The standard emf for the cell using the overall cell reaction below is +0.76 V:               Ag+(aq) + K(s) → Ag(s) + K+(aq)   The emf generated by the cell when [Ag+] = 6.2 × 10-3 M

Q: Mg(s) + Fe2+(aq) – Mg2+(aq) + Fe(s) The galvanic cell described above has a standard cell potential…

A: Galvanic cell is electrochemical cell where, current is supplied to carry out some chemical…

Q: Consider the following cell: Cu(s) | CuCl2(0.025 M) || FeCl2(0.055 M) | Fe(s)

A: Given:  Concentration of CuCl2 = 0.025 M  Concentration of FeCl2 = 0.055 M

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

A:

Q: Consider the voltaic cell: Sr(s)|Sr²+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reactions…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² +] = 0.755 M…

A: Given,

Q: From the following 4 equations can you produce a spontaneous cell? Calculate the cell with the…

A: The 4 half-reactions given are, 1) Br2 (l) + 2 e- → 2 Br- (aq)                                Eo =…

Q: The voltaic cell described by the notation below measured a potential of 1.1 V. If the reaction was…

A: The given cell notation for the voltaic cell is:- Pt(s) | J2- (1.50 M) | J(l) || Ag+ (0.010 M) |…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2+]=0.790 M and…

A: Cell potential calculation:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+…

A:

Q: A galvanic cell is made ot a Ni2*/Ni halt cell with [Ni2 | = 6.00 x 10-2 M and an Ag"/Ag half cell…

A: This is the concept of electrochemistry

Q: Consider the following reaction and its AG° at 25.00 °C. 2 Ag*(aq)+Cu(s) → 2 Ag(s) + Cu2+(aq) AG° =…

A: ∆G = -88.66 KJ/mol = -88660 J/mol  Temperature (T) = 25°C = 25+273 = 298 K  R = 8.314 J/mol.K  Keq =…

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell…

A:

Q: The standard cell potential (E° cell) for the reaction below is +0.63 V. The cell potential for this…

A:

Q: Alkaline dry-cell batteries have a voltage of 1.50 V under standard conditions. Given this standard…

A: Common flashlight batteries are called dry-cell batteries since they do not contain large amounts of…

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.