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At 700 K, equilibrium constant for the reaction `H_(2) (g) + I_(2) (g) hArr hArr 2 HI (g)" is "54*8`
If` 0*5 " mol " L ^(-1)` of HI (g) is present at equilibrium at 700 K, what are the concentrations of `H_(2) (g) and I_(2) (g) ` assuming that we initially started withHI(g) and allowed it to reach equilibrium at 700 K.

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` 2 HI(g) hArr H_(2) (g) + I_(2) (g), K= 1/54*8 `
At equilibrium , ` [HI] = 0*5 "mol" L^(-1) , [H_(2)] = [I_(2)] = x "mol" L^(-1) :. K= (x xx x)/(0*5)^(2)=1/(54*8).`
This gives ` x = 0*068 , i.e., [H_(2)] = [I_(2) = 0*068 "mol"L^(-1) .`

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