20.An equilibrium mixture at 300K contains N2O4 and NO2 at 0.28 and 1.1 atm pressure respectively. If the volume of the container is doubled, calculate the new equilibrium pressure of two gases a)0.095,0.64 b)0.95,0.064 c)0.95,0.64 d)0.95,0.028

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Q. An equilibrium mixture at

300 K

contains

N_{2} O_{4}

and

{N O}_{2}

0.28

and

1.1

atm pressures respectively. If the volume of the container is doubled, calculate the new equilibrium pressure of the two gases.

Q. An equilibrium mixture at 300K contains

N_{2} O_{4}

and

N O_{2}

at 0.28 and 1.1 atm respectively. If the volume of the container is doubled and the new equilibrium pressures of

N O_{2}

x \times 10^{- 2}

atm, then

x - 60

is: (nearest integer value)

Q. For the reaction

N_{2} O_{4} ⇌ 2 N O_{2}

, equilibrium mixture contains

N O_{2}

P = 1.1 a t m

N_{2} O_{4}

P = 0.28 a t m

at 350 K. The volume of the container is doubled. Calculate the equilibrium pressures of the two gases when the system reaches new equilibrium :

At 298 K and 1 atm pressure, the partial pressures in an equilibrium mixture of $N_{2} O_{4}$ and $N O_{2}$ are 0.7 and 0.3 atmosphere respectively. What will be the partial pressure of $N O_{2}$ when the gases are in equilibrium at 298 K and at a total (equilibrium) pressure of 10 atmospheres?

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