Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g), Kc=6.30 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium?

Question

contestada

Respuesta :

Аноним Аноним · Answer 1 · 2020-02-27T09:33:54+01:00

Answer: The equilibrium concentration of [tex]COF_2[/tex] is 0.332 M

Explanation:

We are given:

Initial concentration of [tex]COF_2[/tex] = 2.00 M

The given chemical equation follows:

[tex]2COF_2(g)\rightleftharpoons CO_2(g)+CF_4(g)[/tex]

Initial: 2.00

At eqllm: 2.00-2x x x

The expression of [tex]K_c[/tex] for above equation follows:

[tex]K_c=\frac{[CO_2][CF_4]}{[COF_2]^2}[/tex]

We are given:

[tex]K_c=6.30[/tex]

Putting values in above expression, we get:

[tex]6.30=\frac{x\times x}{(2.00-2x)^2}\\\\x=0.834,1.25[/tex]

Neglecting the value of x = 1.25 because equilibrium concentration of the reactant will becomes negative, which is not possible

So, equilibrium concentration of [tex]COF_2=(2.00-2x)=[2.00-(2\times 0.834)]=0.332M[/tex]

Hence, the equilibrium concentration of [tex]COF_2[/tex] is 0.332 M