CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

At 540 K, 0.10 mole of PCl5 are heated in an 8 litre flask. The pressure of equilibrium mixture is found to be 1.0 atm. Calculate Kp and Kc for the reaction.

Open in App
Solution

PCl5PCl3(g)+Cl2(g)
At equi,(mole) (0.1x x x
total number of moles, n=(0.1x)+x+x=(0.1+x)
PV=nRT
1×8=(0.1+x)×0.082×540
or x=0.08
Kc=[PCl3][Cl2][PCl5]=x2(0.1x)×8=4×102molL1
Kp=Kc(RT)Δn=Kc(RT)[Δn=+1]=4×102×0.082×540=1.77atm

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Equilibrium Constants
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon