At 298 K, the standard electrode potentials of Mg2+/Mg, Ni2+/Ni, Cu2+/Cu and Au3+/Au are –2.36 V, –0.25 V, 0.34 V and 1.40 V respectivelyOn the basis of standard electrode potential, predict which of the following reactions can occur?

the standard electrode reduction potentials of Zn and Ag and Cu are -0.76 , 0.80 and 0.34 volt respectively then

What is the standard cell potential of a cell made of theoretical metals Ma/Ma and Mb/Mb if the reduction potentials are –0.19 V and –0.85 V, respectively?Group of answer choices+1.04 V+0.66 V–1.04 V–0.66 V

1°) Balance the following equations. Préciser les changements de nombre d’oxydation des éléments concernés. a) N2H4 + IO3-  N2 + I- b) Cr2072- + H2C2O4  Cr3+ + CO2 (acid medium) c) MnO4- + I-  MnO42- + IO3- d) NO3- + HS-  NO2- + S 2°) Calculate the potential of each of the following electrodes with respect to NHE at 25°C: - Cupper bare in 10-3 M Cu2SO4 an aqueous solution - Platinum bare in 10-2 M FeSO4 + 2 x 10-3 M Fe2(SO4)3 aqueous solution ; - Silver plate 0,5 M aqueous solution saturated with AgCl (Ks = ; 3°) How much is the apparent standard potential equal in acid buffered solution of pH = 2 for Cr2O72-/Cr3+couple ? E0(Cu+/Cu) = 0.52 V ; E0(Fe3+/ Fe2+) = 0.77 V ; E0(Ag+/Ag) = 0.80 V

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.

These NiCad batteries each have a potential of 1.75 V.The two half reactions occurring are:2Ni(OH)3(s) + 2e- 2Ni(OH)2(s) + 2OH-(aq)Cd(s) + 2OH-(aq) Cd(OH)2(s) + 2e-Which statement is incorrect:Select one:a.Cadmium forms the anode.b.Nickel metal is not involved in the reaction.c.The cadmium becomes eroded as the battery is used.d.The nett battery reaction involves only solid substances.e.The cadmium electrode has the more positive potential.