What is the oxidation state of C in CO2?

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

Consider the following equilibrium system:                                                                CaCO3(s)  ⇄ CaO(s) +  CO2(g)             Which one of the following changes would cause the above system to shift leftwards (towards reactant)?

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.

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)

A standard hydrogen electrode (SHE) is shown in the following figure. What are the standard conditions (A, B and X) for the SHE-cell Question 33.docx

Consider the following half-cell reactions: Zn2+(aq)  +  2e-  ↔  Zn(s)  Ecell = -0.76 V Cu2+(aq)  +  2e-  ↔  Cu(s)  Ecell = +0.34 V If a cell is built by combining above two half-cells, what will be its cell potential?  Hint: The half-cell with the highest positive potential gets reduced: Ecell= E(cathode) – E(anode)

Which statement is true regarding a half-cell potential of a reaction

Which of the following metal ion gives the highest acidity in water?

In the diagram shown, if A was Cu metal and B was Mg metal, what would be the cell potential of this electrochemical cell? Use: Cu2+(aq)  +  2e-  = Cu(s)       Ecell = +0.34 V Mg2+(aq)  +  2e-  = Mg(s)     Ecell= -2.36 V Please open the file Question 20.docx