The Edison accumulator is symbolized by:Fe(s) FeO(s) |KOH(aq, a) ||Ni2O3(s) |NiO(s) |Ni(s)Where half-stack reactions are:NizO3(s) + H2O(1) + 2e → 2NIO) + 20H',FeO(s) + H20(1) + 2e Fes) + 20H',$° = 0,45 VO° = -0,90 Va) What is the overall reaction of the stack?b) What is the. standard electrical potential of the battery,E°?

Galvanic cell are the cells which are used to convert chemical energy into electric energy . And…

The Edison accumulator is symbolized by: Fe(s)FeO(s) |KOH(aq, a) ||Ni2O3(s) |NiO(s) |Ni(s) Where half-stack reactions are: NizO3(s) + H20(1) + 2e 2NIO19) + 20H, FeO + H¿O(I) + 2e' Fes) + 20H, $° = 0,45 V 0° = -0,90 V a) What is the overall reaction of the stack? b) What is the. standard electrical potential of the battery, E°?

The Edison accumulator is symbolized by: Fe(s)FeO(s) |KOH(aq, a) ||Ni2O3(s) |NiO(s) |Ni(s) Where half-stack reactions are: NizO3(s) + H20(1) + 2e 2NIO19) + 20H, FeO + H¿O(I) + 2e' Fes) + 20H, $° = 0,45 V 0° = -0,90 V a) What is the overall reaction of the stack? b) What is the. standard electrical potential of the battery, E°?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

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Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Parágrafo Estilos The Edison accumulator is symbolized by: Fe(s) FeO(s) |KOH(aq, a) ||Ni2O3(s) |NiO(s) [Ni(s) Where half-stack reactions are: NizO3(s) + H20(1) + 2e 2NIO9 + 20H', FeOs) + H2O(1) + 2e → Fes) + 2OH', $° = 0,45 V 0° = -0,90 V a) What is the overall reaction of the stack? b) What is the standard electrical potential of the battery, E°?
An electrochemical cell consists of a Pt|H+ (aq,1.00 M)|H₂(g) cathode connected to a Pt|H+ (aq)|H₂(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.181 M), mixed with its conjugate base, A (0.157 M). The measured cell voltage is Eºcell = 0.258 V at 25 °C, with PH₂ = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. Submit Answer Retry Entire Group pH = K₂ = 9 more group attempts remaining
If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)
for the following galvanic elements under standard conditions write the reactions for each half element: Sn | SnSO4 || H2SO4 | Pt H2 Mg | MgCl2 || NiCl2 | Ni Pt H2 | H2SO4 || Hg2SO4 | Hg
Consider the following electrochemical cell: Pt|H,(8,p°)|HCI(aq,b)|Hg.Cl,(s)|Hg() The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg E/V I (ionic strength) Y: (DHLL) |Y: (linear fit) 1.6077 3.0769 5.0403 7.6938 10.9474 0.60080 0.56825 0.54366 0.52267 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. (ii) Determine the standard cell potential through simple calculation.
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What is Eocell in volts? In (s) | In(OH)3 (s) || SbO2- (aq) | Sb (s) In(OH) 3 (s) + 3 e-⟶In (s) + 3 OH- Eo = -1.00 VSbO2- (aq) + 2 H2O (l) + 3 e-⟶ Sb (s) + 4 OH- (aq) Eo = -0.66 V Group of answer choices +1.66 +0.34 -0.34 +1.98 -1. 66
A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
ELECTROCHEMISTRY Write the redox reactions and calculate the standard e.m.f.: Ce3+(aq) | Ce4+(aq) || Fe3+(aq) | Fe2+(aq) Pt | Cl2(g), Cl-(aq) || Br2(l), Br-(aq) | Pt
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
For the cell Pt(s) | H2(1 atm) | NaOH(aq) | Ag2O(s) | Ag(s), & = 1.172 V at 25°C (Hint: The cathode half-reaction involves Ag₂O -> 2Ag while the anode half-reaction involves the oxidation of H₂ to H₂O. Moreover, for the reaction H2(g) + ¹/2O2(g) → H₂O (1) AG has been calculated to be -237.32 kJ at the same temperature. At what partial pressure (in mm Hg) will oxygen be in equilibrium with silver oxide and silver at 25°C? Express your answer in two significant figures. R = 8.314 J K-¹ mol-¹ * = 96,485 C mol-1