Honors Chemistry Period 4
13 May 2012
Redox Reactions Lab Report
We wished to investigate the oxidation number of a metal that would form aqueous ions when reacted with an aqueous nitrate salt. For this purpose, we chose to investigate the reaction of solid copper metal, in the form of a wire, with aqueous silver nitrate. Before we began the lab, we hypothesized that when silver nitrate, AgNO3, reacts with copper, Cu, the oxidation number of silver (Ag) ions that form will be +1. The unbalanced chemical equation that we used to represent this reaction is Cu + AgNO3 → Ag + Cu(NO3)2. In order to find the approximate masses of reactants needed to produce about 2 grams of silver, we found the molar masses of each of the reactants and products: Molar Masses
| |AgNO3 |Cu |Ag |Cu(NO3)2 | |Molar Mass (in g) |169.88 |63.55 |107.87 |187.57 |
Next, we used stoichiometry to calculate the necessary mass of reactants to produce about 2 grams of silver: [pic]
The limiting reactant is the reactant in a chemical reaction that limits the amount of the product that can be formed. The reaction will not continue after all of the limiting reactant is consumed. The limiting reactant in our reaction is Cu because we want the entire amount of the element to bond with the AgNO3. The excess reactant is the reactant in a chemical reaction that is left over after a reaction. The excess reactant remains because there is nothing left for it to react with. The excess reactant in our reaction is AgNO3 because we want to isolate it, so that we can determine the oxidation number. In order to carry out this experiment, we used the following masses of reactants and...