Consider the following standard reduction potentials in acid solution: E degree
ID: 530471 • Letter: C
Question
Consider the following standard reduction potentials in acid solution: E degree (V) Al^3+ + 3e^- rightarrow Al(s) -1.66 AgBr(s) + e^- rightarrow Ag(s) + Br^- +0.07 Sn^4+ + 2e^- rightarrow Sn^2+ +0.14 Fe^3+ + e^- rightarrow Fe^2+ +0.77 The strongest oxidizing agent among those shown above is (1)Fe^3+ (2) Fe^2+ (3)Al^3+ (4) Al Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl_4(g) + 1/2 O_2(g) COCl_2(g) + Cl_2(g), K_c = 4.4 times 10^9 at 1,000 K Calculate K_c for the reaction 2CCl_4(g) + O_2(g) 2COCl_2(g) + 2Cl_2g). (1) 1.9 times 10^19 2) 4.4 times 10^9 (3) 8.8 times 10^9 (4) 1.9 times 10^10 What is the reduction half-reaction for the following overall galvanic cell reaction? Ni^2+(aq) + 2Ag(s) rightarrow Ni(s) + 2Ag^+(aq) (1) Ni(s) rightarrow Ni^+(aq) + 2e^- (2) Ni^2+(aq) + 2e^- rightarrow Ni(s) (3) Ag(s) rightarrow Ag^+(aq) + e^- (4) Ag^+(aq) + e^- rightarrow Ag(s) Identify the conjugate acid of HPO_4^2- (1) H_2O (2) H_2PO_4^- (3) H_3PO_4 (4) PO_4^3-Explanation / Answer
23.As the standard reduction potential increases the strength of oxidizing agent increases.
Among the given the reduction potential of Fe3+ is more (+0.77V),so Fe3+ is having strongest oxidizing agent.
Therefore option (1) is correct.