Question

Initially, only AA and BB are present, each at 2.00 MM. What is the final concentration of AA once equilibrium is reached

Answer 1

`[A]_(eq)=0.854M`

Step-by-step explanation:

Hello.

In this case, for the chemical reaction at equilibrium:

`A+B\rightleftharpoons C+D`

The equilibrium expression is:

`K=([C][D])/([A][B])=1.8`

Which in terms of the ICE methodology can be written as:

`1.8=(x*x)/((2.00M-x)(2.00M-x))`

Solving for
`x`, we obtain:

`x=1.15M`

It means that the concentration of A once equilibrium is reached turns out:

`[A]_(eq)=2.00M-1.15M=0.854M`

Best regards.