Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co²+ (aq) + Cd(s) → Co(s) + Cd²+ (aq) Co2+ (aq) + 2e →Co(s) = -0.280 V Cd2+ (aq) +2e → Cd(s) F = -0.403 V red red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining than zero. greater

What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Ag(s) and Mn2+(aq) to give Ag+(aq) and Mn(s) Use the reduction potential values for Ag+(aq) of +0.80 V and for Mn2+(aq) of -1.18 V

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Cd²+ (aq) + Zn(s) → Cd(s) + Zn²+ (aq) AG⁰ = Cd2+ (aq) +2e → Cd(s) E red Zn²+ (aq) +2e → Zn(s) E red K for this reaction would be greater less = -0.403 V -0.763 V kJ than one.

Rank the following in increasing ability as oxidizing agents. The reduction potentials of all species are shown below. Cl, (g) + 2e → 2C1 (aq) E° = 1.3583 V Ag*(aq) + le Cu²+ (aq) + 2e¯ → Ag(s) E° = 0.7996 V → Cu(s) E° = 0.342 V Sn²+ (aq) + 2e → Sn(s) E° = - 0.136 V к"(ад) + 1е — → K(s) E° - 2.95 V 1st attempt

What is the equilibrium constant for the dissolution of copper (II) hydroxide: Cu(OH)₂ (s) Given the standard reduction potentials Cu(OH)₂ (aq) + e- → Cu (s) + OH¯ (aq) Cu²+ (aq) + e¯ →→ Cu (s) O 5.16 x 10^-9 O 1.63 x 10^3 O 1.93 x 10^8 O 6.12 x 10^-4 Cu²+ (aq) + OH¯ (aq) O 2.20 x 10^-20 EO = -0.15 V Eº = +0.34 V

Balance the following skeletal reaction in acidic solution. Be sure to include “1” in the blank if the coefficient is 1. Ag+(aq) +PbO(s) → PbO2(s) + Ag(s)

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Co²+ (aq) + Zn(s) → Co(s) + Zn²+ (aq) red Co²+ (aq) + 2e → Co(s) Ee Zn²+ (aq) + 2e¯ → Zn(s) Ee red AGO K for this reaction would be kJ = -0.280 V -0.763 V than one.

Using standard reduction electrode potentials, calculate standard free-energy change at 25°C for the following reaction:3Cu(s) + 2NO3-(aq) + 8H+(aq) → 3Cu2+(aq) + 2NO(g) + 4H2O(l).

Just the last one. And use table if needed

Use the standard reduction potentials given below to predict if a reaction will occur when Fe metal is put into a 1 M aqueous Cd²+ solution. Cd²+ red (aq) + 2e¯ → Cd(s) Ee Fe²+ (aq) + 2e → Fe(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) -0.403 V -0.440 V + +