8.5 Using data from Table 8.1, write down the spontaneous cell process, and calculate E°cell and AG° for the following combinations of half-cells: (a) Ag*(aq) + e¯ = Ag(s) with Zn* (aq) + 2e" = Zn(s) (b) Br, (aq) + 2e- = 2Br (aq) with Cl,(aq)+ 2e = 2C1" (aq) (c) [Cr0; (aq) + 14H* (aq) + 6e = 2Cr* (aq) + 7H,0(1) with Fe* (aq) +e = Fe* (aq) 1.

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: EFM of the cell is calculated by using below formula,

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

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 standard cell potential for the following galvanic cell is 0.390 V.  What is the cell potential…

A: Given: Temperature = 325 K Eocell = 0.390 V Concentration of Sc+3 = 0.077 M Concentration of Ti+2 =…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E°…

A:

Q: The galvanic cell utilizes the following reaction of oxidation of iron and reduction of cadmium at…

A: Fe + Cd+2       - - - - - > Fe+2  + Cd Cd+2 +2e- - - - - - > Cd         E° = - 0.40 V Fe - - -…

Q: A voltaic cell utilizes the following reaction and operates at 298 K. (a) What is the emf of this…

A:

Q: Calculate K for scandium fluoride, SCF3, given that the cell potential at 25 °C for the following…

A:

Q: ) Determine the cell potential, Eo, for an electrochemical cell described by the following cell…

A:

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

A: Given-> [MnO4-] = 3.06 M [H+] = 1.02 M [Mn2+] = 4.19 M [Pb2+] = 2.07M

Q: 11.)

A: We have given that From representation of the cell reaction  Oxidation half reaction :  Zn(s)…

Q: [A4] Consider: Ag2S(ag) + Au(s) → 2Ag(s) + S2-(ag) + Au3+ + S2- (a0) + Au³+ (ag) (a) write out the…

A: Given reaction is :  Ag2S (aq) + Au (s) -------> 2Ag (s) + S2- (aq) + Au3+ (aq)  a) Write out the…

Q: [A4] Consider: Ag2S(ag) + Au(6) → 2Ag) + S2- + S2-(a0) + Au³+ (aq) (a) write out the reduction…

A:

Q: A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) ||…

A: Half Cell Reaction is the way of writing both oxidation and reduction half part of the reaction and…

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: The following reaction occurs in an electrochemical cell: 3 HCIO,(aq) + 2 Cr³* (aq) + 12 H2O(e) → 3…

A: Given: The concentration of Cr2O72-, HClO2, and [HClO] is 0.80 M, 0.15 M and 0.20 M, respectively.…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3669 V at 25 C Pt(s) / H2 (g, 0.723…

A: We will use nernesy equation to get the answer

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

A: Standard reduction potential of nickel = -0.257 V  Standard reduction potential of silver = 0.7996 V…

Q: Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems…

A: The question is based on the concept of electrochemistry.   the electrode which has higher reduction…

Q: A voltaic cell is constructed that uses the following reaction and operates at 298 K. (a) What is…

A:

Q: Given the following standard electrode potentals: Ag°(aq) + e¯ = Ag(s) N,(g) + 5H°(aq) + 4e° =…

A: Consider the given values as; Ag+ aq + e- ⇌ Ag s…

Q: Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for…

A:

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.