A sample containing the following was prepared: For this sample, the following b

Question

A sample containing the following was prepared: For this sample, the following balanced half-reactions and net reaction can occur: C) Calculate the value of E for this system at equilibrium. D) Determine the pH at which the given concentrations of Pb2+, Pb4+ Mn2+, and MnC Less than 4 would be at equilibrium. For part A, pay attention to the number of electrons transferred in this reaction. Examine the hatf-reactions to determine the value of n. Determine E degree from the half-reaction standard reduction potentials. To find the value of the cell potential (E) for part B, first determine the value of E+ and E_ using the Nernst equation with the given ion concentrations and take their difference. At equilibrium, there is no net transfer of electrons. Remember, E differs from E degree . Part D is solved by using the Nernst equation for the net reaction at equilibrium and the given ion concentrations, then solve for H+

Explanation / Answer

?G0=-nFE0=-10*96485*0.183=-176.567 kJ

K=e-?G/RT=e176567/8.314*298=8.92*1030

=0.183 -0.059/10 ln(0.115*0.112*0.8816/(1.5*10-6)5*[1.5*10-6]2)

=0.183-0.379=-0.196 V

?G=-nFE=-10*96485*-0.196=189.559 kJ

0.183*10/0.059= ln(0.115*0.112*[H+] 16/(1.5*10-6)5*[1.5*10-6]2)

1.83/0.059=ln[H+]16+ln 1.14*1034

                -log[H+]=1.28

pH=1.28

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