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)'

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

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)'

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)

The equilibrium constant of the following redox reaction at 298 K is 1 xx 10^(8) 2Fe^(3+) (aq.)+ 2I^(-) (aq.) rarr 2Fe^(2+) (aq)+I_(2) (s) If the standard reduction potential of iodine becoming iodide is +0.54 V. What is the standard reduction potential of (Fe^(3+))/(Fe^(2+)) ?

Justify the following reaction is redox reaction Fe_2O_3 (s) + 3CO (g) to 2Fe (s) + 3CO_2 (g)

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 .

Identify the subtance oxidized, reduced, oxidizing agent and reducing agent ror each of the following reactions. a) '2 AgBr(s)+C_6 H_6 O_2(aq) rarr 2 Ag(s)+2 HBr(aq)+C_6 H_4 O_2(aq)' b) 'HCHO(l)+2[Ag(NH_3)_2]^+(a q)(+3) OH-(aq) rarr 2 Ag(s)+HCOO^-(aq)+ 4 NH_3(aq)+2 H_2 O(l)' c) 'HCHO(l)+2 Cu^(2+)(aq)+5 OH^-(aq) rarr Cu_2 O(s)+HCOO^-(aq)(+3) H_2 O(l)' d) 'N_2 H_4(l)+2 H_2 O_2(l) rarr N_2(g)+4 H_2 O(l)' e) 'Pb(s)+PbO_2(s)+2)H_2 SO_4(aq) rarr 2 PbSO_4(s)+2 H_2 O(I)'

Justify that the following reaction is a redox reaction: Fe_2O_3(s) + 3COg rarr 2Fe(s) + 3CO_2(g) ?

Complete the following reaction. (Zn_(s) + NaOH_(aq) rarr^(heat) ……………….)