Consider the following half-reactions: Ag*(aq) + e¯ → Ag(s) Cu2*(aq) + 2 e¯ → Cu(s) Pb2*(aq) + 2 e¯ → Pb(s) Fe2+(aq) + 2 e→ Fe(s) Al3*(aq) + 3 e¯ E° = +0.80 V E° = +0.34 V E° = -0.13 V E° = -0.44 V → Al(s) E° = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)? O Cu2*(aq) and Fe2*(aq) Fe(s) and Al(s) O Ag*(aq) and Cu2+(ag) O Fe2*(aq) and A13*(aq) O Ag(s) and Cu(s)

Identify the strongest reducing agent based on the following half- reactions. 2+ +1.22 V → Mn (aq) + 2H₂O(1) +0.61 V MnO₂(s) + 4H* (aq) + 2e- Hg₂SO4(s) + 2e → 2Hg(1) + SO4 (aq) SnO₂(s) + 2H₂O0+ 4e → Sn(s) + 4OH(aq) Cr(OH)3(s) + 3e → Cr(s) + 3OH(aq) -0.95 V -1.48 V Cr Mn02 Hg2SO4 Sn Hg

7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.

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

Consider the following half-reactions.   Cl2(g) + 2 e– → 2 Cl–(aq) E° = +1.36 V   Ag+(aq) + e– → Ag(s) E° = +0.80 V   Cu2+(aq) + 2 e– → Cu(s) E° = +0.34 V   Sn2+(aq) + 2 e– → Sn(s) E° = –0.14 V   Al3+(aq) + 3 e– → Al(s) E° = –1.66 V Which of the following species will reduce Cu2+(aq) ion? Ag(s) and Sn^2+(aq) Cl^-(aq) and Ag(s) Cl2(g) and Ag^+(aq) Sn(s) and Al(s) Sn^2+(aq) and Al^3+(aq)

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: (aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq) AG° Pb²+ = Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V red 2+ Cu²+ (aq) + e → Cu+ (aq) Fº red kJ K for this reaction would be = = 0.153 V + than one.

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 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)

Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?

Using data in the Table, what is the equilibrium constant for the reaction: 2Fe 3+(aq)+H 2(g) 2Fe 2+(aq) + 2H +(aq)?

A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V).The button form of this cell is used in watches, hearing aids, and other electronic devices.The half-reactions are:Zn(s) + 2OH- (aq) → Zn(OH)2(s) + 2e￾Ag2O(s) + H2O(l) + 2e- → 2Ag(s) + 2OH(aq)(a) Identify the anode and the cathode reactions.(b) What’s the overall reaction in this galvanic cell?