The equilibrium constant is given for one of the reactions below. determine the value of the missing equilibrium constant. n2o4(g) ⇌ 2 no2(g) kc = 1.46 5 n2o4(g) ⇌ 10 no2(g) kc = ? a) 1.46 b) 0.292 c) 6.63 d) 1.08 e) 7.30 c,

The answer is C) 6.63

Explanation:

When the coefficients in a balanced equation are multiplied by a factor, the resulting equilibrium constant is raised to this factor.

In this case, you have the following equilibrium:

N₂O₄(g) ⇌ 2 NO₂(g) Kc = 1.46

In which the coefficients are 1 (for N₂O₄) and 2 (for NO₂)

In the second equation, notice that you have the coefficients of the first equation multiplied by 5 (1 x 5= 5 for N₂O₄; 2 x 5= 10 for NO₂) :

5 N₂O₄(g) ⇌ 10 NO₂(g)

Thus, to obtain the equilibrium constant of the second equation (Kc'), you have to raise the first equilibrium constant (Kc) to 5:

K'c= (Kc)⁵= (1.46)⁵= 6.63