Question

What is the value of X, using the ICE method?

Given:

The initial concentrations are [H2O]=0.125M[H2O]=0.125M and [Cl2]=0.270M [Cl2]=0.270M. The equilibrium constant Kc for the reaction

H2O(g)+Cl2(g)⇌2HCl(g)+O2(g)H2O(g)+Cl2(g)⇌2HCl(g)+O2(g)

is 8.96×10−98.96×10−9 at 298 K.

Answer 1

1)

balanced equation :

2 H2O(g) + 2 Cl2(g) <-------------> 4 HCl (g) + O2(g)

0.125           0.270                               0               0   ----------> I

-2x                -2x                               +4x           +x      ---------> C

0.125-2x       0.270-2x                        4x              x       ---------> E

Kc = (4x)^4 (x) / (0.125 -2x)^2 (0.270-2x)^2

8.96×10^−9 = 256 x^5 / (0.125 -2x)^2 (0.270-2x)^2

here Kc value is very small .so we neglect x in the denominator.

8.96×10^−9 = 256 x^5 / (0.125)^2 (0.270)^2

x = 2.09 x 10^-3

value of X = 0.00209 M