5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ), how many coulombs of charge must have been transferred from V2+ to Fe3+ ? Given Faraday constant F = 96490 C/mol e-  , A.W.Fe  = 55.85 g/mol.       how many seconds must have been passed if a constant electric current 1.5 amperes were maintained?

1.Which of the following is the correct cell representation of the reaction: MnO4-(aq) + 5Fe2+(aq) + 8H+(aq) ---> Mn2+(aq) + 5Fe3+(aq) + 4H2O (l) a.Fe|Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq)|Ptb.Pt|Mn2+(aq), MnO4-(aq)||Fe3+(aq), Fe2+(aq)|Ptc.Pt|Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq)|Ptd. Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq) 2. To make the synthesis of ATP from ADP spontaneous, which reaction is coupled with the following nonspontaneous reaction? ADP → ATP  ΔG°’= 30.5 kJ mol-1 a.fructose-1,6-bisphosphate → fructose-6-phosphate (ΔG°’ = -16.7 kJ mol-1) b.glucose 6-phosphate → glucose (ΔG°’ = -13.8 kJ mol-1) c.glucose-6-phosphate → fructose-6-phosphate (ΔG°’ = +1.67 kJ mol-1) d.phosphoenolpyruvate → pyruvate (ΔG°’ = -61.9 kJ mol-1)3. Consider the dissolution of NH4NO3:  NH4NO3(s) ---> NH4+ + NO3- (aq)                 ΔHrxn = 25 kJ/mol Which of the following is true regarding the spontaneity of the reaction? a.The reaction is spontaneous at high temperature only…

6. Consider the following galvanic cell: Ag- shown: 1.00 M Ag 1.00 M Cd2+ A 15.0-mole sample of NH3 is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as Ag+ (aq) + NH3(aq) AgNH3+ (aq) K₁ 2.1 x 10³ = AgNH3+ (aq) + NH3(aq) ⇒ Ag(NH3)2+(aq) K₂ = 8.2 x 10³ Calculate the cell potential after the addition of 15.0 moles of NH3.

For the cell diagram below, what is the equilibrium constant K for the reaction at 25 °C? * Pt(s) | [Fe(bpy),2*(aq), [Fe(bpy),]3"(aq) || S,0, (aq), So,2 (aq) | Pt(s) E° ([Fe(bpy),]3*/[Fe(bpy);]*) = +1.12 V E° (S,0, /SO,2) = +2.01 V O 8.54 x 1018 O 8.93 x 107 O 1.22 x 1030 O insufficient data

The reaction Cr(NH3)6*(aq) + 3en(aq) --> Cr(en)3+*(aq) + 6 NH3(aq)where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction. the reaction is spontaneous for all temperatures. the reaction is spontaneous for low temperatures. the reaction is non-spontaneous for all temperatures. the reaction is spontaneous for high temperatures. not enough info to tell.

3. (a) b C. d. e. f. Given 0.01 Molar concentration Au³+ ion and 0.01 molar of Ag+ ion, and the following reaction: or Au³(aq) Ag+ (aq) -→ Au (s) -→ Ag (s) Write the balanced oxidation reduction equation for the cell E° = 1.52 V Eº = 0.80 V Which specie is being oxidized Which Specie is at the anode? Which Specie is the oxidizing agent? Which specie lost electron/s? Which specie saw an increase in oxidation state? Calculate the Ecell at non-standard condition for the reaction

Open with Calculate ECELL and indicate whether the cell is galvanic or electrolytic. 8. Zn | 0.0364 M Zn+2 || 6.09 x 10-3 M T1+3, 0.0620 M TI+| Pt 9. Cu | 0.0601 M Cu+2 || 0.1350 M I-, AgI(s)| Ag 10. Pt, 1.00 atm H2 | 0.438 M NH3, 0.379 M NH4+ || SHE

11. Consider the following reaction and its AG-AG• at 25.00 °C. 12 Coeside 2Ag*(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG =-88660 J/mol a. Calculate the standard cell potential, Ecellº, for the reaction. b. Calculate the equilibrium constant, K, for the reaction. Wtoxided what is reduced? CLEAREY

Give detailed Solution..don't give Handwritten answer

Calculate the EMF of the following electrochemical cell: Pt | VO2+(0.25 M), V3+(0.10 M), H+ (0.001 M) || TI3+ (0.10 M), TI+(0.05 M), | Pt Indicate whether the cell is galvanic or electrolytic. Evo2+/v3+ = 0.361 V, ET³+/T+ = 1.25 V   Ans: 1.23 V, galvanic