2}{3}$

(4) 53$\frac{1}{2}$

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Dalton’s Law of Partial Pressure/ Henry"s law

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Explain why aquatic species are more comfortable in cold water rather than in warm water. (2 marks)

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Dalton’s Law of Partial Pressure/ Henry"s law

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State Henry's law and mention two of its important applications. (2 marks)

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Dalton’s Law of Partial Pressure/ Henry"s law

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