Question

14) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Agt in the balanced reaction? 14) - Cd(s) + Agt(aq) → Ag(s) + Cd2+(aq) A) Cd = 2, Agt = 2 B) Cd = 3, Agt = 1 Cd = 1, Ag - 2 D) Cd -2, Agt = 1 E) Cd = 1, Ag+ - 1 15) What is undergoing oxidation in the redox reaction represented by the following cell notation? 15) Pb(s) | Pb2+(aq) | H+(aq)H2(g) Pt ^) Pb(s) B) Hz(6) C) Pt D) H+ (aq) E) Pb2+ (aq)

Answer 1

14) It is a redox (Reduction - Oxidation) reaction · Here, one species getz oxidized and other gets reduced. Taking electrons is reduction and giving electron is oxidation. In this reaction cd (s) has become čo + (aq) by giving ze. so the oxidation takes place. The oxidation reaction is Cd (5) ► cd" (aq) + 2e - 0 In the reaction Agic aq) has become Ag (s) by taking le.. Jo the reduction has taken place. The reduction reaction is, Agt (29) te → Mg(s) +® In Oxidation reaction 2e are released but in reduction reaction le is taken . So we have to balance the electron 1+2x@ 7 cd (s)-> cd?*(aq)+22 2 Ag*(ag)+ 2e —+2A9.Cs) 24gt (aq)+ Cd(s) 4 cd" (29)+ 2Ag (5) Balanced equation . Ag = 2, (dz! +© 15 the cell notation is the following Pb (5) 1 Pk?(aq) 11 H(aq) I H2(g)/Pt line represents Anode - half cell oxidation cathode half cell reduction . phase change 'll represents " salt bridge In anode the oxidation tanes place, the half cell ox?dation reachion is Pb(s) + P6**(12)+22 So here Pb(s) [A] is undergoing oxidakon.