Two half-cells are shown below: Fe2+(aq) + 2e- ↔ Fe(s) …
Two half-cells are shown below: Fe2+(aq) + 2e- ↔ Fe(s) Ecell = – 0.44 V Cu2+(aq) + 2e- ↔ Cu(s) Ecell = +0.34 V Hint: The half-cell with the highest positive potential gets reduced. the other half-cell must get oxidized. The complete cell reaction is
Read DetailsConsider the following half-cell reactions: Zn2+(aq) + 2e-…
Consider the following half-cell reactions: Zn2+(aq) + 2e- ↔ Zn(s) Ecell = -0.76 V Cu2+(aq) + 2e- ↔ Cu(s) Ecell = +0.34 V Identify the species (element or ion) that is acting as the oxidizing agent Hint: The half-cell with the highest positive potential gets reduced
Read DetailsTwo half-cell reactions are shown below: Fe2+(aq) + 2e- …
Two half-cell reactions are shown below: Fe2+(aq) + 2e- ↔ Fe(s) Ecell = – 0.44 V Cu2+(aq) + 2e- ↔ Cu(s) Ecell = +0.34 V Hint: The half-cell with the highest positive potential gets reduced. the other half-cell must get oxidized. Find the Gibbs free energy for the above cell reaction (ΔG = -nFE: F = 96485 C, n = no. of electrons and E = cell potential). Use the cell voltage you received in questions 21.
Read DetailsLi-ion batteries are well known. The reaction of a Li-ion ba…
Li-ion batteries are well known. The reaction of a Li-ion battery is shown below LiCoO2 + C6 ↔ Li1-xCoO2 + LixC6 Forward reaction occurs during the charging process, and the reverse reaction (discharge) occurs when the battery is in use. What is the oxidation state of Co in the LiCoO2 species? (Hint: Li has the same oxidation number as other elements in the same group)
Read Details