Question

hello, please can you please help with these questions, i will give a thumb for sure, thanks!

(x) When Iron (Fe) is added to a solution of CuSO4 no reaction occurs. What can you deduce about the standard electrode potentials of Fe/Fe2+ and Cu/Cu2+ from this fact?

1. (xi) A plastic container of nickel sulfate (NiSO4) solution develops a leak and the solution comes into contact with a steel machine part. What would happen?

   Fe2+ Ι Fe = -0.44V; Ni2+ Ι Ni = -0.25V

2. (xii) Calculate the mass of Zn deposited at the cathode after a current of 0.5 A was passed for 6 min through an electrolytic cell containing zinc sulfate (ZnSO4 ≡ Zn2+ SO42-)

3. Some ionic solids such as AgCl are very insoluble in water whereas some a very soluble (KCl) explain the different behaviour.

Answer 1

x) From this fact, it can be concluded that the reduction potential of Fe^{​​​​​2+}/Fe couple is definitely greater than the Reduction Potential of the Cu^{​​​​​2+}/Cu couple. That's why, Fe isn't Oxidized and Cu^{​​​​​2+} isn't reduced.

xi) Since, the Reduction Potential of Ni^{​​​​​2+}/Ni couple is greater than that of Fe^{​​​​​2+}/Fe couple, Ni^{​​​​​2+} will oxidise Fe to Fe^{​​​​​2+}, and itself get reduced to Ni.

xii)