Calculate E° for the half reaction: Ag,S03(s) + 2e = 2Ag(s) + SO?- given that Ksp for Ag,S0, is 1.5x10-14 and E° for Ag+ + e = Ag(s) = 0.799v.

Q: For the electrochemical cell 2 Al(s) + 3 Mn2* (aq) – 2 Al$*(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0…

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Q: For the electrochemical cell 2 AI(s) + 3 Mn2*(aq) – 2 Al3*(aq) + 3 Mn(s) (E° = 0.48 V, [A]³*] = 1.0…

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Q: Consider the following reaction: O2 (g) + 4H* (ag) + 4FE²* (aq) 2H20 (1) + 4Fe3+ (aq) %3D O2+ 4H*…

A: E0cell = E0cathode-E0anode The half cell with higher the E0 - value when compared to other half cell…

Q: For the reaction 2C03+ (aq) + 2CI- (aq)→2C0²+(aq) + Cl2 (g). E° =0.483 V what is the cell potential…

A: Cell potential is calculated using Nernst equation .

Q: Determine the value of Ecell (25°C) for the following galvanic cell: Q (s)  ∣  Q2+(aq, 0.088 M)  ‖…

A: In electrochemistry, the Nernst equation is an equation that relates the reduction potential of an…

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

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Q: What is the standard emf of a galvanic cell made of a Ni electrode in a 1.0 M Ni(NO3)2 solution and…

A: Oxidation is lose of electrons. Reduction is gaining of electrons. The reactions where oxidation and…

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A: Given,  2Al(s) + 3Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M),…

Q: In a galvanic cell based on the half reactions Ni²⁺(aq) + 2e⁻ → Ni(s) E° = -0.250 V 2H⁺(aq) + 2e⁻…

A: The cell reactions are :   Ni²⁺(aq) + 2e⁻ → Ni(s) E° = -0.250 V 2H⁺(aq) + 2e⁻ → H₂ E° = 0.000 V…

Q: For the galvanic (voltaic) cell Fe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A: Given electrochemical cell reaction equation; Fe (s) + Mn2+(aq) → Fe2+(aq) + Mn (s) Given standard…

Q: Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an…

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Q: Calculate AG° and K for the following cell reactions. State whether the cell reaction is spontaneous…

A: recall the given reaction and also the values of electrode potential of the given half cell Cus +…

Q: The free energy change for the following reaction at 25 °C, when [Zn²+] = 4.75×10³ M and [Ni2*] =…

A: Answer: These questions are based on relationship between Gibbs free energy change and cell…

Q: The following photos supplement what is included in the video on Courseworks. IMC Equipment for the…

A: Given data,  For Copper - Copper concentration cell   CuSO4(aq) = 0.001 M  CuSO4 (aq) = 1 M  The…

Q: Calculate the cell potential, at 298 K, for the following reaction under the conditions given. Pb(s)…

A: The cell reaction taking place is given as, => Pb (s) + Fe2+ (aq, 0.0100 M) ------> Pb2+ (aq,…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A: A redox reaction takes place in an electrolytic cell where the electrical energy is fed into the…

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

A: Given equation :             2Co3+(aq)+ 2Cl-(aq) → 2Co2+(aq)+ Cl2(g)                       Eο =…

Q: (i) Pt(s) + 2 NH3(aq) + 2 CI ( (aq) cis-[PtCl₂(NH3)2](aq) + 2 e¯ E° = 0.274 V The likely cathodic…

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Q: For the galvanic (voltaic) cell Cd²*(aq) + Fe(s) – Cd(s) + Fe2*(aq) (E° = 0.0400 V), what is the…

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Q: For the galvanic (voltaic) cell Cd²*(aq) + Fe(s) – Cd(s) + Fe²*(aq) (E° = 0.0400 V), what is the…

A: The expression of Nernst equation is shown below: Where; Ecell= cell potential E0cell = standard…

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V   what is the cell potential at 25…

A: Nernst equation defines the cell's potential in any electrochemical reaction. The cell potential…

Q: Consider the following reaction at 25 °C. (Ans.: 0.369 V) Cd*2 + 2e → Cd Zn* + 2e –→ Zn E° = -0.403…

