Question 17.13: Will a reaction occur when copper metal is placed in an iron...

No, copper lies below iron in the series, loses electrons less easily than iron, and therefore will not displace iron(II) ions from solution. In fact, the reverse is true. When an iron nail is dipped into a copper(II) sulfate solution, it becomes coated with free copper. The equations are

Cu(s) + FeSO_4(aq)→ no reaction

Fe(s) +CuSO_4(aq)→FeSO_4(aq) + Cu(s)

From Table 17.2, we may abstract the following pair in their relative position to each other:

Fe→Fe^{2+} + 2 e^-

Cu→Cu^{2+} + 2 e^-

According to Step 2 in Problem-Solving Strategy: Using the Activity Series, we can predict that free iron will react with copper(II) ions in solution to form free copper metal and iron(II) ions in solution:

Fe(s) + Cu^{2+}(aq)→Fe^{2+}(aq) + Cu(s) (net ionic equation)