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: Br_2 (aq) and Fe^(2+) (aq) .

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: Ag^+ (aq) and Cu(s)

Use the following standard electrode potentials, calculate DeltaG^(@) in kJ // mol for the indicated reaction : 5Ce^(4+)(aq)+Mn^(2+)(aq)+4H_(2)O(l)to5Ce^(3+)(aq)+ MnO_(4)^(-)(aq)+8H^(+)(aq) MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51 V Ce^(4+)(aq)+e^(=)toCe^(3+)(aq)" "E^(@)=+1.61 V

The equilibrium constant of the following redox reaction is 298K is 1xx10^8 2Fe^(3+)(aq)+2I^-(aq)Leftrightarrow2Fe^(2+)(aq)+I_2(s) If the standard reduction potential of iodine becoming iodide is +0.54V, what is the standard reduction potential of Fe^(3+)/Fe^(2+) ?

Calculate the reductoin potential of a half cell consisting of a platinum electrode immersed in 2.0M Fe^(2+) and 0.02M Fe^(3+) solution (E^@Fe^(3+)|Fe^(2+)=0.771V) .

For M^(2+)//M and M^(3+)//M^(2+) system the E^@ values for some metals are as folows : Use this data to comment upon : the stability of Fe^(3+) in acid solution as compared to that of Cr^(3+) or Mn^(3+) .

Calculate the electrode potential at copper electrode dipped in a 0.1 M solution of copper sulphate at 298K, assuming CuSO_4 to be completely ionised. The standard electrode potential of Cu^(2+)|Cu is 0.34V at 298K.

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 .

Fuel cells convert the energy produced during the combustion of fuels cells directly into electrical energy. Probably the most successful fuel cell so far is hydrogen oxygen fuel cell, which has ben used in spacecraft. The electrodes consist of porous screens of titanium coated with a layer of platinum catalyst. concentrated KOH or NaOH soloution is placed beween the electrodes to serve the as electrolyte. hydrogen and oxygen gases are bubbled through the porous electrodes into the electrolyte solution The following electrodes reactions occur: At anode: 2H_2(g)+4OH^(-)(aq)rarr4H_2O(l)+4bare At cathode: O_2(g)+2H_2O(l)+4barerarr4Oh^-(aq) Overall reaction: 2H_2(g)+O_2(g)rarr2H_2O(l) In this cell, the gaseous materials are consumed and continously supplied. The thermodynamic properties of fuel cell reaction at 25^@C are: DeltaH^@=-285.8kJ mol^-1,DeltaG^@=-237.2kJ mol^-1, E^@=1.23V If the potential of the half cell reaction is at cathode is, E^@=0.41V , then E^@ for the half cell reaction at anode is