Given the partial pressure of H2 (g) PH2 = 0.0500 atm, [Cd2+] = 0.150 M and the pH of the cell is 2.34. Calculate E at 25°C for a cell based on the reaction:                               Cd(s) + 2 H+(aq) → H2(g) + Cd2+(aq)  E° = +0.400 V.

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: Fe³+ (aq) + e 2 103(aq) + 12 H (aq) + 10e answer the following questions about this cell. Write a…

A: Given:We have to determine Cathode half-reactionAnode half-reactionOverall balanced equationCell…

Q: 1.calculate of the change in Gibbs' free energy to the formation of the silver ion (Ag+(aq)) ∆°Gf…

A: 1.

Q: A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential…

A: In an electrochemical cell, the electrode with higher standard reduction potential acts as a cathode…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.828 M…

A:

Q: The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq)   Calculate the…

A: Answer: The free energy change for the given reaction is0 J/moland the cell potential is-1.35 Vat…

Q: Answer the following questions about this cell. If you need any electrochemical data, be sure you…

A:

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: Given the following half-reactions and half-cell potentials, write the balanced overall…

A:

Q: Given the following standard reduction potentials: Half reaction E° (V) Cr3*(aq) + 3e → Cr(s) -0.740…

A:

Q: Using the following standard reduction potentials, Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Cu2+(aq) +…

A: The standard cell potential (Eocell) for the cell is determined  using the following equation…

Q: Calculate the gibbs free energy (ΔGo)  in kilojoules (KJ) for ColCo2+ II Cd2+I Cd   The faraday…

A: In an electrochemical cell, the electrode with higher electrode potential acts as cathode. The…

Q: 6. Consider the following cell. Al(s) | Al³* (1 M) || OH- (1 M) | Al(OH)3(s), Al(s) Given the Ksp…

A:

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Half reaction at cathodeelectrode which has more reduction potential act as cathode. 2Cl 2(g) + 2e →…

Q: A galvanic cell reaction transfers 4 electrons as it proceeds. Calculate ΔGº in kJ/mol if the Eº for…

A: Standard cell potential (E°) = +0.589 V = +0.589 J/C Faraday constant (F) = 96485 C/mol Number of…

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: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A: For a cell   Cell potential = E°Reduction half  - E°Oxidation half Species whose reduction potential…

Q: Consider the following standard reduction potentials: Al³+ (aq) + 3e-→→ Al(s), Eº = -1.66 V AgBr(s)…

A: The species which undergo oxidation and help other species to undergo reduction are called…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A:

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: A chemist designs a galvanic cell that uses these two half-reactions: Br₂(1)+2e Cro(aq) +4H₂O(1)+3e¯…

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

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

A: Redox reaction are those in which both oxidation and reduction take place simultaneously.

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: A reaction is spontaneous when the cell potential is positive. Reduction takes place at cathode and…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The standard free energy change is also known as Gibb's free energy change. It is denoted by symbol…

Q: A solution of Mno is electrolytically reduced to Mn3+. A current of 7.79 A is passed through the…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: Representation of a galvanic cell (Cell notation) i.Galvanic cell consists of two electrodes, anode…

Q: Calculate the free energy, AG°, (kJ/mol) for the galvanic cell performing the following reaction as…

A: Oxidation is the loss of electrons. Reduction is the gain of electrons. The reactions where…

Q: A galvanic cell was created using the following electrode reactions. Anode half-cell: Co(s) + 3…

A:

Q: Use standard reduction potentials to calculate the standard free energy change (ΔGº) for the…

A: The standard reduction potential is the reduction potential of a molecule which measures the…

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: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A:

Q: Consider the following electrochemical cell reaction:   Pb2+(aq)  +  2 Cr2+(aq)  →  Pb(s)  +  2…

A: We will calculate cell potential using nernst equation.

Q: A galvanic cell is powered by the following redox reaction: Cl,(g) + H,(g) + 2 OH (aq) → 2 Cl (aq) +…

A: Given : We have to write half reaction taking place at anode and cathode.

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

A:

Q: A voltaic cell utilizes the following redox reaction and operates at 298 K: 3 Ce¹+ (aq) + Cr (s) → 3…

A:

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: A galvanic cell is powered by the following redox reaction: 3+ NO3(aq) + 4H* (aq) + 3 Fe²+ (aq) →…

A: Redox reactions contain both reduction and oxidation reactions. One of the compounds is oxidized and…

Q: Sketch the galvanic cell based on the following overall reactions. Calculate e°; show the direction…

A: The standard reduction potentials of the two half-cells are: Cl2/2Cl-: 1.36 VCr2O72-/Cr3+:1.33 V

Q: Write the balanced equation for the overall reaction that occurs in the cell. Calculate E ̊ for the…

A: The reaction with smaller standard electrode potential, that reaction occurs at anode and reaction…

Q: For the electrochemical cell, Cd(s) | Cd2*(aq) || Co2*(aq) | Co(s), determine the equilibrium…

A: In this question, we will determine the value of Keq ( equilibrium constant) value. First we will…

Q: If the concentration of Ag* is 0.0115 M, the concentration of H* is 0.355 M, and the pressure of H2…

A: Use Nernst equation, to get the cell potential:

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.