At 700 K , the equilibrium constant for the reaction : H_2(g) + I_2(g) hArr 2HI(g)is 54.8 . If 0.5 mol L^(-1)of HI(g) is present at equilibrium at 700 K, what are the concentrationof H_2(g) and I_2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K ?

At 700 K , the equilibrium constant for the reaction : H_2(g) + I_2(g

1.	At 700 K , the equilibrium constant for the reaction : H_2(g) + I_2(g) hArr 2HI(g)is 54.8 . If 0.5 mol L^(-1)of HI(g) is present at equilibrium at 700 K, what are the concentrationof H_2(g) and I_2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K ?
Answer» Solution :`{:(,2HI(G) hArr,H_2(g) +, I_2),("At equi.",0.5,X,x):}` `K_c=([H_2][I_2])/[HI]^2=1/54.8` `x^2/(0.5)^2=1/54.8` `x^2=0.25/54.4.56xx10^(-3)` x=0.068 `[H_2]=[I_2]="0.068 mol L"^(-1)`