Consider the following equilibrium:

4ko2(s) + 2h2o(g) 4koh(s) + 3o2(g)

which of the following is a correct equilibrium expression?

a.
`"k"_("eq") = (["koh"]^4["o"_2]^3)/(["ko"_2]^4["h "_2"o"]^2)`

b.
`"k"_("eq") = (["h"_2"o"]^2)/(["o"_2]^3)`

c.
`"k"_("eq") = (["ko"_2]^4["h"_2"o"]^2)/(["koh"]^4 ["o"_2]^3)`

d.
`"k"_("eq") = (["o"_2]^3)/(["h"_2"o"]^2)`

Answer is option D

Explanation:

The explanation is embedded in the word document attached

Keq= [KOH]^4 [O2]^3/[[KO2]^4

Explanation:

4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g)

Looking at the equation, the correct equilibrium expression is shown in the answer. The equilibrium constant for a reaction is given by the active masses of species involved in the reaction. The relative molar coefficients of species are raised to the power of their molar concentrations to give the active mass of each specie. This active mass now goes into the equilibrium equation.

Water is not included in the equilibrium equation because, as a solvent, it is present in large excess.

b. th3 n4zc4 pl4t3 15 c0nv3rg1ng w1th the s0uth 4m3ric4n pl4t3.

i believe the answer is a.