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One mole of N2O(4(g)) at 300 K is kept i...

One mole of `N_2O_(4(g))` at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K to decompose to `NO_(2(g))`. If the resultant pressure at equilibrium is 2.4 atm, then which is correct?

A

% dissociation = 20%

B

pressure of `NO_2` at equilibrium = 0.8 atm

C

pressure of `N_2O_4` at equilibrium =1.2 atm

D

`K_p = 0.4` atm

Text Solution

Verified by Experts

The correct Answer is:
A, B, D
`underset(1-alpha)underset(1)(N_(2)O_(4)) harr underset(2alpha)underset(0)(2NO_(2))`
Total no. of moles at equlibrium = `1+alpha`
from Ideal gas equation
`(P_(1))/(P_(2))=(n_(1)T_(1))/(n _(2)T_(2)), underset("equlibrium")underset("before")((P_(1))/(n_(1)T_(1)))=underset("equlibrium")underset("after")((P_(2))/(n_(2)T_(2)))`
`(1)/(1 xx 300)=(2.4)/((1+alpha)600) implies alpha=0.2 implies %alpha = 20%`
`P_(NO_(2))=(2alpha)/(1+alpha)`, Total pressure = 0.8
`K_(P)=(P_(NO2)^(2))/(P_(N_(2)O_(4)))=0.4` atm
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