Ans :-
No. of moles of COCl2 = Molarity x Volume in L = 0.264 M x 10.5 L = 2.772 mol
No. of moles of each CO and Cl2 = Molarity x Volume in L = 8.15 x 10-2 M x 10.5 L = 0.85575 mol
Addition of 4.32 L, volume will change the concentration of each species and therefore new initial concentration of each species is :
Initial concentration of COCl2 = Moles/Volume in L = 2.772 mol / 4.32 L = 0.642 M
and
Initial concentration of each CO and Cl2 = Moles/Volume in L = 0.85575 mol / 4.32 L = 0.198 M
Now, ICE table is :
......................................COCl2 (g) <-------------------------> CO (g).....................+.........................Cl2 (g)
Initial.............................0.642 M..........................................0.198 M............................................0.198 M
Change..........................+y.......................................................-y......................................................-y
Equilibrium.................(0.642+y) M........................................(0.198-y) M.................................(0.198-y) M
Where, y = Amount dissociated per mole.
Expression of Equilibrium constant i.e. Kc (which is equal to the product of the molar concentration of products divided by product of the molar concentration of reactants raise to power their stoichiometric coefficient when reaction is at equilibrium stage).
Kc = [CO].[Cl2]/[COCl2]
2.52 x 10-2 = (0.198-y)2/(0.642+y)
y2 - 0.396 y + 0.039204 = 0.0161784 + 0.0252 y
y2 - 0.4212 y + 0.0230256 = 0
On solving
y = 0.06456
Therefore,
Equilibrium concentrations of each CO and Cl2 = 0.198-y = 0.198 - 0.06456 = 0.133 M
and
Equilibrium concentrations of COCl2 = 0.642+y= 0.642+ 0.06456 = 0.707 M
So,
[COCl2] = 0.707 M
[CO] = 0.133 M
and
[Cl2] = 0.133 M
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