For the following reaction in equilibrium
PCI;(9) = PCI;(9) + Cl (9)
Vapour density is found to be 100 when 1 mole of PCI, is taken in a 10 litre flask at 27°C.
Calculate the equilibrium pressure.
(1) 1.57 atm
(2) 2.57 atm
(3) 3.57 atm
(4) 4.57 atm
Answers
Answered by
6
The value of equilibrium pressure is 2.57 atm.
Option (2) is correct.
Explanation:
PCI5(g) ⇆ PCI3 (g) + Cl2 (g)
We know that
α = Mi - Mf / Mf (n-1)
Where
Mi = Molar mass before dissociation
Mf = Molar mass after dissociation
n = number of moles of product
Mi = 31 + 5 x 35.5 = 208.5
Mf = 2 x VoDo = 2 x 100 = 200
n = 2
α = 208.5 - 200 /200 (2 -1) = 4.25 / 100
% dissociation of PCl5 = α x 100
= 4.25 / 100 x 100 = 4.25 %
We also know that total no. of moles at equilibrium = 1 + α (n-1)
= 1 + 4.25 / 100 (2-1)
= 1.0425
Total pressure at equilibrium
PV = nRT
P = nRT/ V
P = 1.0425 x 0.082 x 300 / 10 = 2.57 atm
Thus the value of equilibrium pressure is 2.57 atm.
Answered by
1
Answer:
2.57atm
Explanation:
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