Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)3(s) + 3e-Cr(s) + 3OH-(aq) SnO₂(s) + 2H₂O(l) + 4e¯ ⇒ Sn(s) + 40H-(aq) MnO₂(s) + 4H+ (aq) + 2e- ⇒ Mn²+ (aq) + 2H₂O(l) Hg2SO4(s) + 2e-2Hg(/) + SO4²-(aq) A) Cr(s) B) OH-(aq) C) Sn(s) D) Hg(/) E) Mn²+ (aq) E° = -1.48 V E° = -0.945 V E° = 1.224 V E° = 0.613 V

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.

Balance the following redox reaction in acidic solution. 2+ Fe²+ (aq) + MnO₂(s) ->> 3+ 2+ Fe (aq) +Mn (aq)

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–

Given the following2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq)         E°cell = 0.73 V and AgCl(s) → Ag(s) + Cl-(aq)          E°= 0.222 V What is the standard reduction potential for X2+(aq)?

Calculate the equilibrium constant for each of the reactions at 25 ∘C .2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)

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

Consider these two entries from a fictional table of standard reduction potentials. X+ (aq) + e¯ Y+ (aq) + e- →Y(s) E = 2.01 V →X(s) O X and Y O X+ and Y+ O X and Y+ O X+ and Y E = 2.62 V Which pair of species will react under standard conditions at 25 °C?