15. What is the balanced spontaneous reaction and standard cell potential of an

Question

15. What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions? Cu"(aq) + 2e- Cu(s) E' = 0.337 V Pbt (a)+2ePb(o) -0.130 V a. Cu?"(aq) + Pb(s) Cu(s) + Pb2. (a): 0.467 V b. Cu(s) + Pb"(aq) Cu2+(aq) + Pb(s);-0.467 V C. Cu?"(aq) + Pb?"(aq) Cu(s) + Pb(s); 0.207 V d. Cu2+(aq) + pb(s) Cu(s) + Pb?"(aq); 0.234 V e. Cu(s) + Pb?"(aq) Cu2.(aq) + Pb(s);-0.234 V 16. Given: Lit(aq)eL(s) E -3.04 V Mg"(aq) + 2e-=-Mg(s); E=-2.38 V Fe"(aq) + 2e Fe(s); E.--0.41 V Ag"(aq) + e Ag(s); E= 0.80 V Br:0 + 2e--2Br(a): E' = 1.07 V Which of the following species is the best oxidizing agent? a. Mg2* b. Br c. Fe2 d. Li e. Ag 17. For a certain oxidation-reduction reaction, Ece is negative. This means that a. AG" is positive and K is less than 1. b. AG is negative and K is greater than 1. c.aG" is positive and K is greater than 1. d. AG is negative and K is less than 1. e. AG is zero and K is greater than 1.

Explanation / Answer

15. Pb(s) --------> Pb^2+ (aq) + 2e^-             E0 = 0.13v
    Cu^2+ (aq) + 2e^- ------> Cu(s)               E0 = 0.337v
----------------------------------------------------------
    Pb(s) + Cu^2+ (aq) -----> Pb^2+ (aq) + Cu(s) E0cell= 0.467v
a.Pb(s) + Cu^2+ (aq) -----> Pb^2+ (aq) + Cu(s) E0cell= 0.467v>>>>answer
16.The more positive reduction potential ion is strong oxidizing agent.
e. Ag^+ >>>>answer
17.DG^0 = -nE0cell*F
   DG^0 = -RTlnK
a.DG^0 is positive and K is less than 1

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