A Cu2+(1.00 M) | Cu half-cell is connected to a Br2(|) | Br2half-cell in which the concentration of bromide ion isunknown. The measured cell potential is 0.963 V, and theCu2+ | Cu half-cell is the anode. What is the bromide ionconcentration in the Br2(|) | Br2 half-cell?

Q: Calculate the standard e.m.f, standard free energy change and equilibrium constant for the following…

A: Answer: Since, Copper is getting oxidized therefore it will be at anode and chlorine is getting…

Q: For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe3+|Fe2+electrode, what is the…

A: In voltaic cell, a spontaneous reaction occur. Greater the value of standard reduction potential of…

Q: 1)))) How many faradays must pass through an electrolytic cell to reduce 0.32 mol Ag+ ion to silver…

A:

Q: Consider the following electrochemical cell at 25 oC: www Zn Zn²+(1 M)||Cr³+ (0.1 M) Cr (a) what is…

A: Cell : Zn | Zn2+(1 M) || Cr3+(0.1 M )| Cr

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

A: Answers are explained below.

Q: Cr|Cr3+ ||Co2+ |Co Eo is 0.46V. the same cell was prepared in the laboratory at standard conditions.…

A:

Q: 40. In a galvanic cell, the cathode consists of a Ag"(1.00 M)|Ag half-cell. The anode is a platinum…

A:

Q: A Zn-Ag Galvanic cell has an Ecell value of 1.536 V. The cell diagram is as blow. Calculate the…

A: This is a simple question of electrochemistry for the application of Nernst equation.

Q: Calculate the cell potential (Ecell) for the following lead concentration cell at 298 K. Anode Pb…

A: Answer:Concentration cell is a type of galvanic cell in which solution of same electrolyte with…

Q: A student is given two beakers in the laboratory. One beaker contains a solution that is 0.14 M in…

A: Given: [Mn3+ ] = 0.14 M [Mn2+ ] = 0.46 M [Sn2+ ] = 0.28 M And [Sn4+ ] = 0.056 M

Q: Provide the half-reactions and calculate the potential for the following galvanic cell.…

A: When we take a reaction there are two half cell for that reaction which are connected by external…

Q: Calculate the cell potential (Ecell) for the following lead concentration cell at 298 K. Anode Pb…

A:

Q: Consider the following cell: | Zn (s) | Ca²* (aq) , SO3² (aq) || Hg²* (aq) , F` (aq) | Pt (s) | a)…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Consider the following silver-cadmium cell: Cd(s)/Cd2+(0.50 M)//Ag+(0.0025 M)/Ag(s). Compute the…

A: To calculate the cell potential for the given silver-cadmium cell at 25oC, we can use the…

Q: O Confirm that the following concentration cell has a cell potential of 0.068 V at 298 K. Cu(s) Cu2+…

A: To confirm that the concentration cell has a cell potential of 0.068 V at 298 K, we will use the…

Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

A: The given cell notation is: Cu|Cu2+0.020 M||Cu2+2.0 M|Cu It is a concentration cell (electrolytic…

Q: Write the cell voltage of the ff cell. Define if it is in Spontaneous or Nonspontaneous reaction. Au…

A: Given cells are : a). Au | 1.0 M AuNO3 || 1.0 M AgNO3 | Ag  b). Li | 1.0 M LiNO3 || 1.0 M AlCl3 | Al…

Q: Fe2+ (0.2 M) | Pt (s) A)  At 25 ºC, when the reaction quotient, Q, is equal to the equilibrium…

A:

Q: onsider the following half-cells:    (1)  AgCl(s) | Ag(s), Cl–(aq)                      E°red =…

A: The given half cells are:    (1)  AgCl(s) | Ag(s), Cl–(aq)                       E°red = +0.22 V…

Q: X(s)|X4+ (0.87 M) || Mn O4 1 minus (1.61 M)|Mn2+ (2.98 M)|H+ (1.49 M) The reduction potential for…

A: Given information: Reduction potential for X4+ = 2.22 V Reduction potential for MnO4- = 1.51 V

Q: A concentration cell is built using two Au/Au3+half-cells. In half-cell A, [Au3+] = 7.0 x 10-4 M and…

A: The objective of this question is to determine the cell potential (E_cell) and identify which…

Q: Calculate the cell potential for the following concentration cell at 25 °C.…

A: Here the cell represented consists of a cathode and the anode made up of nickel. In the cell…

Q: standard cell potential f

A:

Q: A Galvanic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34…

A: 0.03 MExplanation:

Q: Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10M Zn(NO3)2…

A: In the given question we have to calculate the reduction potential of Sn2+/Sn . given data:…

Q: Consider a galvanic cell below and calculate the concentration of Au*3 solution. The measured cell…

A:

Q: Calculate the value of the potential for the following electrochemical cell under the conditions…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: Calculate the emf of the following concentration cell at 25oC:  Ag(s)|Ag+(0.12 M)||Ag+(1.9 M)|Ag(s)

A:

Q: 30) Write the balanced overall reaction and calculate the standard cell emf (E) for: Al(s) | Al"(aq)…

A:

Q: The voltaic cell Cd(s)|Cd?+ (aq) || Ni²+ (1.0 M)|Ni(s) has a cell potential of 0.310 V at 25°C. What…

A: The voltaic cell is as follows: Cd(s)|Cd2+(aq)||Ni2+(1.0 M)|Ni(s) Ecell=0.310 VEcell°=0.170 V The…

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.