Using the standard electron potentials given in the Table 8.1, predict if the reaction between the following is feasible :
(a) `Fe^(3+) (aq) and I^(-) (aq)`
(b) `Ag^(+)(aq) and Cu(s)`
(c) `Fe^(3+) (aq) and Cu (s)`
(d) `Ag(s) and Fe^(3+)(aq)`
(e) `Br_(2) (aq) and Fe^(2+) (aq)`

Using the standard electrode potentials predict if the reaction between the following is feasible. (a) Fe^(3+) (aq) and I_(aq)^(-) (b) Ag_(aq)^(+) and Cu_(s)

Using the standard electrode potentials predict if the reaction between the following is feasible. a) Fe_((aq))^(3+) and I_((aq))^(-) b) Ag_((aq))^(+) and Cu_((s)

The cell reaction of the galvanic cell, Cu(s) // Cu^(2+)(aq) // Hg^(2+) (aq) // Hg (l) is

What is the effect of added sodium thiocyanate on the following equilibrium? Fe^(3+) (aq)+SCN^(-) (aq) leftrightarrow [FeSCN]^2+(aq)

Calculate the standard cell potentials of galvanic cell in which the following reactions take place. (i) 2Cr(s) + 3Cd^(2+)(aq) to 2Cr^(3+) (aq) + 3Cd (ii) Fe^(2+)(aq) + Ag^(+)(aq) to Fe^(3+)(aq) + Ag(s) Calculate the ΔrG and equilibrium constant of the reactions.

The standard reduction potentials at 298 K for the following half cell reactions are given below Zn^(2+) (aq) + 2e^(-) to Zn (s)-0.762 Cr^(3+) (aq) + 3e^(-) to Cr (s)-0.740 2H^(+) (aq) + 2e^(-) to H_(2) (g)-0.000 Fe^(3+) (aq) + e^(-) to Fe^(3+) (aq)-0.770 Which one is the strongest reducing agent?

Identify A and B respectively in the following reactions : 4Au(s)+8CN^(-) (aq)+2H_(2)O (aq) overset(O_(2)(g))(rarr) A(aq)+4 OH^(-) (aq) overset(Zn (s))(rarr) B+2 Au (s)

Write the cell reaction taking plce in the cell CU_((s))|Cu_((aq))^(+2)||Ag _((aq))^(+) |Ag _((s))

The standard reduction potentials for the two half-cell reactions are given below : Cd^(2+) (aq) + 2e^(-) to Cd(s) , E^(0) = -0.40 V " "Ag^(+)(aq) + e^(-) to Ag(s) , E^(0) = 0.80 V The standard free energy change for the reaction 2Ag_((aq))^(+) + Cd_((s)) + Cd_((aq))^(2+) is given by