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Understanding the reactivity series is crucial in predicting which metals will react in a chemical reaction. The reactivity series is a list of metals arranged in order of their reactivity from highest to lowest. More reactive metals tend to lose electrons and form positive ions more readily than less reactive metals. In our exercise, zinc is more reactive than copper, which means it can displace copper ions from copper(II) nitrate. Silver, being less reactive than both zinc and copper, will not react in this scenario. Essentially, knowing this series allows us to identify that zinc will engage in a chemical reaction, displacing copper ions and forming copper metal in the process. When assessing chemical reactions involving metals, always refer back to the reactivity series to determine potential reactions.

Net ionic equations simplify chemical reactions by showing only the particles involved in the actual chemical change. This type of equation eliminates spectator ions, or ions that remain unchanged during the reaction, from the complete ionic equation. For the zinc and copper(II) nitrate reaction:

• Begin by writing the balanced molecular equation.
• Identify spectator ions, eliminating them to focus on the ions and compounds that undergo change.
• The resulting net ionic equation for zinc reacting with copper(II) nitrate is: \[ \text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s) \]

This equation effectively highlights that zinc is oxidized to Zn虏鈦�, while Cu虏鈦� is reduced to copper metal. Writing net ionic equations helps to clearly visualize the chemical process and identify changes to each species involved.

In a chemical reaction, the limiting reagent is the reactant that is entirely consumed first, limiting the amount of product formed. To find the limiting reagent, compare the mole ratio of the reactants based on the balanced chemical equation. In our example:

• Calculate the moles of each reactant available: zinc is 0.0459 mol, and Cu虏鈦� is 0.1 mol.
• Determine the stoichiometry of the reaction: the reaction requires a 1:1 ratio of zinc to copper ions.
• Since zinc provides fewer moles than Cu虏鈦�, it is the limiting reagent.

Identifying the limiting reagent is important as it dictates the maximum yield of product. In this case, the zinc limits the formation of copper metal, which impacts calculations for the remaining concentration of copper ions after the reaction.

Molarity is a measure of the concentration of a solute in a solution. It is described as moles of solute per liter of solution, denoted as M. In the exercise, it's important for calculating how much of the reactant is used, and how much of the product and remaining reactant are in the solution. In our example:

• After the reaction, you have unreacted Cu虏鈦� left in the solution.
• To find the molarity of Cu虏鈦� remaining, subtract moles of zinc reacted from initial moles of Cu虏鈦�, which is 0.1 mol - 0.0459 mol, leaving 0.0541 mol of Cu虏鈦�.
• Divide by the solution volume, 0.5 L, to find the new molarity of Cu虏鈦�:
\[ \text{Molarity of Cu}^{2+} = \frac{0.0541 \, \text{mol}}{0.500 \, \text{L}} = 0.1082 \, \text{M} \]

This calculation allows you to understand the remaining concentration of ions in a solution after the reaction, which is crucial for both practical and theoretical chemistry applications.