In the table of standard reduction potentials, locate the half-reactions for the reductions of the following metal ions to the metal: Sn^+2 (aq), Au^+ (aq), Zn^2+ (aq), Co^2+ (aq), Ag^+ (aq), and Cu^2+ (aq). Among the metal ions and metal that make up these half reactions: a. Which metal ion is the weakest oxidizing agent? b. Which metal ion is the strongest oxidizing agent? c. Which metal ion is the strongest reducing agent? d. Which metal ion is the weakest reducing agent? e. Will Sn(s) reduce Cu^2+(aq) to Cu(s)? f. Will Ag(s) reduce Co^2+ (aq) to Co(s)? g. Which metal ion on the list can be reduce by Sn(s)? h. What metals can be oxidized by Ag^+(aq)?

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X

› Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au³ +(aq) + 3 Ni(s) = 2 Au(s) + 3 Ni² + (aq) AGⓇ = kJ

A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: Cr(s) + 3 Ag*(aq) → Cr³*(aq) + 3 Ag(s) Which of the multiple choices correctly describes how the cell emf changes when a change is made to the cell? Ca) Adding water to the anode compartment makes the cell emf less positive. C b) Increasing the size of the silver electrode makes the cell emf stay the same. C C) Adding a solution of 1.0 M AGNO, to the cathode compartment makes the cell emf more negative. C d) Adding Na,s to the anode compartment to precipitate chromium sulfide makes the cell emf less positive. Ce) Adding a solution of 5 M Ag* to the cathode compartment makes the cell emf stay the same.

5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.

Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. 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.) +

A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12

Consider a cell that uses the redox reaction: Cu2+ (aq) + Zn (s) → Zn2+ (aq) + Cu (s).   The standard reduction potentials for the two half reactions that make up this cell are shown below. A potentiometer is used to measure the potential difference between two half cells. What is the reading on the potentiometer when [Cu2+] = 0.010 M and [Zn2+] = 0.10 M.  Cathode: Cu2+(aq) + 2e- → Cu(s)       E° = 0.34 V Anode:    Zn2+(aq) + 2e- → Zn(s)        E° = -0.76 V     1.10 V     1.04 V     1.07 V     1.13 V

Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V 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 | than zero.

Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=