Question

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
Answer: C,

Answer 1

the value of the missing equilibrium constant is E. 7.30
Solution:
N2O4(g) ⇌ 2 NO2(g) Kc = 1.46
5 N2O4(g) ⇌ 10 NO2(g) Kc =?

If 1 atom of N2O4(g) is 1.46
So to get 5 atoms of N2O4(g), you will simply multiply it by 5.

1.46 x 5 = 7.30

Answer 2

The answer is C) 6.63

Step-by-step 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