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

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)

Identify the oxidising and reducing agents in the reaction: Cus +O_2 rarr Cu+SO_2

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)'

Identify the substance oxidised, reduced, oxidising agent and reducing agent in the reaction: 2Cu_2O+ Cu_2S rarr 6Cu+SO_2

Identify the substance oxidised, substance reduced, oxidising agent and reducing agent in the reaction: Cl_2 +2I^(-) -- I_2 +2Cl

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

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 substance oxidised, substance reduced, oxidising agent and reducing agent in the reaction. MnO_2 + 4HCl rarr MnCl_2 + Cl_2 + 2H_2O

Which of the following condition will increase the voltage of the cell, represented by the equation? Cu(s)+2Ag^(+) (aq) rarr Cu^(2+) (aq) + 2Ag(s)