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1-3 I. Cus)+AgNOga) 1. II II. I. Pb)Cu(NO)2() 2. II. II teor n I. Zn)+Pb(NO)2a) 3....
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
For each of the following assign oxidation numbers to the individual elements: 1) Zn+Pb(NO3)2= Zn (NO3)2+Pb 2) Mg+ H2SO4= MgSO4+H2 3) 2 Zn+ 2 HCl=2 ZnCl2+ H2 4) Cu (NO3)2+2 Zn= Cu+ 2NO3
Circle the stronger oxidizing agent in each pair? Zn^2+ or Pb^2+ Cu^2+ or Ag^+ Ni^2+ or Cd^2+ Ni^2+ or Cu^2+ Circle the species that is easier to oxidize in each pair. Cu or Ag Pb or Zn Ni or Pb Cd or Ni a. Circle the reaction that will occur spontaneously. NiSO_4(aq) + Al_(s) Ni_(s) + Al_2((SO_4)_3(aq)
10. Given a Galvanic cell Zn(s) I zs. I cu-l cus) the right-hand side of this notation represents the A. The spontaneous nait ot the reaction B. The reduction half-reaction C. The oxidation half-reaction D. The anode side of the cell E. You cannot split up the cell; everything works together
1 Zno Zn2+ con +2 é "Cu 2+ hog) + 2 é Cuica) Znas + Cut 2 hout Cus FE 0.34 F. E: -0.76 21 2nw + Zn Zon + 2 é TF + 26 Few Znow & Fell Zarag, "Fels) E": - Full 3) Few Fearot 20 the Luc Few + 20249) ► Fehling) * Cu E = 0.45 v E: 0.34 Elan I
ORGANOMETALLIC REACTIONS CH2l2, Zn(Cu) ether N. CHa2, Zn(Cu) ether CHała Zn(Cu) ether CH212, Zn(Cu) ether CHzz Zn(Cu) ether CH22, Zn(Cu) ether R. 1 ether NaNH2, NH3 NaNH2, NH3 NaNH2, NH3 T. 1 ether U. 1 ether 〇2.Hor NaNH2, NH3 1 ether W. 2. H3O NaNH2, NH3 1 ether 2. H3O 1 ether x. NaNH2, NH3 Y. NaNH2, NH3 1 ether
Part A Calculate the voltage of the following cell: Zn I Zn(2+} (0.05 M) II Cu2+} (0.25 M) | Cu ν ΑΣφ V Submit Request Answer
(2) Zn (3) Pb (4) CU - Ag 6. On the basis of the reactions observed in the six test tubes, explain why the position of hydrogen cannot be fixed exactly with respect to all of the other elements listed in the activity series in Question 5. 7. What additional tests) would be needed to establish the exact position of hydrogen in the activity series of the elements listed in Question 5? 8. On the basis of the evidence developed...
EXPERIMENT 1: List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you expect given electrochemical cell to be spontaneous or nonspontaneous? Explain your answer. Pb|Pb(NO3)2||Zn|Zn(NO3)2 EXPERIMENT 1: What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL? EXPERIMENT 1: Calculate the theoretical standard cell potential for the electrochemical cell that includes the reaction. Mn+Pb2+⟶Mn2++Pb The standard reduction potentials for each half reaction are...
For each of the following provide: i) The phases present ii) The composition of each phase iii) The relative wt% of each phase a) 15 wt% Sn-85 wt% Pb at 100°C b) 1.25 kg Sn and 1.4 kg Pb at 200oC c) 55 wt% Zn-45 wt% Cu at 600 °C d) 1.88 kg Cu and 2.12 kg Zn at 500°C e) 21.7 mol Mg and 35.4 mol Pb at 350°C
For each of the following provide: i) The phases present...