Mg 2+ (MgSO 4 ) Summarize the redox reactions that you observed in this investig

Question

Mg2+ (MgSO4)

Summarize the redox reactions that you observed in this investigation. List the reactions in descending order of activity, referring to Data Table 1.
For each reaction in the data table, perform the following steps:

• Write the overall single-displacement reaction.

• Write the half-cell reaction for oxidation.

• Write the half-cell reaction for reduction.

• Add the two half-cell reactions, and write the net ionic equation.

• Identify the reducing agent.

• Identify the oxidizing agent.

After identifying the reaction, use the following format to report the information:

Overall reaction:

Oxidation:

Reduction:

Net ionic reaction:

Reducing agent:

Oxidizing agent:

metal tested

Mg2+ (MgSO4)

Fe2+ (FeSO4) Cu2+ (CuSO4) no of reactions mg(s) no reaction mg rusted, orange color for solution bubbles , black solution, black mg 5 Fe(s) no reaction fe turned black, bubbles formed fe rusted 3 Cu(s) no reaction no reaction no reaction 0

Explanation / Answer

From the observation

i)Mg is most reactive as Mg(s) can reactabd replace both Fe+2 and Cu+2 from their solutions

ii) Cu (s) is the least reactive, as it can not react/replace both Mg+2 and Fe+2 from their solutions.

iii) Fe(s) can replace only Cu+2 but not Mg+2 from its solution.

Thus the order of reactivity of metals = Mg > Fe > Cu

Q2)

1)Net reaction Mg(s) + FESO4(aq) ------------> MgSO4 (aq) + Fe(s)

oxidation rxn Mg(s) ----------> Mg+2 + 2 e-

reduction rxn Fe+2 + 2e- ---------> Fe(s)

net ionic reaction Mg + Fe+2 ----------> Mg+2 + Fe

oxidizing agent fe

reducing agent Mg

2)

Net reaction Mg(s) + CuSO4(aq) ------------> MgSO4 (aq) + Cu(s)

oxidation rxn Mg(s) ----------> Mg+2 + 2 e-

reduction rxn Cu+2 + 2e- ---------> Cu(s)

net ionic reaction Mg + Cu+2 ----------> Mg+2 + Cu

oxidizing agent Cu

reducing agent Mg

3)Net reaction Fe(s) + CuSO4(aq) ------------> FeSO4 (aq) + CU(s)

oxidation rxn Fe(s) ----------> Fe+2 + 2 e-

reduction rxn Cu+2 + 2e- ---------> Cu(s)

net ionic reaction Fe + Cu+2 ---------->Fe +2 + Cu

oxidizing agent Cu

reducing agent Fe

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