What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell reaction? Fe (s) + Co2+ (aq) → Fe2+ (aq) + Co (s) Note: this is the original reaction posted for the question was wrong. Someone suggested that this equation might be correct. Option choices are given below. If the answer found is not in the given answer choices, the reaction is wrong. The reaction given for the original problem was Fe(s) +Ni2+→Ni2+ + Co(s) Equilibrium constant: A. 1.39x1018 B. 6.0 C. 4.7 D. 9.7 E. 5.7x106   Gibbs Energy: A. 4.4 B. 39 C. -3.85 D. -4.4 E. 39

Q: Consider the following cell notation : Cr (s) |Cr^ 3+ (aq)||H 3 AsO 4(aq) ,H^ * (aq),H 3 AsO 3(aq)…

A: In the cell notation, the left most part indicates anode. At anode oxidation takes place. After the…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cu (s) is oxidized…

A: The cell notation for electrochemical celk is given below.

Q: Consider the following reaction at 298K. 2Fe³+ (aq) + Fe(s) 2Fe2+ (aq) + Fe²+ (aq) The standard…

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Q: NO3 + H* + Zn → Zn²+ + NO2 + H2O

A: Given skeletal equation is: NO3-+H+ +Zn →Zn2++NO2 +H2O Calculate its standard cell potential(Eo) and…

Q: The following electrochemical cell is constructed at standard state: Mg(s) | Mg2+ || Cr2+ | Cr(s) a)…

A: Answers are explained below.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2* (aq) is…

A: Answer:

Q: Devise cells in which the following are the reactions and calculate the standard cell potential in…

A: An Electrochemical is made of cathode and anode. In the cell process goes on are: oxidation and…

Q: Calculate the equilibrium constants of the following reactions at 25°C from standard potential data…

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Q: Cl2 + Br → Ch + Br2

A: The questions are based on the concept of redox reactions.   Redox Reaction  are those reactions in…

Q: s ) | B a 2 + | | C r 2 + | C r ( s )  a) Provide and label the oxidation and reduction…

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Q: Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

A: GIVEN:- Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

Q: Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized…

A: In this question, we will write cell notation for given anode and cathode half cell Reaction. How we…

Q: The reaction Sn (s) + 2 Cu²⁺ (aq) ⇌ Sn²⁺ (aq) + 2 Cu⁺ (aq) has a standard potential of 0.29 V at 25…

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Q: Consider the following equation, if the cell potential is 1.136 V at 25∘ C, determine the standard…

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Q: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

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Q: Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized…

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Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)|Cr3*(aq, 1.0 M) ||…

A:

Q: The reaction Sn (s) + 2 Cu²+ (aq) = Sn²+ (aq) + 2 Cu+ (aq) has a standard potential of 0.29 V at 25…

A:

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)ICr+(aq, 1.0 M) ||…

A: The cell given is, => Cr (s) | Cr3+ (aq, 1.0 M) || Ag+ (aq, 1.0 M) | Ag (s)

Q: The galvanic cell made up of cobalt, copper, and their M2+ ions, has a standard cell potential of…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Al (s) is oxidized…

A: CELL NOTATION Cell notation is the shorthand method of expressing the redox reaction. Both the half…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Fe2+ (aq) is…

A:

Q: Calculate the standard cell potential, standard free energy change, and equilibrium constant for the…

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Q: Calculate the standard cell potential and describe the reaction as spontaneous or non-…

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Q: construct a cell under standard conditions. The anode and cathode are iron and silver rods. Using…

A: We have to give information about the given cell

Q: John set up a galvanic cell. The balanced redox reaction equation is Mg(s) + 2 Ag+ (aq) →Mg2+(aq) +…

A: emf of cell can be calculate by Nernst equation  Ecell = Eocell  - (0.0591/n ) log Q   ----(1)…

Q: A current of 0.452 Amps is passed through an electrolytic cell containing molten CaCl2 for 1.50 hrs.…

A:

Q: For a single galvanic cell based on the (unbalanced) reaction:   Ag+(aq) + Zn(s)  Zn2+(aq) + Ag(s)…

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Q: The equilibrium constant of a cell with a cell potential of 0 V is a. 1.5 b. 2.5 c. 0 d. 1 e. 0.5 f.…

A: To Solve this problem we will calculate the equilibrium constant .

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) –→MN2*(1.00 M) + H2(g)(1.00 atm) If the cell…

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Q: 4H* + 4e + O2 -> 2 H2O, E• = + 0.82 V NAD* + H* + 2e -> NADH, E• = -0.32 V applied to the…

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Q: Write the cell notation for an electrochemical cell consisting of an anode where Fe2+ (aq) is…

A: Answer is explained below. According to the question,  At anode : Fe2+ (1M) | Fe3+ (1M) At cathode :…

Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

A: We have given that    the balanced chemical equation                    Cl2  + 2Br-  → Br2  + 2Cl-…

Q: The following spontaneous reaction occurs when metallic zinc is dipped into a solution of copper…

A: The given reaction is: Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s) When a zinc rod is inserted into a…

Q: Sketch  a galvanic cell  ( immersed in 1M solution)  with the cell notation…

A: Galvanic cell is an an electrochemical cell in which the chemical energy is converted into…

Q: Given the following cell notation for a galvanic cell, calculate the cell potential. Mg(s) Mg²* (aq)…

A:

Q: f the potential of a galvanic cell is +1.20 V, what is the Gibbs free-energy change when one mole of…

A: Given  potential of a galvanic cell is +1.20 V when one mole of electrons is transferred in the…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: Cell notation is a way to represent an electrochemical cell with anode and cathodes.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized…

A:

Q: You have the following setup to construct a cell under standard conditions. The anode and cathode…

A: Electrochemical cell of iron and silver contains silver as cathode in right hand side vessel while…

Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

A:

Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

A: The balanced redox reaction can be written as: MnO4- + 8H+ + 5e-  →  Mn2+ + 4H2O (Reduction)5Ce3+  →…

Q: In what way does a galvanic cell become an electrolytic cell? What is the difference between…

A: (1) Galvanic cell work on an spontaneous electrochemical Reaction in which Chemical energy is…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: The oxidation number represents the number of electrons gain or loses by an element to become…

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

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Q: The cell reaction for the ‘Bunsen cell’ is Zn(s) + 2 NO3−(aq) + 4 H+(aq) → Zn2+(aq) + 2 H2O(l) + 2…

A: Given data contains, Standard cell potential is -0.040V. The given cell reaction is, Zn(s) + 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.