QUESTION 7 Consider the following reduction potentials and answer the questions that follow: Mn04 (ag) +8 H (aq) +5 eMn" (aq) + 4 H20 (1) °- 1.51 V Zn2+ (aq) + 2e - Zn (s) e°--0.76 V How will the pH of the solution in the manganese compartment change as the cell runs?

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Ni

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V

Examine the following half-reactions and select the strongest reducing agent among the species listed.      AuBr4(aq) + 3e– → Au(s) + 4Br–(aq)                           E° = 0.854 V      Mn2+(aq) + 2e– → Mn(s)                                             E° = –1.185 V      K+(aq) + e– → K(s)                                                       E° = –2.931 V      F2O(aq) + 2H+(aq) + 4e– → 2F–(aq) + H2O(l)           E° = 2.153 V Group of answer choices K K+ F2O F–

half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V red MnO, (aq)+2 H,0(1)+3e MnO,(5)+4 OH (aq) E° =+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If said it was you possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.

Consider the following two half-reactions and their standard reduction potentials. N2(g) +H,0(1) E° = 1.766 V MnO, (s) + 2H,0(1) E° = 1.673 V N,0(g) + 2H*(aq) + 2e¯ → MnO,(aq) + 4H*(aq)+3e¯ 1st attempt l See Calculate E°for the spontaneous redox reaction that occurs when these two half-reactions are coupled. V

Draw a diagram for the following standard cell Ag(s) I Ag (aq) Il Cu²+ (aq) I Cu(s) Label the following: (i) (ii) (iii) (iv) Electrodes; cathode or anode; positive or negative Electrolytes Direction of electron flow Direction of ion movement

1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential 2) Calculate the free energy change and the cell potential for the reaction at 298.0 K if all reactants are at 2.00 M and/or 2.00 atm and all products are at 0.0100 M and/or 0.0100 atm

What is the potential at 25 ° C of a cell made up of the semi-cells Zn / Zn²- and Cu / Cu²- where [Zn² -] = 0.25 M and [Cu²-] = 0.15 M? Standard reduction potentials at 25 ° C