Identify the oxidants and reductants in the following reactions.
a. `CH_4(g)+4 Cl_2(g) rarr C Cl_4(g)+4 HCl(g)`
b. `2 H^+(aq)+MnO_2(s)+C_2 H_2 O_4(aq) rarr Mn^(2+)(aq)+2 CO_2(g)+2 H_2 O(l)`
c. `Cl_2(g)+2 Br^-(aq) rarr 2 Cl^-(aq)+Br_2(aq)`

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)

Identify the oxidant and reductant in the following reactions. a) 'Zn(s)+ 1/2 O_2(g) rarr ZnO(s)' b) 'C H_4(g)+4 Cl_2(g) rarr CCl_4(g)+4 HCl(g)' c) 'I_2(a q)+2 S_2 O_3 ^(2-)(a q) rarr 2 I(a q)+S_4 O_6^(2-)(a q)' d) 'Zn(s)+2 H^+(a q) rarr Z n^(2+)(a q)+H_2(g)'

Identify the limiting reagent in the above reaction. Zn_(s) + HCl_(aq) rarr ZnCl_(2(aq)) + H_(2(g))

Justify that the following reaction is a redox reaction H_2S_(g) + Cl_(2(g)) rarr 2HCl_(g) + S_(s)

Predict the sign of entropy change in the following reactions. i) O_2(g)+2 SO_2(g) rarr 2 SO_3(g) ii) 2 H_2(g)+O_2(g) rarr 2 H_2 O(g)

Identify the oxidant and reduction in the following ionic equation and balance it using oxidation number method MnO_4(aq) +Br^(-)(aq) H^(+) (aq) rarr Mn^(2+) (aq) +Br_(2) (I) +H_2O (I)

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

Complete the following equations. CH_3CH_2Cl + KOH_(aq) rarr ……….. + ……….

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)'

Write the oxidation state of each element and identify the oxidising agent and reducing agent in the following reaction : H_2S (g)+ Cl_2(g)rarr 2HCl(g)+ S(s)