Question 7 (1 point) Saved Consider these metal ion/metal standard reduction potentials Cu2(aq)|Cu(s) Ag+1(aq)|Ag(s) Co2(aq)|Co(s) Zn+2(aq)]Zn(s) +0.34 +0.80 V -0.28 V -0.76 V Based on the data above, which one of the species below is the best oxidizing agent? 0 1 Cols) O2) Zn(s) 3) Cutlaq) 04) Culs) 5) Ag+h(aq)
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Which metal is being oxidized? [Select] Which metal is being reduced? (Select] Identify and label the anode and cathode. anode (Select] cathode (Select] Salt bridge is made with potassium nitrate, show ion flow. [Select] Which electrode decreases in mass during cell operation? [Select] In which direction do electrons flow in the external circuit? [Select] At which electrode are electrons generated? [Select]
-6. Calculate the AG for the cell, Ag | Ag+! || Cut? Cu Aggit Cu2+ -> Curst Agron 064.980 Till 77.11-64.98 89.285 AG=128360
Which ion had the greatest tendency to oxidize a metal sample? Which ion had the least tendency to oxidize a metal sample?
1. What is E° for the reaction Cu+ + Ag+ → Cu2+ + Ag ? 2. What is the standard cell potential at 298K for the reaction: 2IO3- + 2H+ + 5H2O2→ I2 + 5O2 + 6H2O 3. Will Cu react with 1M HCl?
Part C. Effect of Concentration on Cell Potentials • Ecall for the Cu(s). Cu2+||Ag*, Ag(s) system: 0.450 V 0,851 v • Ecate for the Cu(s). Cu2+||Ag, Ag(s) system after the addition of 6M NH: • Write the balanced redox reaction for the entire cell: • • How many electrons are transferred? Use the Nernst Equation (given below) to calculate the concentration of Cu left in the solution Een = Ecen (0:0257) in (1960 [Cu2+] =
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s) Eo= 0.8V If you increase the concentration of Cu2+(aq), which of the following would be true about the cell potential E? It would remain constant It would increase It would decrease This cannot be determined
Compare the potentials between the Ag/Ag+ and Cu/Cu2+ half cells before and after adding excess NH3 to the Cu/Cu2+ half cell. Did the potential increase or decrease? Explain the result in terms of the Nernst equation.
The concentration of Cu2+ ion in a sample of spring water is 5.3 ppm. What mass of Cu2+ ion is present in 6.5 L of this pring water, which has a density of 1.00 g/mL? O 2.6 g 0 0.068 g O 0.034 g O 0.34 g