Consider reacting copper(II) sulfate with iron. Two possible...

Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. $\operatorname{copper}($ II $)$ sulfate $(a q)+\operatorname{iron}(s) \longrightarrow$ $\operatorname{copper}(s)+$ iron(II) sulfate $(a q)$ $\operatorname{copper}($ II $)$ sulfate $(a q)+\operatorname{iron}(s) \longrightarrow$ $\operatorname{copper}(s)+$ iron(III) sulfate $(a q)$ You place $87.7 \mathrm{~mL}$ of a $0.500 \mathrm{M}$ solution of copper(II) sulfate in a beaker. You then add $2.00 \mathrm{~g}$ of iron filings to the copper(II) sulfate solution. After one of the above reactions occurs, you isolate $2.27 \mathrm{~g}$ of copper. Which equation above describes the reaction that occurred? Support your answer.

Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations.
$\operatorname{copper}($ II $)$ sulfate $(a q)+\operatorname{iron}(s) \longrightarrow$
$\operatorname{copper}(s)+$ iron(II) sulfate $(a q)$
$\operatorname{copper}($ II $)$ sulfate $(a q)+\operatorname{iron}(s) \longrightarrow$
$\operatorname{copper}(s)+$ iron(III) sulfate $(a q)$
You place $87.7 \mathrm{~mL}$ of a $0.500 \mathrm{M}$ solution of copper(II) sulfate in a beaker. You then add $2.00 \mathrm{~g}$ of iron filings to the copper(II) sulfate solution. After one of the above reactions occurs, you isolate $2.27 \mathrm{~g}$ of copper. Which equation above describes the reaction that occurred? Support your answer.

Key Concepts

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first in a chemical reaction, thereby limiting the amount of products formed. Identifying the limiting reagent using stoichiometric calculations is essential for accurately predicting the yield of a reaction.

Oxidation States

Oxidation states describe the degree of oxidation of an atom in a chemical compound. They help identify the electron transfer occurring during redox reactions. Understanding oxidation states is integral when evaluating whether a metal will reduce ions in solution and determining the products formed in a reaction.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. It enables the determination of which reactant is present in insufficient quantity (the limiting reagent) and helps predict the amounts of products that will be formed under given conditions.

Redox Reactions

Redox reactions, short for reduction-oxidation reactions, involve the transfer of electrons between chemical species. One reactant is oxidized (loses electrons) while another is reduced (gains electrons). This concept is crucial for understanding reactions in which metals change oxidation states, such as when a metal displaces another from its compound.

Displacement Reactions

Displacement reactions are a type of redox reaction in which a more reactive element displaces a less reactive element from its compound. In these reactions, the metal that is more reactive will oxidize (lose electrons), causing the less reactive metal ion to be reduced (gain electrons), leading to the formation of a new compound.

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