For each electrochemical cell, calculate the cell voltage using the table of standard reduction potentials linked in the instructions and indicate whether or not the reaction is spontaneous.(a) Zn2+(aq) + Pb(s) → Zn(s) + Pb2+(aq) VIs this reaction spontaneous as written?yesno    (b) 2Cu(s) + Br2(l) → 2Br-(aq) + 2Cu+(aq) VIs this reaction spontaneous as written?yesno    (c) 2Au(s) + 3MnO2(s) + 12H+(aq) → 2Au3+(aq) + 6H2O(l) + 3Mn2+(aq) V

Which one is the correct condition for spontaneous reaction in an electrochemical cell(a) L1Gr,p < 0, EcelJ > 0;(c) L1Gr,v < 0, EcelJ < 0;(b) L1Gr,p > 0, EcelJ < 0(d) L1Gr,p = 0, EcelJ = 0

In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses.Zn(s)|Zn2+(aq)||H+(aq)|H2(g)|Pt(s) Question 2Select one or more:Eºcell is negativeZn/Zn2+ is the anodeZn/Zn2+ is the cathodeEºcell is positiveH+/H2 is the cathodeH+/H2 is the anode

The cell potential of an electrochemical cell is positive. What does that tell you about the redox reaction?A.The reduction part of the reaction occurs at the anode.B.The oxidation part of the reaction occurs at the cathode.C.The reaction is spontaneous.D.The reaction is nonspontaneous.

III. Solve all the following problems.1. Which of the following reactions are spontaneous at standard state? (Consult table ofelectrode potentials.) A) I2 + 2 Fe2+ 2 I + 2 Fe3+ B) 8 H+ + 2 NO3 + 3 Cu(s) 2 NO(g) + 3 Cu2++ 4 H2O C) 4 MnO4 + 12 H+ 4 Mn2+ + 5 O2 + 6 H2O D) Cu(s) + Cl2(g) Cu2+(aq) + 2 Cl(aq)2. A standard electrode X when coupled with a standard H2 electrode to make a cell gives a cellvoltage of 0.34. What is the potential of the standard electrode X?3. How much time is required to plate a 0.01 mm thick layer of Cr on an object whose area is200 cm2 if the current used is 1.00 A and the density of Cr is 7.1 g/cm3?4. The same quantity of electricity that caused 10.0 g of Ag to plate out from a solution ofAgNO3 is passed through a solution of CuSO4. How much Cu will plate out?5. A current of 0.01 A is passed through a solution of iridium bromide. The only reaction at thecathode is the deposition of Ir. After 3.00 hr, 0.072 g of Ir has been deposited. What is thecharge on the iridium ion?6. A. Calculate the potential of the cell where the reaction: 2 HClO2 HClO + ClO3 + H+ occursif: [HClO2] = 0.01 M; [HClO] = 0.10 M; [ClO3] = 0.10 M and pH = 5.0 B. Taking all species to be1 M except HClO2, calculate the concentration of HClO2 at which the reaction would no longerbe spontaneous.7. Show that the oxidation of Cl to Cl2(g) by Cr2O72 in acidic solution will NOT occur withreactants and products in their standard states. If, however, this method is to be used for theproduction of Cl2 in the laboratory, how would you go about it?8. Design a cell that will enable you to measure the Ksp of PbCl2.9. A compound contains 21.35 % Cr, 28.70 % N, 6.209 % H and 43.68 % Cl by mass. (a) Itdoes not react with HCl. (b) On reaction with AgNO3, it gives 2 moles of AgCl per mole of thecompound. (c) It has an electrical conductivity corresponding to 3 moles of ions per mol ofcompound. A) Give the inferences of (a), (b) and (c). B) Write the formula and give the name ofthe compound.10. Explain why [Fe(CN)6]3 is poisonous while [Fe(CN)6]4 is not.11. Describe how the diamagnetic behavior of [Co(en)3]3+ is explained by: A) Valence BondTheory B) Crystal–Field Theory12. A certain coordination compound has the simplest formula PtN2H6Cl2. It has a molar massof about 600 g and contains both a complex cation and a complex anion. What is its structure?13. When Cr2+ is linked with a strong–field ligand to produce an octahedral complex, the ionhas two unpaired electrons. When it is linked with a weak–field ligand, the ion has four unpairedelectrons. In contrast, the complex resulting from Cr3+ always has three unpaired electronsregardless of the nature of the ligand. Explain.14. Draw a structure to represent the complex ion, [Co(en)3]3+.15. When 6.0 M NaOH solution is added to a solution containing equimolar concentrations ofCd(NO3)2 and Zn(NO3)2, the precipitate that first forms contains both Zn and Cd. However,upon the addition of an additional base with stirring, part of the precipitate dissolves. Theundissolved precipitate contains Cd but no Zn. Describe what happened in terms of net ionicequations.

The half-reaction at the cathode in an electrochemical cell is given below. What other half-reaction would most likely occur at the anode to produce a spontaneous reaction?Zn2+(aq) + 2e- Zn(s)Click for a reduction potential chartA.H2(g) 2H+(aq) + 2e-B.K+(aq) + e- K(s)C.Al(s) Al3+(aq) + 3e-D.Zn(s) Zn2+(aq) + 2e-