At 2000°C, the equilibrium constant for the reaction below is Kc = 4.10 ´ 10–4 . If 0.600 moles of NO is placed in a 1.0-L reaction vessel, what will the equilibrium concentration of N2 be?

At equilibrium, the concentration of is going to be 0.30M

Explanation:

We first need the reaction.

With the information given we can assume that is:

+ ⇄ 2

If there is placed 0.600 moles of NO in a 1.0-L vessel, we have a initial concentration of 0.60 M NO; and no nor   present. Immediately, and are going to be produced until equilibrium is reached.

By the ICE (initial, change, equilibrium) analysis:

I: []=0   ;     [ ]= 0    ; []=0.60M

C: []=+x   ;     [ ]= +x    ; []=-2x

E: []=0+x   ;     [ ]= 0+x   ; []=0.60-2x

Now we can use the constant information:

=

=

=

At equilibrium, the concentration of is going to be 0.30M

the increase of protons   hope this