One mole of pcl5 is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.
Answers
Hi, please consider the answer given below
The question is one mole of pcl5 is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.
So here you need to get the equilibrium concentrations of PCl5, PCl, and Cl2.
Equation for dissociation; PCl5 ----------> PCl3 + Cl2
equilibrium concentrations are; PCl = 0.4 M, PCl3 =0.6 M, Cl2= 0.6M
So equillibrium constant is = 0.6 x 0.6/0.4
= 0.9
Answer:
the answer is 9
Explanation:
pcl5 ⇔ pcl3 + pcl2
at initial time moles: 1 0 0
at euillibrium 1-α(1) α(1) α(1)
here α is degree of dissociation
we know that alpha = 0.6 from question
therefore mole of pcl3 is also 0.6 and moles of pcl5 is 1-0.6 =0.4
Kc = [pcl3][cl2]/[pcl3]
kc= 0.6*0.6/0.4
kc=0.36/0.4
kc=9
hope i explained very clearly took more than 10mins to explain u clearly mark as brainliast answer :)