If a 2L reaction vessel initially contains 2 mols of Hydrogen and 2 mols of Iodine, what will be the molar concentrations at equilibrium of all species?
H2 (g) + I2 (g) --> 2HI (g)
Kc = 50.5
Initial concentration of H2 = mol of H2 / volume in L
= 2 moles / 2 L
= 1 M
Initial concentration of I2 = mol of I2 / volume in L
= 2 moles / 2 L
= 1 M
ICE Table:
Equilibrium constant expression is
Kc = [HI]^2/[H2]*[I2]
50.5 = (2*x)^2/(1-1*x)^2
sqrt(50.5) = (2*x)/(1-1*x)
7.106 = (2*x)/(1-1*x)
7.106-7.106*x = 2*x
7.106-9.106*x = 0
x = 0.78037
At equilibrium:
[H2] = 1.0-1x = 1.0-1*0.78037 = 0.220 M
[I2] = 1.0-1x = 1.0-1*0.78037 = 0.220 M
[HI] = +2x = +2*0.78037 = 1.56 M
Answer:
[H2] = 0.220 M
[I2] = 0.220 M
[HI] = 1.56 M
If a 2L reaction vessel initially contains 2 mols of Hydrogen and 2 mols of Iodine,...
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