Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

On the basis of the standard electrode potential values states for acid solution, predict whether Ti^(4+) species may be used to oxidise Fe^(2+) to Fe^(3+) .

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Ag^+ (aq) and Cu(s)

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Ag(s) and Fe ^(3+) (aq)

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Br_2 (aq) and Fe^(2+) (aq) .

Give the technical terms used for the following: The difference between chemical potential of water at any point in a system and that of pure water under standard conditions.

Tarnished silver contains Ag_2S . Can this tranish be removed by placing tranished silver articels in an aluminium pan containing an inert electrolyte solution such as NaCl? The standard electrode potentials for the half cell reactions are: Ag_2S(s)+2barerarr2Ag(s)+S^(2-)(aq) , E^@=-0.71V and Al^(3+)+3barerarrAl(s) , E^@=-1.66V .

The standard reduction potentials for two reactions are given below: AgCl(s)+barerarrAg(s)+Cl^(-)(aq) , E^@=0.22V and Ag^(+)(aq)+barerarrAg(s) , E^@=0.80V The K_(sp) of AgCl under standard conditions of temperature is given by

Can Fe^(3+) oxidise Br^- to Br_2 under standard conditions? E_(Fe^(3+)|Fe^(2+))=0.771V , E_(Br_2|Br^-)=1.09V .