The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq)   Calculate the free energy change and the cell potential for the reaction at 298.0 K if all reactants are at 2.00 M and/or 2.00 atm and all products are at 0.0100 M and/or 0.0100 atm

Q: 4) Using the following standard reduction potentials, Fe3+ (aq) + e- →→ Fe2+(aq) E° = +0. 77 V…

A: Standard reduction potential,Fe3+(aq) + e- -----> Fe2+(aq)  E° = +0.77 VNi2+(aq) + 2e- ------>…

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Interpretation -  To calculate the experimental standard cell potential, Eocell for the reaction…

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: For cell Ni|Ni2+||Ag+|Ag At anode- Ni(s) -----> Ni2+(aq) + 2e-       ∆E° = 0.23 V At cathode-…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Given-> [Cr2+] = 0.790 M [Fe2+] = 0.0190 M T = 25°C

Q: At 25 oC, if the potential of a Zn–H + cell is 0.55 V at 25oC when [Zn2+] = 1.0 M and PH2 = 1.0 atm,…

A: Given Temperature = 25°C = (25 + 273.15)K = 298.15 KGiven Cell Zn-HCell reaction Zn(s)    +   2H+…

Q: student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

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

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: The Relation between cell potential and free energy change is given by: Ecell can be determined from…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Cr(s)+Fe+2 (aq )<==>  Cr+2 (aq)+Fe(s) [Cr+2] = 0.768 M [Fe+2] = 0.0170 M

Q: Calculate ΔG for the following cell reaction:  3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s)       where…

A: Concept:  For a cell reaction: The overall cell potential can be calculated by using the equation…

Q: The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3…

A:

Q: A galvanic (voltaic) cell consists of an electrode composed of cadmium in a 1.0 M cadmium ion…

A: Given: Cd2+aq+2e-→Cds; ECd2+|Cd0=-0.403 VCo2+aq+2e-→Co(s): ECo2+|Co0=-0.28 V

Q: Based on the following information 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)  Eºcell=0.71 V What is the…

A: Nernst equation is  Ecell = E0cell - 0.059n × log Q  Q = reaction quotient  n = number of electrons…

Q: The free energy change for the following reaction at 25 °C, when [Cd²+] = 2.15×10-³ M and [Ni2+] =…

A: It is given that standard Gibb's free energy, ∆G = 45.0 KJ

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: Given : half cell reaction and their reduction potential

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: Reduction ----> when oxidation state of an element decreases oxidation----> when oxidation…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A:

Q: Calculate the change in standard Gibbs energy (AC), in kilojoules, for the reaction below at 25 °C.…

A:

Q: Calculate E° and Ecell (at 25 °C) for the following cell reaction: Mg (s) + Sn2+ (aq) → Mg2+ (aq)…

A: Given, Sn2+ (aq) → Sn (s)             E°= ‒0.14 V Mg2+ (aq) → Mg  (s)          E°= ‒2.37 V

Q: voltaic cell reaction at 298 K: 3Ce4+(aq) + Cr(s) → 3Ce3+(aq) + Cr3+(aq) Given: Ce4+ (aq) + e- →…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.864 M and…

A: The cell potential for a reaction can be calculated by using Nernst's equation as…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A:

Q: The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for…

A: Given,   2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq)   We need to Calculate the following for the…

Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

A:

Q: The following half reactions are used for a galvanic cell: Zn2+(aq)+2e-→Zn(s)E°=-0.76V…

A: Nerst Equation:Where,E is the cell potential under non-standard conditions.E∘ is the standard cell…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.807 M and…

A:

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Given that : A student constructs an electrochemical cell with a half-cell composed of a nickel…

Q: What would be the cell reaction and standard cell potential of a galvanic cell employing the…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M…

A: Given data :  Cr(s) + Fe2+ (aq) ==> Cr2+(aq) + Fe(s)  From table :  E(Fe2+/Fe) = -0.44 V…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

A:

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…

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.