Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4 (aq) + 8H*(aq) + 5e - Fe3+ (aq) + e → Fe2*(aq) Mn2+(aq) + 4H20() E° = 1.51 V E°= 0.77 V

Q: Calculate the equilibrium constant, K, for the following reaction at 25˚C. 2 Fe3+(aq) + Cu(s) → 2…

A: We have given with a reaction and we have to find equilibrium constant.

Q: Consider the following reductions. Cu+(aq) +  e- ⟶⟶ Cu(s)                                     Eored…

A: Oxidizing agent:-  It is a substance that oxidizes other substances and gets reduced by itself.…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Given: 4Cl-(aq) + N2(g) + 4H2O(l) →2Cl2(g) + N2H4(aq) + 4OH-(aq) To find: ∆G0 for the given…

Q: Write balanced half-reactions for the following redox reaction: 2+ 12 Cu²+ (aq) + C₂H₂OH(1) + 12…

A:

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A:

Q: Consider the following standard reduction potentials: Al3+(aq) + e-  →  Al(s)           E° = -1.66…

A: Al3+(aq) + e-  →  Al(s)           E° = -1.66 V Sn2+(aq) + 2e-  →  Sn(s)       E° = -0.14 V Cl2(g) +…

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: The point should be kept in mind while solving this problem, If the value of ΔGo is positive then…

Q: Chlorine dioxide (CIO,), which is produced by the reaction below, has been tested as a disinfectant…

A:

Q: Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) →…

A:

Q: Calculate the standard free‑energy change for this reaction at 25 °C. A list of standard reduction…

A: The given cell reaction is   2Au3+(aq) + 3Ni(s) → 2Au(s) + 3Ni2+(aq) ... (A)  Temperature = 25 °C =…

Q: Consider these two entries from a fictional table of standard reduction potentials. X+ (aq) + e Y+…

A:

Q: Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- →…

A: The half reactions are  1) Mt3+ (aq) + 3 e- → Mt (s)                                Eo = 1.09 V 2)…

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.