Chapter 7, Problem 10A

Interpretation Introduction

Interpretation: The unbalanced chemical equation for the reaction taking place by keeping a piece of pure zinc metal into a solution of copper(II) sulfate should be determined.

Concept Introduction: An unbalanced reaction is that chemical reaction in which the number of atoms of each element in the product side and on reactant side are not equal.

Answer to Problem 10A

The chemical equation is:

  ${\text{Zn(s) + CuSO}}_{\text{4}}\left(\text{aq}\right)\to {\text{ ZnSO}}_{\text{4}}\left(\text{aq}\right)\text{+ Cu (s)}$

Explanation of Solution

The elemental formula for zinc is $\text{Zn}$ .

The molecular formula for copper(II) sulfate is ${\text{CuSO}}_{\text{4}}$ .

The molecular formula for zinc sulfate is ${\text{ZnSO}}_{\text{4}}$ .

The elemental formula for copper is $\text{Cu}$ .

The physical state of the reactants and products are shown by writing the symbols after each reactant and product in the reaction. The symbol “l” represents liquid, “aq” represents aqueous, “s” represents solid, and “g” represents gas.

The reaction taking place by keeping a piece of pure zinc metal into a solution of copper(II) sulfate is written as:

  ${\text{Zn(s) + CuSO}}_{\text{4}}\left(\text{aq}\right)\to {\text{ ZnSO}}_{\text{4}}\left(\text{aq}\right)\text{+ Cu (s)}$

The reaction is already balanced as the number of each atom of each element on both the sides of the equation is same.

Conclusion

The chemical equation is:

  ${\text{Zn(s) + CuSO}}_{\text{4}}\left(\text{aq}\right)\to {\text{ ZnSO}}_{\text{4}}\left(\text{aq}\right)\text{+ Cu (s)}$