Using the standard electrode potentials given : in Table 3.1( book), predict if the reaction between the following is feasible: i. `Fe^2`+(aq)` and `I-(aq)` ii. `Ag+` (a q)` and `Cu(s)` iii `Br_2(aq)` and `Fe^2+(aq) .`

Using the standard electrode potentials given in the text (Table 8.1), predict if the reaction between the following is feasible? a) 'F e^(3+)(a q)' and 'I^-(a q)' b) 'Ag^+(aq)' and 'Cu(s)' c) 'Fe^(3+)(aq)' and 'Cu(s)' d) 'A g(s)' and 'F e^(3+)(a q)' e) 'Br_2(aq)' and 'Fe^(2+)(aq)'

Write the half reaction for the following redox reaction. 2Fe^(3+)(aq) + 2l (aq) rarr I_2 (s) + 2Fe^(2+) (aq)

Write the half reactions for the following redox reaction. Zn(s) + 2H^+ (aq) rarr Zn^(2+) (aq) + H_2(g)

Find out the oxidising agent and reducing agent in the following reaction: Cu(s)+2Ag^(+) (aq)rarr Cu^(2+) (aq) + 2Ag(s)

Calculate the standard cell.potentials of galvanic cell in which the following reactions take place: Fe^2+(aq)+Ag+^*(aq)^* -> Fe^3+(aq)+Ag(s) Calculate the Delta r G^circ and equilibrium constant of the reactions.

Identify the oxidant and reductant in the following reaction: 2K_4[Fe(CN)_6](aq) + H_2O_2(aq) rarr 2K_3[Fe(CN)_6](aq) + 2KOH (aq)

Calculate the standard cell potentials of galvanic cell. Also calculate Delta G^0 and equilibrium constant of the following cell, reaction. Fe^(2+)(aq)+Ag^+(aq) rarr Fe^(3+)(aq)+Ag(s) E^0 Ag^+I Ag =0.80V,E^0 Fe^(3+)IFe^(2+)=0.77V .

The standard reduction potentials at 298K for the following half reactions are given against each. Zn^(2+) (aq)+2e= Zn(s), -0.762V Cr^(3+) (aq) +3e= Cr(s), -0.74V 2H^+ +2e=H_2 (g), pm 0.0V Fe^(3+) (aq)+e =Fe^(2+) (aq), +0.77V What is the strongest reducing agent?

Balance the following redox reaction by ion electron method MnO_4^- (aq) + I^- (aq) to MnO_2 (s) + I_2(s) (base medium)

Using the following E^(@) values for electrode potentials, calculate triangle G^(@) in kJ for the indicated reaction: 5Ce^(4+) (aq) + Mn^(2+) (aq) + 4H_(2)O(l) rarr 5Ce^(3+) (aq) + MnO_(4)^(-) (aq) +8H^(+) (aq) MnO_(4)^(-) (aq) +8H^(+) (aq) +5e^(-) rarr Mn^(2+) (aq) + 4H_(2) O(l), E^(@) = +1.51V Ce^(4+) (aq) + e^(-)rarr Ce^(3+)(aq), E^(@) = +1.61V