A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell potential is E=0.8V Faraday Constant is 96485 C/mol. Write the cell diagram with a salt bridge. i) ii) Calculate the standard formation energy of Ag+ and standard equilibrium constant K at 300K.

Q: (c) Calculate the standard cell potential, E° of the following reaction at equilibrium. Show your…

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Q: Calculate the cell potential for the galvanic cell in which the reaction   Ti(s)+Cu2+(aq)↽−−⇀…

A: Given:  The concentration of Ti2+ is 0.00140 M. The concentration of Cu2+ is 0.875 M. Introduction:…

Q: Why is it necessary to use the standard hydrogen half-cell as a reference when calculating standard…

A: Given statement is :  Why is it necessary to use the standard hydrogen half-cell as a reference when…

Q: The standard reaction Gibbs energy for the electrochemical reaction Cr2O7^2- + 2 Fe + 14 H+ → 2 Cr3+…

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Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

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Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au³+ (aq)= Al3+(aq)…

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Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

A: The question is about a concentration cell based on A+

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³*(aq) = Fe*(aq)…

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Q: State what is expected to happen to the cell potential when the specified changes are made to the…

A: As there are many parts of the question, and have not asked about specific part, discuss first three…

Q: (a) Balance the following simple redox reaction. Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4 OH- (3) (b) If…

A: Redox reaction : it is the reaction where oxidation and reduction are occurred simultaneously . the…

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

Q: The standard potential of a Daniell cell, with cell reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), is…

A: The reaction:

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Please find your solution below :

Q: If the free energy of an electrochemical process is +12 kJ/mol and n=3, what is the standard cell…

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Q: The standard cell potential for the reaction provided below is 0.301 V, (where X is a non-metal…

A: Interpretation -  To determine the cell potential when there are 14.6 g of X,  PH2 =  2.99atm, and…

Q: In the electroplating of nickel from a solution containing Ni2+ ions what weight of nickel-metal…

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Q: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

Q: A constant current flows for 3.75 h through an electrolytic cell containing aqueous AgNO3(aq).…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

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

A: Given, 2VO2+(aq) + 4H+(aq) + Fe(s) --------> 2VO2+(aq) + 2H2O(l) + Fe2+(aq)  [VO2+] = 1.50 M…

Q: (c) Calculate the standard cell potential, E° of the following reaction at equilibrium. Show your…

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Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

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Q: The standard cell potential for the Daniell cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) is +1.102 V at…

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Q: The standard cell potential for the reaction Zn + 2 Ag+(aq) → Zn2+(aq) + 2 Ag is 1.56 V. Given that…

A: In the given reaction the Zn is getting oxidized to Zn2+ while the Ag+ is getting reduced to Ag. So…

Q: Devise a cell in which the cell reaction is Mn(s) + Cl2(g) → MnCI, (aq). Give the half-reactions for…

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Q: The standard cell potential of a voltaic cell consdtructed using the cell reaction below is 0.772 V.…

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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: In an experiment of a redox reaction, an electrochemical cell has been set up by connecting a vessel…

A: The balanced redox reaction that represents the described galvanic cell can be written as follows:…

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

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

Q: One ecologically important equilibrium is that between carbonate and hydrogencarbonate (bicarbonate)…

A: The relation between free energy and cell potential is shown below: ∆G0 =-nFE0cell where; ∆G =…

Q: The standard cell potential of a Daniell cell, with cell reactionZn(s) + Cu2+(aq) → Zn2+(aq) +…

A: Given, a Daniell cell with the cell reaction as follows,Zn(s)+Cu2+→Zn2++Cu(s)the standard cell…

Q: 1. (a) Balance the following simple redox reaction. Fe (s) + O2(g) + 2H2O (I) → Fe3* + 4 OH (b) If…

A: In an electrochemical reaction redox reaction occur in different electrode  At cathode we expect…

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: Calculate the cell potential for the galvanic cell in which the reaction   Al(s)+Au3+(aq)↽−−⇀…

A: Cell potential of a galvanic cell can be calculated using nernst equation

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: Gibbs energy change, A;G°, is related to cell potential, Eel, by the equation A;G° = -nFEl Part B…

A: The given reaction is as follows: Xs+2Y+(aq) → X2+(aq) + 2Y(s) ∆rG° of the reaction can be…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³*(aq) =…

A: Given:  Temperature (T)=25oC                             =(25+273)K…

Q: Calculate the standard cell potential, ?∘cell,Ecell∘, for the equation…

A: Since the cell potentials for the half reactions are as Sn(s)  -----> Sn2+ (aq) + 2 e-…

Q: 1. (a) Balance the following simple redox reaction. Fe (s) + O₂(g) + 2H₂O (1)→ Fe³+ + 4 OH (b) If…

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Q: The standard cell potential for the reaction at 298.15 K: Fe (s) + Zn2+ (aq) ⇋ Fe2+ (aq) + Zn (s)…

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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: onsider the following reaction at 298K. Fe³+(aq) + Cd(s)→→→→→2Fe²+ (aq) + Cd²+ (aq) he standard…

A: Given,             ∆G°=-226.58kJ 2Fe3+(aq) + Cd(s) →2Fe2+(aq) + Cd2+(aq)∆G°=-nFEocelln= Number of…

Q: What mass of iron (III) sulfate is present in 100 cm3 of the solution used to measure the standard…

A: 39.9 g

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

A: Write the reactions taking place at anode and cathode,

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

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Q: A student does an experiment to determine the molar solubility of lead(II) bromide. She constructs a…

A: Electrochemical Potential is the chemical potential of the cell generated through the means of…

Q: Use the biological standard potentials of two reduction reactions 4H* + 4e + 02-> 2 H20, E = + 0.82…

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Q: Calculate the standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s) and the standard…

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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.