Answer:
See full explanation.
Explanation:
Hello.
In this case, since we apply the law of mass action in order to write the equilibrium expression for each chemical reaction, we proceed as follows:
a. The reaction is:
[tex]2COF_2(g)\rightleftharpoons CO_2(g)+CF_4(g)[/tex]
And the equilibrium expression:
[tex]Kc=\frac{[CO_2][CF_4]}{[COF_2]^2}[/tex]
Since all the species are in gaseous phase they are included on the equilibrium expression.
b. The reaction is:
[tex]Cu(s)+Ag^+(aq)\rightleftharpoons Ag(s)+Cu^{2+}(aq)[/tex]
And the equilibrium expression:
[tex]Kc=\frac{Cu^{2+}}{Ag^+}[/tex]
Since only copper (II) ions and silver (I) ions are in aqueous phase.
c. The reaction is redox and it turns out:
[tex](S_2O_8)^{2-}+Fe^{2+}\rightleftharpoons Fe^{3+}+(SO_4)^{2-}\\\\S_2^{7+}+2e^-\rightarrow 2S^{6+}\\\\2\times (Fe^{2+}\rightarrow Fe^{3+}+1e^-)\\\\\\(S_2O_8)^{2-}(aq)+2Fe^{2+}(aq)\rightleftharpoons 2Fe^{3+}(aq)+2(SO_4)^{2-}(aq)[/tex]
And the equilibrium expression:
[tex]Kc=\frac{[Fe^{3+}]^2[(SO_4)^{2-}]^2}{[(S_2O_8)^{2-}][Fe^{2+}]^2}[/tex]
Since all the species are in aqueous phase.
