A voltaic cell is based on a nitrate/NO half-cell and a NiCl2/Ni half-cell. (Heads up, the chloride ions in this reaction are bystander ions.) Eo for NO-3 (aq) → NO(g) = +0.96 Eo for NiCl2 (aq) → Ni(s) = –0.28  What is the cell potential of the reaction when pH = 2.7, [NO3-] = 1.5 M, PNO = 0.010 atm and [Ni2+] = 0.21 M

Q: 3. A galvanic cell is constructed comprising cadmium anode and nickel cathode: Cd (s) + Ni²+ (aq) →…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2103(aq)…

A: Answer: Cell potential will be calculated using Nernst equation which is shown below:…

Q: A galvanic cell is constructed that uses the following half-cell reactions: Cu+(aq) + e−→ Cu(s)…

A: Find the complete solution given below

Q: A galvanic cell is constructed that carries out the reaction 2Ag(s) + Cl2 (g) → 2Ag+(aq) + 2CI- (ag)…

A:

Q: Suppose that you want to construct a voltaic cell from nickel and cadmium for a chemistry project.…

A: Given data,Molarity of Cd2+=0.01ME=0.17V

Q: Consider the electrochemical cell described by the following reaction at 310 K. The measured cell…

A: Given Cell potential is 0.242 V  E° CuI/I-/Cu= -0.17 V E° Cd 2+/Cd= -0.403V

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

A: Standard cell potential, E0: The standard cell potential (E°cell) is the potential of the cell under…

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

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2     E0= -2.87…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) +…

A: We can use Nerst Equation to solved the above problem.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²+ (aq) +…

A:

Q: A galvanic cell is based on the following two half-reactions: Pb(s) → Pb2+(aq, 0.10 mol L−1 ) + 2e −…

A:

Q: A concentration cell consisting of two hydrogen electrodes (P = H₂ 1atm), where the cathode is a…

A: Answer:Concentration cell is galvanic cell in which same electrolyte of different concentrations is…

Q: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution :    Nernst equation is used to calculate the potential of the cell at non-standard…

Q: ) Consider the galvanic cell, Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s). Which one of the following…

A: Galvanic cell : The notation in galvanic cell is written as : So , the reaction for given cell…

Q: Consider a galvanic cell that uses the reaction Zn(s) + 2H+(aq) →Zn2+(aq) + H2(g) Calculate the…

A: Concentrations [H+] = 1.0 M  [Zn2+] = 0.0010 M pH2 = 0.10 atm Cell reaction Zn(s) + 2H+(aq)…

Q: When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Given reaction is :  Cu2+ (aq) + Mg (s) ------> Cu (s) + Mg2+ (aq)  [Cu2+] = 1.49 M  Non-standard…

Q: what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The…

A: The solution is as follows :

Q: Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter.…

A: The objective of the question is to-a) Write the balanced chemical equation.b) Determine the…

Q: The cell notation for a galvanic cell is shown below. What is the oxidizing agent?…

A: The species undergoing an increase in oxidation state is oxidation or reducing agent whereas species…

Q: What is the overall reaction for the following cell line notation of a galvanic cell? Al(s)|AI3*(aq)…

A: Cell line notation of a galvanic cell :  Al(s)|Al3+(aq) || H+(aq)|H2(g)|Pt  Overall reaction for…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) +…

A:

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: A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e →…

A: two half reactions and reduction potential of each is given

Q: A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500 M…

A: Given,  A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500…

Q: Fe+ (ag) + Zn(s) Fe(s) + Zn?+(aq) E cell = +0.32 V A galvanic cell generates a cell potential of…

A:

Q: A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a…

A: The given equation is, The anode reaction of given cell is, The cathode reaction of given cell is,…

Q: The potential of a voltaic cell is 0.698 V in which the following reaction takes place: 2NO, (aq) +…

A: Given data, EMF = 0.698V [NO3-] = 0.0315M PNO = 0.922atm PH2 = 0.437atm

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M)…

A: Given the cell reaction is: Cu(s) + 2Ag+(aq) (0.100 M)  <-----> Cu2+(aq) (0.200 M) + 2Ag(s)…

Q: The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard…

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

Q: What is the maximum electrical work obtainable from this cell when 0.150 g of Al is consumed?

A: Provided data :- E°cell = 1.63 V  Cell reaction :- Al(s) + Cr3+(aq) -> Cr(s) + Al3+(aq) It means…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) +…

A: We have to find standard electrode potential  Eocell = Eocathode - Eoanode

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.