Consider this cell: Sn (s) | Sn+ (aq) I| Br2 (u | Br" (aq) | Pt (s) Sn (s) + Br2 (u → Sn2+ (ag) + 2 Br (ag) A,H° = -252 kJ/mol Br2 () + 2 e→ 2 Br 1.09 V (aq) • What is the standard cell potential for this cell at 25 °C? You will also need to refer to your table of standard potentials. • What is the potential of the cell at this temperature if the concentration of bromide ions is 0.131 M and the concentration of tin ions is 18 µM? What is the equilibrium constant for the reaction at this temperature?

Q: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) | Hg() | Pt(s) Use…

A:

Q: The standard reaction Gibbs energy for the reaction: K2CrO4 (aq) + 2 Ag (s) + 2 FeCl3 (s) → Ag2CrO4…

A: Gibbs' free energy for an electrochemical reaction, whose standard potential is to be determined.

Q: Give the standard line notation for each cell. (a) 2 IOs (ag) + 10 Fe²+ (aq) + 10 H* (ag) = 10 Fe+…

A: Answer:- This question is answered by using the simple concept of writing the cell notation using…

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: Consider the cell: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) |…

A:

Q: The cell reaction of the “Bunsen cell” is Zn(s) + 2NO3-(aq) + 4H+(aq) Zn+2(aq) + 2H2O(l) + 2NO2(g).…

A: Zn(s) + 2NO3-(aq) + 4H+(aq) --> Zn+2(aq) + 2H2O(l) + 2NO2(g)2NO3- + 4H+(aq)  +2e  -->2NO2 +…

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

A: Given: Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s)

Q: Give the standard line notation for each cell. (а) 2 IO3 (aq) + 10 Fe?+ (aq) + 10 H* (aq) = 10 Fe…

A: Single vertical line indicate phase boundary, double vertical line is salt bridge.Left of the salt…

Q: =

A: Given: Sn | Sn2+ (aq) =−0.140 V Pb | Pb2+(aq) =−0.126 V, T= 298 K

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 standard cell potential at 25°C for the following cell reaction from standard free…

A: The question contains more than one question so only the first one is solved here, if the other one…

Q: Given the following notation for an electrochemical cell Pt(s) | Sn²+(aq), Sn 4+ (aq) || Cl2(g) |…

A: The electrochemical cell notation represents, The oxidation half cell reaction on the left and the…

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: What is the copper(II)-ion concentration at 25°C in the cell Zn(s) | Zn2+(aq, 1.0 M) || Cu2+(aq) |…

A:

Q: An electrochemical cell Bi(s) | Bi2S3(s) | Bi2S3(aq) | Bi(s) the standard potential is 0.96 V at 25…

A: we  have to calculate the equilibrium constant for the cell

Q: 4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider…

A: The question is based on the concept of electrochemistry. we need to calculate standard cell…

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

A:

Q: Consider the cell: Pt(s) | H₂(g, 0.100 bar) | H+ (aq, pH = 2.54) || Cl(aq, 0.200 M) | Hg₂Cl₂(s) |…

A: In the given cell notation, H2(g) is undergoing oxidation to H+(aq), and Hg22+(aq) from Hg2Cl2(s) is…

Q: The cell potential of the following electrochemical cell is determined by using an unspecified…

A: We have find out the answer.

Q: he observed cell potential for a voltaic cell is 2.067 V when the temperature is 298 K and the…

A: Electrochemistry is the branch of chemistry which studies the change of chemical energy into…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A:

Q: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

A:

Q: Electrochemical cell Pt | H2(g) | Hl(aq) || Agl(s) | Ag(s)has electromotive potential of 0.52 V at…

A:

Q: A galvanic cell was constructed where one electrode was a Cu2*(aq)|Cu(s) electrode and the other was…

A: In general,in a galvanic(voltaic) cell, the electrode at which reduction takes place is written on…

Q: 1. Write the electrode reactions and the cell reactions for the following galvanic cells, and…

A: 1)   Cu CuCl2(aq) | Cl2(g), Pt The electrode reactions for this galvanic cell are as follows:   At…

Q: The standard reaction Gibbs energy for the reaction: K2CrO4 (aq) + 2 Ag (s) + 2 FeCl3 (s) → Ag2CrO4…

A:

Q: Consider the following galvanic cell at 25°C:Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|CoThe overall…

A:

Q: Consider the following galvanic cell at 25°C Pt|Br (aq) (0.25 M), H* (aq) (0.1 M) |Br2 () || O2 (g)…

A:

Q: The following cell with the standard cell notation shown below has an t potential of 0.92 Volts…

A: As per the Nernst equation under standard conditions,   Ecell=Ecell0-0.0591nlog[A2+][B+]2----(1)

Q: ) For the concentration cell: Pt(s) | H2(g), H+(aq) (pH = 10) || H+(aq) (pH = 4), H2(g) | Pt(s),…

A: From nernst equation, E cell can be calculated

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) Determine the cell…

A: Given cell reaction:

Q: Using these metal ion/metal reaction potentials Cu2+(aq)|Cu(s)       Ag+(aq)|Ag(s)…

A:

Q: Find the nonstandard cell potential for the galvanic cell described by the cell notation provided…

A: The Nernst equation is as follows,                      Ecell = Ecello - 0.0592 Vn log10 Q Where,…

Q: Zn(s) | Ag*(aq) || Zn²* (aq) | Ag(s) Ag(s) | Ag* (aq) || Zn2+ (aq) | Zn(s) Ag(s) | Zn* (aq) || Ag*…

A: In electrochemical cell,  Anode half reaction is written left side and cathode half reaction is…

Q: The cell potential of an electrochemical cell with the cell reaction 2Al(s) + 3cu2+(aq) → 3cu(s) +…

A: Welcome to bartleby !  We have to tell the maximum work .

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.