Asked by katya
consider the cell
Pt(s)I H2 (g. 0.100 bar)I H+ (aq, pH= 2.54)IICl^- ( aq, 0.200 MI Hg2Cl2(S)IHg (l)IPt(s)
a. write a reduction reaction and nernst equation for each half- cell. For the Hg2Cl2 half reaction, E^0 = 0.268 V
b. Find E for the net cell reaction and state whether reduction will occur at the left ot right hand electrodes
Pt(s)I H2 (g. 0.100 bar)I H+ (aq, pH= 2.54)IICl^- ( aq, 0.200 MI Hg2Cl2(S)IHg (l)IPt(s)
a. write a reduction reaction and nernst equation for each half- cell. For the Hg2Cl2 half reaction, E^0 = 0.268 V
b. Find E for the net cell reaction and state whether reduction will occur at the left ot right hand electrodes
Answers
Answered by
DrBob222
I'm sure you know the equation for the H2.
2H^+ + 2e ==> H2(g)
E=Eo-(0.059/n)*log(pH2/H^+) but you need to add the partial pressures and concentrations to that. Here is a site you can read about the SCE.
http://en.wikipedia.org/wiki/Saturated_calomel_electrode
2H^+ + 2e ==> H2(g)
E=Eo-(0.059/n)*log(pH2/H^+) but you need to add the partial pressures and concentrations to that. Here is a site you can read about the SCE.
http://en.wikipedia.org/wiki/Saturated_calomel_electrode
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