Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq) + B(s) + 6H,0(1) - Fe(s) + H BO,) + 3 H,

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Calculate The Equilibrium Constant K For The Reaction Shown At 25 C Fe Aq B S 6h 0 1 Fe S H Bo 3 H 1 (19.13 KiB) Viewed 60 times

Calculate The Equilibrium Constant K For The Reaction Shown At 25 C Fe Aq B S 6h 0 1 Fe S H Bo 3 H 2 (10.7 KiB) Viewed 60 times

Calculate The Equilibrium Constant K For The Reaction Shown At 25 C Fe Aq B S 6h 0 1 Fe S H Bo 3 H 3 (39.21 KiB) Viewed 60 times

Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq) + B(s) + 6H,0(1) - Fe(s) + H BO,) + 3 H, 0+ (aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe+ (aq) + 3 e Fe(s) E* = -0.04 V H,BO,() + 3H, 0+ (aq) + 3c" —B(s) + 6H, O(1) E = -0.8698 V
Calculate the cell potential for the reaction as written at 25.00 °C, given that (Zn2+] = 0.864 M and [Sn2+] = 0.0100 M. Use the standard reduction potentials in this table. Zn(s) + Sn²+ (aq) = Zn2+ (aq)+Sn(s)
The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 5.63 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb + (aq). The Sb3+ (aq) is completely oxidized by 23.7 mL of a 0.135 M aqueous solution of KBro, (aq). The unbalanced equation for the reaction is BrO; (aq) + Sb)*(aq) - Br"(aq) + Sb** (aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ote. mass of antimony: 8 percentage of antimony: