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How many moles per litre of PCl5 has to be taken to obtain 0.1 mole of Cl2 if the value of equilibrium constant is 0.04: A. 0.15 B. 0.25 C. 0.35 D. 0.05

How many moles per litre of PCl5 has to be taken to obtain 0.1 mole of Cl2 if the value of equilibrium constant is 0.04:
A. 0.15
B. 0.25
C. 0.35
D. 0.05

Grade:12th pass

1 Answers

Arun
25750 Points
4 years ago
Consider a as initial concentration of PCl5 and x be degree of dissociation.
Dissociation of PCl5 takes place according to following reaction
PCl5 → PCl3+Cl2
Initial conc: a 0 0
Final conc : a(1-x) ax ax
[Cl2] = 0.1 = ax ...(1)
Kc = ([PCl3][Cl2])/ [PCl5]
0.04 = (ax. ax)/a(1-x)
Solving this we'll get,
x=0.4
From (i) 
a = 0.1/0.4 = 0.25
Hence, we can say moles of PCl5 added is 0.25 moles
 
 

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