Shown here is the balanced molecular equation for the reaction that would occur between CuCl₂(aq) and Pb(s). Which of the following, if any, shows the correctly balanced net ionic equation Molecular equation: CuCl₂(aq) + Pb(s) $\rarr$ Cu(s) + PbCl₂(s) A) Net ionic equation: Cu²⁺(aq) + 2Cl^-(aq) + Pb(s) $\rarr$ Cu(s) + Pb²⁺ (aq) + 2 Cl^-(aq) B) Net ionic equation: 2Cu²⁺(aq) + 2Cl^-(aq) + Pb(s) $\rarr$ 2Cu(s) + PbCl₂(s) C)Net ionic equation: Cu²⁺(aq) + Pb(s) $\rarr$ Cu(s) + Pb²⁺(aq) D) Net ionic equation: Cu²⁺(aq) + 2Cl^-(aq) + Pb(s) $\rarr$ Cu(s) + PbCl₂(s) E) None of the above

Question

Quizplus · Accepted Answer

The net ionic equation should only include the reactants and products that are directly involved in the chemical reaction, meaning any spectator ions should be eliminated. In this case, the spectator ions are the Cl- and Pb2+ ions, which do not participate in the reaction. Thus, the net ionic equation should be:
Cu2+(aq) + Pb(s) → Cu(s) + Pb2+(aq)
However, since CuCl2 is a soluble salt, it will dissociate in water and form Cu2+ and Cl- ions. Thus, the complete net ionic equation is:
Cu2+(aq) + 2Cl-(aq) + Pb(s) → Cu(s) + PbCl2(s)
Choice D is the correct net ionic equation, which eliminates the spectator ions and correctly includes the products Cu and PbCl2.

Shown Here Is the Balanced Molecular Equation for the Reaction →\rarr→

Shown Here Is the Balanced Molecular Equation for the Reaction $\rarr$