Kc is 1.67 x 10^20 at 25 °C for the formation of iron(III) oxalate complex ion:

Fe^3+ (aq) + 3C2O4^2- (aq) <--> [Fe(C204)3]^3- (aq)

Determine the number of moles of C2O4^2- used to react with 0.53 moles of Fe^3+.

In this case, according to the given information and chemical equation, it turns out possible for us to calculate the moles of C2O4^2- by firstly setting up the equilibrium expression:

[tex]Kc=\frac{[[Fe(C_2O_4)_3]^{3-}]}{[Fe^{3+}][C_2O_4^{2-}]^3}[/tex]

However, according to the question, we just need to apply the given 1:3 mole ratio in the chemical reaction, of iron (III) ions to oxalate ions to obtain:

[tex]n_{C_2O_4^{2-}}=0.53molFe^{3+}*\frac{3molC_2O_4^{2-}}{1molFe^{3+}}=1.59mol C_2O_4^{2-}[/tex]

Regards!

Kc is 1.67 x 10^20 at 25 °C for the formation of iron(III) oxalate complex ion: Fe^3+ (aq) + 3C2O4^2- (aq) <--> [Fe(C204)3]^3- (aq) Determine the number of moles of C2O4^2- used to react with 0.53 moles of Fe^3+.

Respuesta :

Otras preguntas

Kc is 1.67 x 10^20 at 25 °C for the formation of iron(III) oxalate complex ion:

Fe^3+ (aq) + 3C2O4^2- (aq) <--> [Fe(C204)3]^3- (aq)

Determine the number of moles of C2O4^2- used to react with 0.53 moles of Fe^3+.