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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 = ?

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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.

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