The chemical equilibrium being studied is H_2 + I_2 = 2HI In the beginning, only

Question

The chemical equilibrium being studied is H_2 + I_2 = 2HI In the beginning, only 0.05 mole of each H_2 and l_2 are present When the system reaches equilibrium, the molar quantities are as follows: H_2 and I_2 = 0.02 mole each. HI = 0.06 moles. The reaction is taking place in a 2.0 container at 300K. Assume all reactants and products behave as ideal gases. From this data, find extent of reaction, equilibrium constant K, Delta G and Delta Go Find K for this reaction at 500K. if Delta Hf for HI = 263 KJ/mol 18.07 cm^2

Explanation / Answer

H2 + I2 ----------> 2 HI

Initial 0.05 0.05 0

Eqn. 0.02 0.02 0.06

Degree of dissasociation = 1-Ceq(of reactant)/Cin(of reactant) = 1 - 2/5=3/5 = 60 %

Now Kc = [HI]2/[I2][H2]

= 0.0036/0.0004 = 9

At equilibrium G = 0,

Now we know G= G0 + RTlnK

SO  G0 = -RTlnK =-2.303*8.314*300*log9 = 5481.1 J

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