contestada

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)`

Respuesta :

quasarJose

Answer:

Answer is option D

Explanation:

The explanation is embedded in the word document attached

Ver imagen quasarJose
pstnonsonjoku

Answer:

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.

Otras preguntas