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

Phosphorus pentachloride decompose according to the reaction PCl3(g)PCl3(g)+Cl2(g), 1 mol of PCl5 is placed in a 500 mL closed reaction vessel and allowed to reach equilibrium with decomposition products, phosphorus trichloride and chlorine at 523 K. Equilibrium constant, Kc=1.80. What is the composition of the mixture at equilibrium?

Open in App
Solution

Initial concentration of PCl5=10.5=2M.
PCl5(g)PCl3(g)+Cl2(g)
At t=0:200
At equilibrium :- (2x)xx
Now, KC=x×x2x1.80=x22x3.61.8xx2=0x=1.2
The equilibrium concentration of both the components of product is 1.2M.
Therefore, the composition of mixture at equilibrium is,
PCl5=0.83.2=0.25=25%
PCl3=1.23.2=0.375=37.5%
Cl2=1.23.2=0.375=37.5%

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