Question

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇋ 2NO2(g) Kc = 1.46 5N2O4(g) ⇋ 10NO2(g) Kc = ?

Answer 1

Answer:- Kc = 6.63

Solution:- First given equation is:

`N_2O_4(g)\rightleftharpoons 2NO_2(g)`

The equilibrium expression for this equation is written as:

`Kc=([NO_2]^2)/([N_2O_4])`

The second given equation is:

`5N_2O_4(g)\rightleftharpoons 10NO_2(g)`

The equilibrium expression for this equation is written as:

`Kc^'=([NO_2]^1^0)/([N_2O_4]^5)`

Comparing these two expressions, to get this second expression from the first one, we need to do the fifth power of first equilibrium expression.

Hence,
`Kc^'=(Kc)^5`

Plug in the value of Kc in it from first expression,
`Kc^'=(1.46)^5`

`Kc^'` = 6.63

So, the Kc of second equation is 6.63.