6. In the laboratory, you place a few drops of aqueous magnesium nitrate into th

Question

6. In the laboratory, you place a few drops of aqueous magnesium nitrate into three wells in a well plate. To the first well, you add a few drops of magnesium chloride. To the well, add a few drops of second you calcium chloride, To the third well, you add a few drops of lead iodide. For the well that undergoes a redox reaction, write the balanced molecular and net ionic equation and oxidation and reduction half reactions, calculate the Ecell value, and determine spontaneity. (3pts) Balanced Molecular Equation (3pts) Net Ionic Equation (4pts) oxidation & Reduction Half Reactions (label)

Explanation / Answer

Magnesium Nitrate --> Mg(NO3)

1) Magnesium Chloride --> MgCl2

2) Calcium Chloride --> CaCl2

3) Lead II Iodide --- >PbI2

redox reaction....

the only possible reaction is that of Pb+2 and Zn+2 ions...

so

redox reaction:

Pb2+ + 2 e Pb(s) 0.126

Mg2+ + 2 e Mg(s) 2.372

Then.... Pb will reduce, and Mg should oxidize ( lowest potential)

The net ionic equation

Pb+2(aq) + Mg(s) ----> Mg+2(aq) + Pb(s)

For REDOX:

Pb2+ + 2 e Pb(s) 0.126 --> reduction/cathode

Mg(s)  Mg2+ + 2 e +2.372 --> oxidation/anode

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