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Question

Please answer these questions: All points will be rewarded if correct =]

Predict from the table of standard reduction potentials whether: Pb2+ can oxidize Cu(s) or Al(s). Br2 can oxidixe I- or Cl-. Which is the stronger oxidizing agent, Cl2(g) or Ag+? Which is the stronger reducing agent, Ca(s) or Mg(s)? Calculate the cell potential for the reaction below at 25 degree C if [H+] = 1.0 M, [Zn2+] = 0.0010 M, and PH2 = 0.10 atm. Zn(s) + 2H+(aq) rightarrow Zn2+ (aq) + H2(g) Calculate the equilibrium constant for the following reaction at 25 degree C Sn(s) + 2Cu2+(aq) rightarrow Sn2+ (aq) + 2 Cu+ (aq) Calculate the molar concentration of H+ (and the pH) for the reaction shown below. The emf, Ecell, for this cell is 0.54 V at 25 degree C Zn(s) + 2H+(?) rightarrow Zn2+ (1.0M) + H2(1 atm)

Explanation / Answer

6)a) it can oxidise Cu(s) but not Al(s)

b) it can oxidise I- but not Cl-

7) Cl2 (since Eo is greater)

8) Mg2+

9)Eo=0.76 V

so E=Eo-0.059/2 *log(0.001^2*0.1/1)

or e=0.76-0.059/2 *log(0.001^2*0.1/1)

=0.9665 V

10)Eo=0.14 + 0.16

=0.3 V

so 0.3=-0.059/2 *log(k)

or k=6.77*10^-11

11)Eo=0.76

so,

0.54=0.76-(0.059/2)log(1*1/x^2)

or x=1.87*10^-4 M

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