K_c is 1.67 times 10^20 at 25 degree C for the formation of iron(III) oxalate co

Question

K_c is 1.67 times 10^20 at 25 degree C for the formation of iron(III) oxalate complex ion: Fe^3+ (aq) + 3 C_2 O_4^2- (aq) leftrightarrow [Fe(C_2 O_4)_3]^3- (aq). If 0.0800 M Fe^3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe^3+ ion at equilibrium? K_c is 1.67 times 10^20 at 25 degree C for the formation of iron(III) oxalate complex ion: Fe^3+ (aq) + 3 C_2O_4^2- (aq) leftrightarrow [Fe (C_2O_4)_3]^3- (aq). If 0.0800 M Fe^3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe^3+ ion at equilibrium? 1.97 times 10^21 M 2.09 times 10^19 M 1.09 times 10^-21 M 0.0100 M Consider the reaction. NiO(s) + CO(g) Ni(s) + CO_2(g) Kc = 4.0 times 10_3 (at 1500 K) If a mixture of solid nickel(II) oxide and 0.10 M carbon monoxide comes to equilibrium at 1500 K, what is the equilibrium concentration of CO2? Express your answer using two significant figures.

Explanation / Answer

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

Kc = [Fe(C2O4)3]/ [Fe^3+] [C2O4]^3

Kc is very large so that all the Fe^3+ will be converted to the product. Conce ntration of Fe(Ox)3 =0.08 M

[C2O4] = 1.00 M - 3*0.08 M = 0.76 M

concentration of Fe^3+ is very small and we will assume it to be x

Kc = 0.08 /x * (0.76)^3

6.7 *10^20 = 0.08 /x * (0.76)^3

or, x =1.09*10^-20 M

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