Question

I’m a bit confused on how to do this ICE table question

Answer 1

When the Equilibrium equation for ammonia is solved, x is obtained:

`x=(1.849-1.214)/(-2)=-0.313`

using this value of x to calculate the concentration of the other components in the equilibrium:

[H2] = 0.275mol/L

[N2]=0.901mol/L

Then we can calculate the equilibrium constant using the following equation:

`\begin{gathered} k=([H_2]^3[N_2])/([NH_3]_^2) \\ k==(0.275^3\cdot0.901)/(1.84^2)=0.0055 \end{gathered}`