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)

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) .

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+) .

The standard electrode potential for Daniell cell is 1. IV. Calculate the standard Gibbs energy for the reaction: Zn(s) + Cu^(2+) (aq) rarr Zn^(2+)(aq) + Cu(s)

Complete the following reaction : CH_3 CH_2 Br + KOH(aq) to

Complete the following reaction : Fe_2O_3 + Al rarr

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+) ?

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 .

Consider the following standard electrode potentials and calculate the eqillibrium constant at 25^(@) C for the indicated disproportional reaction : 3 Mn^(2+)(aq)toMn(s)+2Mn^(3+)(aq) Mn^(3+)(aq)+e^(-)toMn^(2+)(aq), E^(@)=1.51 V Mn^(2+)(aq)+2e^(-)toMn(s), E^(@)=-1.185 V