A: Given:  E°(Cd+2|Cd) = -0.403 V And E°(Zn+2|Zn) = -0.763 V [Zn+2] = 0.05 M  [Cd+2] = 0.1M

Q: The free energy change for the following reaction at 25 °C, when [Ni²*] = 1.14 M and [Ca2+] =…

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Q: For the galvanic (voltaic) cell Fe(s) + Mn2 (aq) - Fe2 (aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A:

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

A: Given galvanic cell is: Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq)           The standard reduction…

Q: The batteries used in automobiles are rechargeable and consist of Pb and PbO2 anodes and cathodes…

A: Calculation of E˚cell: Ecell of the reaction is given as: Calculation of temperature coefficient,…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 237.73 °C with the…

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Q: Direct methanol fuel cells (DMFCS) have shown some promise as a viable option for providing "green"…

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Q: In a galvanic cell the cathode is an Ag+11.00 M2>Ag1s2 half-cell. The anode is a standard…

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Q: Calculate the standard potential for the following reaction at 25°C.            Cd(s) + 2Ag+(aq) ⇌…

A: The Ecell0 of the cell is given by the sum of oxidation half cell and reduction half cell.

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A: The solution is as follows :

Q: Standard Reduction Potentials at Standard States and 25°C Pb(s) + 2H1+(0.0010 M) Pb2*(.50 M) +…

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Q: Calculate the theoretical cell potential of the following cells. If the cell is short-circuited,…

A: Theoretical cell potential can be calculated using nernst equation for cell: Ecell = E°cell -…

Q: Mn²+ + 2e - Mn e° = -1.18 V Fe2+ + 2e¯ - Fe e° = -0.44 V a. Determine the overall cell reaction and…

A: Given: Mn2++2e-→Mn    eo=-1.18 V Fe2++2e-→Fe  e0=-0.44 V Element with higher reduction potential…

Q: Starting with the standard free energies of formation from the following table, calculate the values…

A: The enthalpy change is calculated for the given reaction as follows,

Q: Calculate the cell potential, G (J), and the equilibrium constant Keq for the following…

A: The answer is given below:

Q: The reaction 2Ag+(aq) + Cu(s) → 2Ag(s) + Cu2+(aq) was used in a galvanic cell. E°=0.46 V for this…

A: Given the chemical reaction as follows,2Ag+(aq)+Cu(s)→2Ag(s)+Cu2+(aq)E°=0.46 Vthe concentrations of…

Q: For the electrochemical cell 2 AI(s) + 3 Mn²*(aq) → 2 Al*(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0…

A: Nernst equation for the given reaction is :  Ecell = E°cell -…

Q: For the galvanic (voltaic) cell Fe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A: We have the given E° cell as 0.77 V Ecell given as 0.78 V All performed at 25°C or 298K We have Mn+2…

Q: half-cell potential for the reaction O2 (g)+ 4H+ (aq) 4e → 2H2O (l) is 1.03V at 310K when activities…

A: Given-> Ecell = 1.03 V T = 310 K Activities of O2, H2O = 1  pH = ?

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A:

Q: Determine the corrosion rate ( mpy ) of steel corresponding to 1µA / cm? of current. Following is…

A: The corrosion rate of the system in mpy for the given current density is calculated as shown in…

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

A: Answer: The ratio [Fe²⁺]/[Cd²⁺] is 10.35.

Q: For the galvanic (voltaic) cell Fe(s) + Mn2" (aq) Fe2*(aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A: We can use the Nernst equation to calculate the Ecell of a reaction. We have to get number of…

Q: For the galvanic (voltaic) cell Fe(s) + Mn² (aq) Fe2 (aq) + Mn(s) (E° :0.77 V at 25°C), what is…

A: Concentration of Fe2+ ion is .039 M

Q: For the electrochemical cell 2 Al(s) + 3 Mn2*(aq) → 2 Al** (aq) + 3 Mn(s) (E° = 0.48 V, [AI*] = 1.0…

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Q: A voltaic cell is constructed with two silver electrodes, where the half-reaction is Ag2+(aq) + 2e-…

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Q: Determine E, AG, and K for the overall reaction from the balanced half-reactions and their standard…

A: Given-> 2Co3+ + H3AsO3 +H2O <-------> 2Co2+ + H3AsO4 +2H+ Co3+ + e- ------> Co2+.  E° =…

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

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.