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.

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

it's all four options.