At equilibrium, the concentrations in this system were found to be [ N 2 ] = [ O 2 ] = 0.100 M [N2]=[O2]=0.100 M and [ NO ] = 0.600 M . [NO]=0.600 M. N 2 ( g ) + O 2 ( g ) − ⇀ ↽ − 2 NO ( g ) N2(g)+O2(g)↽−−⇀2NO(g) If more NO NO is added, bringing its concentration to 0.900 M, 0.900 M, what will the final concentration of NO NO be after equilibrium is re‑established?

### Answers

The final concentration of NO be after equilibrium is re‑established is 0.825 M.

Explanation:

The given balanced chemical equation is as follows.

Now, equilibrium constant for this reaction will be as follows.

It is given that concentrations at the equilibrium are:

= 0.1 M and [NO] = 0.6 M

Therefore, the value of is as follows.

= 36.0

NO concentration of 0.9 M is added to the system. So,

Initial: 0.1 0.1 0.9

Change: x x 2x

Equibm:(0.1 + x) (0.1 + x) (0.9 - 2x)

Now, we will find the value of x as follows.

36.0 =

x = 0.0375

Therefore, final concentration of NO after the equilibrium that is re-established is as follows.

0.9 - 2x

=

= 0.9 - 0.075

= 0.825 M

Therefore, we can conclude that the final concentration of NO be after equilibrium is re‑established is 0.825 M.