Question

44.Consider the following reaction
N2(g) + O2(g) + 2NO ) K = 0.1 at 2000°c ta
If original concentrations of N, and o, were 0.1M each. Calculate
the concentrations of NO at equilibrium.​

Answer 1

Explanation:

You know that at

2000

∘

C

, the reaction

N

2

(

g

)

+

O

2

(

g

)

→

2

NO

(

g

)

has an equilibrium constant equal to

K

c

=

4.1

⋅

10

4

Now, the equilibrium constant is calculated by taking the equilibrium concentrations of the chemical species involved in the reaction.

K

c

=

[

NO

]

2

[

N

2

]

⋅

[

O

2

]

At equilibrium, you have

At equilibrium, you have

[

N

2

]

=

0.036 mol L

−

1

[

O

2

]

=

0.0089 mol L

−

1

Rearrange the equation to isolate the equilibrium concentration of nitric oxide.

[

NO

]

=

√

K

c

⋅

[

N

2

]

⋅

[

O

2

]

Plug in your values to find

[

NO

]

=

√

4.1

⋅

10

4

⋅

0.036 mol L

−

1

⋅

0.0089 mol L

−

1

[

NO

]

=

3.6 mol L

−

1

−−−−−−−−−−−−−−−−−

The answer is rounded to two sig figs.