HALF-REACTION E° (V) HCIO, + 2H,O* + 2e – HCIO + 3H;O +1.628 Co+ +e- Co+ (2 mol // H,SO,) +1.83 First reduction half-reaction: E° red value of first half-reaction: Second reduction half-reaction: E° red value of second half-reaction: Oxidation half-reaction: E° ox: Reduction half-reaction: E° red: Balanced overall equation: E° cell: n value (moles e-): What metal is the anode electrode? What metal is the cathode electrode? AG° value (show set-up and calculation): K value (show set-up and calculation)

Window Help 5% C Su A cvg.cengagenow.com ontent GRLContent Netflix Favorites My Home My Home My Home Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Fe"(aq) + H2(g) Fe(s) + 2H (aq) Answer: kJ K for this reaction would be than one. 團

2. For the following half-reactions, answer the questions below. Co* + e → Co2 ɛ° = +1.95 V Ag* + e → Ag ɛ° = +0.80 V I2(ag) + 2e → 21 8° = +0.53 V Ni*2 + 2e → Ni 8° = -0.24 V Cd*2 + 2e → Cd ɛ° = -0.40 V a. Which of the species listed is the strongest reducing agent? b. Which of the species listed is the strongest oxidizing agent? c. Which of the species listed is the weakest oxidizing agent? d. Which of the species listed can be reduced by nickel? e. Which of the species listed can be oxidized by iodine? f. Write the balanced net ionic equation for the reaction that describes silver being oxidized by cobalt (III). g. If the reaction in (f) were carried out in a galvanic cell, what metal electrodes would be used at the anode and cathode? ANODE CATHODE h. Write the standard line notation for the silver-cobalt (III) reaction in (f).

Given the following two standard reduction half-reaction calculate what the standard cell potential (E°) in volts. Report you answer to 3 decimal places. Cr207 (aq) +14H (aq) + 7H,O, (E*red = 1.33 V) 2- + 6e 2Cr3+ (aq) H2O2 02 + 2H+ + 2e- (E°red = -0.682 V)