Home
Class 11
CHEMISTRY
Calculate the total pressure in a 10 L ...

Calculate the total pressure in a 10 L cylinder which contains `0.4` g helium ,1.6 of oxygen and 1.4 g nitrogen at `27^(@)C`. Also calculate the partial of helium gas in the cylinder. Assume ideal hehaviour for gases.

Text Solution

Verified by Experts

Total number of moles `=(0*4)/(4)+(1*6)/(32)+(1*4)/(28)=0.1+05+0*05=0*2` moles.
`pV=nRT`
`pxx10L=0*2xx0*82xx300rArr p=(24*6xx0*2)/(10)`
`p=0*492 atm`
`P_(He)(0.1)/(0.2)xx0*492=0*246` atm
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • STATES OF MATTER : GASES AND LIQUIDS

    SUBHASH PUBLICATION|Exercise THREE MARK QUESTIONS AND ANSWERS|9 Videos

  • STATES OF MATTER : GASES AND LIQUIDS

    SUBHASH PUBLICATION|Exercise NUMERICAL PROBLEMS AND ANSWERS|25 Videos

  • STATES OF MATTER : GASES AND LIQUIDS

    SUBHASH PUBLICATION|Exercise NUMERICAL PROBLEMS AND ANSWERS|25 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    SUBHASH PUBLICATION|Exercise NUMERICAL PROBLEMS AND ANSWERS:|49 Videos

  • STRUCTURE OF ATOM

    SUBHASH PUBLICATION|Exercise NUMERICAL PROBLEMS AND ANSWERS|29 Videos

Similar Questions

Explore conceptually related problems

Calculate the total pressure in a 10 L cylinder which contains 0.4 g of helium, 1.6 g of oxygen and 1.4 g of nitrogen at 27^(@) C. Also calculate the partial pressures of He gas in the cylinder. Assume Ideal behaviour for gases. R = 0.082 L atm k^(-1) mol^(-1)

Calculate the number of atoms and volume of 1g helium gas at STP

Knowledge Check

  • 3.2 g of oxygen and 0.2 g of hydrogen are placed in a 1.12 L flask at 0^(@)C . The total pressure of the gas mixture will be

    A
    1 atm
    B
    4 atm
    C
    3 atm
    D
    2 atm

  • What will be the total pressure of a mixture of 4 g O_2 +4g N_2 confined in a volume of 1 L at 273 K?

    A
    4
    B
    6
    C
    8
    D
    10

  • 3.2 g of oxygen and 0.2 g of hydrogen are placed in a 1.12 L flask at 0^@C . The total pressure of the gaseous mixture will be

    A
    1 atm
    B
    4 atm
    C
    3 atm
    D
    2 atm

    • Similar Questions

    Explore conceptually related problems

    The osmotic pressure of a solution containing 40 g of solute ("molecular mass 246") per litre at 27^(@)C is (R=0.0822 atm L mol^(-1))

    Ethylene bromide C_(2)H_(4)Br_(2) , and 1,2 -dibromopropane, C_(3)H_(6)Br_(2) ,form a series of ideal solutions over the whole range of composition. At 85^(@)C , the vapour pressure of these two pure liquids are 173 and 127 torr, respectively. . If 10.0 g of ethylene bromide is dissolved in 80.0 g of 1,2-dibromopropane, calculate the partial pressure of each component and teh total pressure of the solution at 85^(@)C . b. Calculate the mole fraction of ethylene bromide in the vapour in equilibrium with the above solution. c. What would be the mole fraction of ethylene bromide in a solution at 85^(@)C equilibrated with a 50 : 50 mole mixture in the vapour?

    0.24g sample of a compound of oxygen and boron was found by analysis to contain 0.144g of oxygen and 0.096g of boron. Calculate the percentage composition of the compound by weight. (AS-1)

    A 10 g mixture of glucose and urea present in 250 mL solution shows the osomotic pressure of 7.4 atm at 27^(@)C . Calculate % composition of mixture.

    The osmotic pressure of a solution containing 4.0 g of solute (molar mass 246) per litre at 27^@C is (R=0.082 l atm k^(-1) mol^(-1)),

    Home
    Profile