wiz-icon
MyQuestionIcon
MyQuestionIcon
5
You visited us 5 times! Enjoying our articles? Unlock Full Access!
Question

9.2grams of N2O4(g) is taken in a closed one-litre vessel and heated till the following equilibrium is reached.

N2O4(g)2NO2(g)

At equilibrium, 50% N2O4(g) is dissociated. What is the equilibrium constant? (in mol litre1)

[Molecular weight of N2O4=92]

A
0.1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
0.4
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
0.2
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
2
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is C 0.2
Given
Mass of N2O4 = 9.2g
Solution
N2O4(g)=2NO2(g)
Initial moles of N2O4 are 9.292 =0.1 moles
50% get dissociated at equilibrium
Therefore At equilibrium, Moles of N2O4 dissociated are 0.05mole
In reaction, every Mole of N2O4 give 2 moles of NO2.
Therefore At equilibrium no. of moles of NO2 formed = 0.05* 2
Kc=[NO2]2N2O4
Kc=(0.10)20.05
Kc=0.2 mol/L
The correct option is C

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Laws of Mass Action
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon