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State the Henry's law about partial pres...

State the Henry's law about partial pressure of a gas in a mixture.

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Henry.s law about partial pressure of a gas in a mixture
The partial pressure of the gas (p) in vapour phase is proportional to the mole fraction of the gas (x) in the solution. It may be expressed as
`p = K_H.x`
where p = partial pressure of the gas
`K_H` = Henry.s constant
x = mole fraction of the gas
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Knowledge Check

  • According to Henry's law the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution . For different gases the correct statement about Henry's constant is

    A
    higher the value of `K_H` at a given pressure , higher is the solubility of the gas
    B
    higher the value of `K_H` at a given pressure , lower is the solubility of the gas
    C
    `K_H` is not a function of nature of gas
    D
    `K_H` value for all gases is same at a given pressure

  • A gaseous mixture contains 220 g of carbon dioxide and 280 g of nitrogen gas. If the partial pressure of nitrogen gas in the mixture is 1.5 atm then the partial pressure of carbon dioxide gas in the mixture will be

    A
    1.25 atm
    B
    0.75 atm
    C
    0.50 atm
    D
    3 atm

  • According to Henry's law, the partial pressure of gas (p'_(g)) is directly proportional to mole fraction of gas in dissolved state, i.e., P_("gas")'=K_(H),X_("gas") where K_(H) is Henry's constant. Which are correct?

    A
    `K_(H)` is characteristic constant for a given gas-solvent system
    B
    Higher is the value `K_(H)`, lower is soubility of gas for a given partial pressure of gas
    C
    `K_(H)` has temperature dependence
    D
    `K_(H)` increase with temperature.

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