Home
Class 11
CHEMISTRY
At equilibrium, N2O(4(g)) Leftrightarrow...

At equilibrium, `N_2O_(4(g)) Leftrightarrow 2NO_(2(g))` the observed molecular weight of `N_(2)O_(4),` is 80 g mol`""^(-1)` at 350 K. The percentage dissociation of `N_2O_(4(g))` at 350 K is

A

0.1

B

0.15

C

0.2

D

0.18

Text Solution

Verified by Experts

The correct Answer is:
B
`N_(2)O_(4(g)) Leftrightarrow 2NO_(2(g))`
Degree of dissociation may be calculated as `x=(N-m)/((n-1)m) ` [n=2 number of moles produced by 1 mol)
`=(92-80)/((2-1)80)=(12)/(80)=0.15`
Percentage dissociation `=0.15 xx 100=15%`
Promotional Banner

Similar Questions

Explore conceptually related problems

At equilibrium of the reaction , N_(2)O_(4)(g) hArr 2NO_(2)(g) the observed molecular weight of N_92)O_(4) is 80g mol^(-1) at 350K. The percentage dissociation of N_(2)O_(4)(g) at 350K is

In reaction N_(2)O_(4)(g)rarr 2NO_(2)(g), The observed molecular weight "80 gmol"^(-1) at 350 K. The percentage dissociation of N_(2)O_(4)(g) at 350 K is

At the equilibrium of the reaction , N_(2)O_(4)(g)rArr2NO_(2)(g) , the observed molar mass of N_(2)O_(4) is 77.70 g . The percentage dissociation of N_(2)O_(4) is :-

During thermal dissociation, the observed vapour density of N_(2)O_(4)(g) is 26.0. The extent of dissociation of N_(2)O_(4) is:

The value of K_P for the equilibrium reaction N_2O_2(g)harr2NO_2(g) is 2. The percentage dissociation of N_2O_2(g) at a pressure of 0.5 atm is