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)'

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) .

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 reactions: a) '2 Fe^(3+)(aq)+2 I-(aq) rarr 2 Fe^(2+)(aq)+l_2(aq)' b) 'Zn(s)+2 H^+(aq) rarr Zn^(2+)+H_2(g)' c) 'Al(s)+3 Ag^+(Aq) rarr Al^(3+)(aq)+ 3 Ag(s)'

Balance the following equation by the half reaction method. Fe^(2+) (aq) + Cr_2O_7^(2-) (aq) +H^(+) (aq) rarr Fe^(3+) (aq) + Cr^(3+) (aq) +H_2O (I)

Predict the sign of entropy change for each of the following changes of state a) 'Hg(l) rarr Hg(g)^circ' b) 'AgNO_3(s) rarr AgNO_3(aq)' c) 'I_2(g) rarr I_2(s)' d) 'C' (graphite) 'rarr C' (diamond)

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 .

Write half equations for each of the following redox reactions: i) 'Zn(s)+PbCl_2(aq) rarr Pb(s)+ZnCI_2(aq)' ii) '2 Fe^(3+)(aq)+2 I-(aq) rarr I_2(aq)+2 Fe^(2+)(aq)' iii) '2 Na(s)+Cl_2(g) rarr 2 NaCl(s)'

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

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

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)