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An equilibrium mixture at 300 K contains...

An equilibrium mixture at `300 K` contains `N_(2)O_(4)` and `NO_(2)` at `0.28` and `1.1 atm`, respectively. If the volume of container is doubles, calculate the new equilibrium pressure of two gases.

Text Solution

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`{:(,N_2O_4(g) hArr, 2NO_2(g)),("Pressure at equilibrium",0.28,1.1):}`
`K_p=(p(NO_2)^2)/(p(N_2O_4))=(1.1)^2/(0.28)`=4.32 atm
If volume of the container is doubled , the pressure will be reduced to half.
`{:(,N_2O_4 hArr, 2NO_2),("New pressure", (0.28/2-p),(1.1/2+2p)):}`
`K_p=((1/1/2+2p)^2)/(0.28/2-p)`=4.32
Solving p=0.045
`therefore p(N_2O_4)` =0.14-0.045=0.095 atm
`p(NO_2)` =0.55+2(0.045)=0.64 atm
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An equilibrium mixture at 300 K contains N _(2) O_(4) and NO_(2) at 0*28 and 1*1 atm respectively. If the volume of the container is doubled, calculate the new equilibrium pressures of two gases.

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Knowledge Check

  • An equilibrium mixture at 300K contains N_(2)O_(4) and NO_(2) at 0.28 and 1.1 atm pressure, respectively. If the volume of the container is doubled, the new equilibrium pressure of these two gases are respectively.

    A
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  • An equilibrium mixture at 300 K has N_(2)O_(4) and NO_(2) at 0.28 atm and 1.10 atm pressures. If the volume of container doubled at same temperature. Calculate the new equilibrium pressures for the gases.

    A
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    B
    1.095, 2.64 atm
    C
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  • An equilibrium mixture at 300 K has N_(2)O_(4) and NO_(2) at 0.28 atm and 1.10 atm pressures. If the volume of container doubled at same temperature. Calculate the new equilibrium pressures for the gases.

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    C
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