The given reaction is
Br2 (g) + Cl2(g) 2 BrCl (g)
The reactants and products are all gaseous species.
n (g) = moles of gaseous products - moles of gaseous reactants = 2 - ( 1+1) = 0
Hence Kp = Kc = 1.1 x 10^-4 at 150 K
Mass of Br2 = 1.070 Kg = 1070 g
moles of Br2 = 1070 / 159.8 moles
Concentration of Br2 = moles / Volume = 1070 / [159.8 x 203] [ since volume = 203 L]
initial conc of Br2= 0.03298 M
Similarly
Mass of Cl2 = 1.115 Kg = 1115 g
moles of Cl2 = 1115 / 70.9 moles
Concentration of Cl2 = moles / Volume = 1115 / [70.9 x 203] [ since volume = 203 L]
initial conc of Cl2 = 0.07747 M
1)
Let 2x be the equilibrium concentration of BrCl. Then by ICE table
Kp = Kc = [2x]^2 / [0.03298-x] [0.07747-x] = 1.1 x 10^-4
since x is small we can approximate[ 0.03298 -x] as 0.03298 and [0.07747 - x ] as 0.07747
Therefore 4x^2 = 0.03298 x 0.07747 x 1.1 x 10^-4
= 28.1 x 10^-8
x^2 = 7.025 x 10^-8
x = 2.65 x 10^-4
Thus the concentration of BrCl = 2x = 2 x 2.65 x 10^-4 M = 5.3 x 10^-4 M
Hence the equilibrium conc of BrCl in the mixture = 5.3 x 10^-4 M
Therefore total moles present in 203 Litres = 203 x 5.3 x 10^-4 moles
= 0.1076 moles
Hence the mass of BrCl in the mixture of gases = 0.1076 x 115.35 = 12.41 g
Thus the mass of BrCl in the mixture at equilibrium is 12.41 g
2)
Now since the limiting reagent is Br2, if the reaction goes to 100% completion, the product formed is
[ 2 x 0.03298] M of BrCl
= 0.06596 M of BrCl
Therefore moles of BrCl in 203L of the gas = 0.06596 x 203 = 13.39 moles
Hence the mass of BrCl = 13.39 moles x 115.35 g / mol = 1545 g
Thus the theoretical amount of BrCl = 1545 g.
Hence the percentage yield is 12.41 x 100 / 1545 = 0.8%
Thus the % yield is 0.8%
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