Half-reaction E' (V) Cr* (aq) + 3e-- Cr (s) -0.74 Fe2 (aq) + 2e- - Fe (s) -0.440 Fe" (aq) +e- - Fe* (s) 3+ +0.771 Sn** (aq) + 2e- - Sn* (aq) +0.154 Part A The standard cell potential (EC) for the voltaic cell based on the reaction below is V. Sn2* (aq) + 2FE3* (aq) → 2Fe?* (aq) + Sn* (aq) O +0.46 O +1.21 O -0.46 O +0.617 O +1.39 Submit Request Answer

For the galvanic cell:            Zn(s)  +  2Tl+(aq)      2Tl(s)  +  Zn2+(aq)             Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq)  +  2e–      Zn(s)  is   Eored = –0.76 V What is the standard reduction potential for Tl+(aq)  +  e–      Tl(s)                  Eored = ? V   a. +0.17 V   b. –0.17 V   c. –0.34 V   d. +0.34 V

Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.

+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)

Calculațe Eo cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu2" (ag) + e Cu'(ag) + e Cu(s) Mno, (aq) + 8H"(aq) + 5e Mn?"(aq) + 4H,0 Fe (aq) + e – Fe? (aq) Cu*(aq) 0.153 0.521 1.507 0.771 Basic solution Zn(OH) (s) + 2e → Zn(s) + 40H (aq) Mno, (aq) + 2H,O + 3e MnO,(s) + 4OH(aq) -1.22 0.588

A galvanic cell using Cu"/Cu and Cu?+/Cu was set up at 293 K and the non-standard cell potential was determined to be 0.175 V. Determine the concentration of ions in the cathode's solution if the concentration at the anode is 0.7787 M: (cathode)(M) number (rtol=0.03, atol=1e-08)

Including the state of reaction (aq),(l),(g),etc Thank you