Answer:
[tex][A]_{eq}=0.854M[/tex]
Explanation:
Hello.
In this case, for the chemical reaction at equilibrium:
[tex]A+B\rightleftharpoons C+D[/tex]
The equilibrium expression is:
[tex]K=\frac{[C][D]}{[A][B]}=1.8[/tex]
Which in terms of the ICE methodology can be written as:
[tex]1.8=\frac{x*x}{(2.00M-x)(2.00M-x)}[/tex]
Solving for [tex]x[/tex], we obtain:
[tex]x=1.15M[/tex]
It means that the concentration of A once equilibrium is reached turns out:
[tex][A]_{eq}=2.00M-1.15M=0.854M[/tex]
Best regards.
