wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Calculate pressure required for 50% dissociation of PCl5. If the Kp at that temprature is 1.8 atm.

A
3 atm
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
5.4atm
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
9atm
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
none
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is D 5.4atm
PCl5PCl3+Cl2
given, Kp=1.8
Moles of different gases at equilibrium are PCl5=0.5 moles
PCl3=0.5 moles
Cl2=0.5 moles
therefore, total number of moles =1.5 moles
Partial pressure are PPCl3=PPCl5=PCl2=0.51.5P
where P is total pressure in atmosphere.
Kp=(PPCl3)(PCl2)(PPCl5)=(0.51.5)2P2(0.51.5)P=13P
13P=1.8
P=5.4 atm
Pressure is 5.4 atmosphere.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Fruendlich and Langmuir Isotherms
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon