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The density of a mixture of O(2) and N(2...

The density of a mixture of `O_(2) and N_(2)` at STP is 1.3 g/litre: Calculate the partial pressure of `O_(2)`

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0.28 atm
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The density of a mixture of O_(2) and N_(2) at NTP is 1.3 g/L. Calculate partial pressure of O_(2) .

The density of a mixturee of O_(2) and N_(2) gases at 1 atm and 273 K is 0.0013 gm/mL. If partial pressure of O_(2) in the mixture is A, then calculate value of 25 A.

Knowledge Check

  • If the density of a mixture of O_(2)&N_(2) at N.T.P. is 1.258 g//l. The partial volume of O_(2) in 3 mole of mixture is

    A
    `1L`
    B
    `2L`
    C
    `3L`
    D
    `4L`

  • Equal weight of N_(2) and O_(2) are put in a flask at 27^(@)C Calculate the partial pressure of N_(2) if partial pressure O_(2)=0.44 atm.

    A
    0.44atm
    B
    0.50atm
    C
    0.94atm
    D
    0.38atm

    • Similar Questions

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    The vapour density of a mixture of NO_(2) and N_(2)O_(4) is 38.3 at 26.7^(@)C . Calculate the number of moles of NO_(2) in 100 g of the mixture.

    The vapour density of a mixture containing NO_(2) and N_(2)O_(4) is 38.3 at 27^(@)C . Calculate the mole of NO_(2) in 100 g mixture.

    The total pressure of a gaseous mixture of 2.8 g N_(2) , 3.2 g O_(2) , and 0.5 g H_(2) is 4.5 atm . Calculate the partial pressure of each gas.

    At 25^(@)C and 1 atm pressure, the partial pressure in equilibrium mixture of N_(2)O_(4) and NO_(2) , are 0.7 and 0.3 atm , respectively. Calculate the partial pressures of these gases when they are in equilibrium at 25^(@)C and a total pressure of 10 atm .

    Calculate the mole present of N_(2) gas in a mixture of N_(2) and O_(2) if the partial pressure of O_(2) is 6.3 cm of Hg in a container of volume 22.4 litre and total pressure is 90 cm of Hg at 300 K

    The density of an equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm and 373.5K is 2.0 g/L. Calculate K_(C) for the reaction N_(2)O_(2)(g) iff 2NO_(2)(g)

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