at 25 ° C, the galvanic element Pt | MnO4- 0.1M, Mn2 + 0.1M, pH = 1 || Ag + 0.0001M | Ag has the electromotive force 0.80V. Calculate the standard electrode potential for the reduction of Ag +, if E ° (MnO4-, H + | Mn2 +) = 1.50V

Q: 5. For the following reaction at 25 °C, 5FE2+ *(aq) + MnO4 (aq) + 8H"(aq) = 5Fe*(aq) + Mn²*(aq) +…

A: Given :  [Fe+2] = 0.50 M  [Fe+3] = 0.10 M  [MnO4-] = 0.025 M  [Mn+2] = 0.015 M pH = 7.00  => [H+]…

Q: A galvanic cell is constructed in which the overall reactionis Cr,0; (aq) + 14 H2O* (aq) + 6I¯ (aq)…

A: Answer:- This question is answered by using the simple concept of calculation standard cell…

Q: To what pH should you adjust a standard hydrogen electrode toachieve an electrode potential of…

A:

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

A:

Q: at a temperature of 25 ° C the galvanic element Pt | ClO3- 0,001M, Cl- 0,01M pH = 3 || Mn2 + 0.0001M…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co2+(aq) = Ti²+(aq)…

A:

Q: (a) The cell potential for the following electrochemical cell at 25°C is 1.00 V. Pt(s) |H2 (g, x…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq)…

A:

Q: Suppose a metal electrode is being coated with silver according to the half-reaction, Ag+(aq) + e-…

A: Current = 0.850 A Time = 20.0 min  ....Or = 20.0 min × (60 sec / 1 min )   ...(because, 1 min = 60…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq)+…

A:

Q: S. Given the following reduction half-reactions at 298 K: Half-Reaction E (V) at 298 K Fe" (aq) + e→…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo (aq) +…

A:

Q: If at 25°C the standard electrode potential of the Ag/Ag* electrode is 0.799 V, and the equilibrium…

A:

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: given data are-  Fe(s) ⟶ Fe2+(aq) + 2e-Eo = -0.44 V  O2(g) + 4H+(aq) + 4e- ⟶  2H2O(l)  Eo = 1.23 V…

Q: (aq) + Sn (aq) 11. Calculate the cell potential of a cell operating with the following reaction at…

A: Q 11)  cell potential  E = - 2.435 V Q 12) Concentration of Ni2+ = 1.832 x 10-5

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: The standard potential of the cell Ag(s)|AgI(s)|AgI(aq)|Ag(s) is +0.9509 V at 25 °C. Calculate the…

A: The given reaction is a concentration cell for which Ecell = 0 Now, the standard cell potential…

Q: For Ag+(aq) + e-→ Ag(s), Eº = +0.80 V and for Zn²+(aq) + 2e¯ → Zn(s), E° = -0.76 V. a) Identify…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: If the potential of a Zn-H+cell is 0.45V at 25 degrees C when[Zn]-1.0M and PH2=1.0 atm, what is the…

A:

Q: Consider the following redox half-reaction at 25 °C: MnO4 (aq) + 8 H* (aq) + 5 e¯ → Mn²* (aq) + 4…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au+(aq) = Al³*(aq)…

A: In this question firs determine standard cell potential then apply Nerst equation.

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. Wate eb. Calculate the equilibrium…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: 8. Given the following unbalanced redox reaction: CIO (aq) + (aq) → 103(aq) + CH(aq) Basic solution.…

A:

Q: Q 2: Galvanic cell presented as Fe/Fe //Co/Co, If reduction potential of iron = - 0.409 V, and for…

A:

Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

Q: The emf of a standard X-Y galvanic cell is -2.763V. If the standard half-cell emf for the oxidation…

A: The overall cell reaction is the sum of the two half-reactions, but the cell potential is the…

Q: A steady current of 3 A is maintained for 10 mins in AgNO3 solution. How much Ag is deposited at the…

A: Given: Current is 3 A. Time is 10 minutes. To find: Mass of Ag on cathode

Q: The standard reduction potential (E°) for the conversion of Cr,0 to Cr* at 25°C in an aqueous…

A: Cr2O7 2- + 14H+ + 6e- ------------------> 2Cr3+  + 7H2O            E0(Cr6+/Cr3+)   = 1.33 V  +6…

Q: A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell…

A: Ag+ (aq) + 0.5 H2 (g) ==> H+(aq) + Ag(s)

Q: Will oxygen, O2, oxidize iron(II) ion in solution under standard conditions? Cathode (Reduction)…

A:

Q: For an aqueous solution of 0.250 M Cd2+, use the Nemst Equation to calculate the theoretical cathode…

A: We need to find the cathode potential using Nerst equation.

Q: If at 25°C the standard electrode potential of the Ag/Ag' electrode is U.799 V, and the equilibrium…

A: Fe+3 + Ag ------> Fe+2 + Ag+ EoAg|Ag+= 0.799 V K = 0.531 V

Q: A galvanic cell is constructed in which the overall reactionis 2- Cr2 0; (aq) + 14 H2O† (aq) + 6 I…

A:

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: Given reaction is :  2Ag+ (aq) + Cu (s) ------------> 2Ag (s) + Cu2+ (aq) , ΔG0 = -88660 J/mole…

Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl, (g) 2 Ag* (aq) + 2 CI…

A:

Q: Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG =…

A:

Q: A galvanic cell is constructed in which the overall reac- tion is Cr,O (aq) + 14 H,0 (aq) + 61 (aq)…

A: GALVANIC CELL A galvanic cell is an electrochemical cell that converts chemical energy into…

Q: Consider the following reaction and its AG° at 25.00 °C. 2 Ag*(aq)+Cu(s) → 2 Ag(s) + Cu2+(aq) AG° =…

A: ∆G = -88.66 KJ/mol = -88660 J/mol  Temperature (T) = 25°C = 25+273 = 298 K  R = 8.314 J/mol.K  Keq =…

Q: 1. Consider the reaction: MnO2(s) + 4H*(aq)+ 2B1¯(aq) → Mn2+(aq) + Br,(l)+2H,O(1) At what pH will…

A: The electrochemical cell is the one that generates electrical energy from chemical energy. It is…

Q: (a) The potential for the following electrochemical cell at 25"C is 0.34 V. Pe(s}l}2 (8, 1 atm)|…

A:

Q: A voltaic cell is constructed with two hydrogen electrodes. Electrode 1 has PH2 = 1.00 atm and an…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given data are as follows: Cell potential =- 0.201 V Temperature = 298 K Pressure = 1 atm.

Q: For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735…

A:

Q: For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M),…

A: Provided concentration of Mn2+=0.215M Provided concentration of Cr3+=0.113M Provided concentration…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A:

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with[Ag+]  = 1.0…

A: The given parameters are: [Ag+]  = 1.0 M molarity of NH3 = 5.0 M  [Cu(NH3)42+] = 0.020 M…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.