Limiting Reactants Lab Report

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The purpose of the experiment was to observe limiting reactants by using a fixed amount of one reagent along with a varying the amount of the second reagent used in a chemical reaction. Through these results, the concept of limiting reactants can be determined. Using a graph to demonstrate the relation between the volumes of hydrogen gas produced versus the moles of the reagents will help figure out the stoichiometric balance required. The success of the experiment will be determined by the comparing the experimental values with the fixed values.

Introduction
Stoichiometry involves converting chemical formulas and equations that represent individual atoms, molecules, and formula units to the laboratory scale that uses milligrams, grams, and kilograms, of these substances (1). A limiting reactant is the reactant that has been completely consumed in a chemical reaction. It is
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A graph of the volume of hydrogen gas produced versus moles of a reagent that is varied will be able to tell you the point in which the stoichiometric balance is achieved and what the limiting reactant is. In this experiment group A used a constant mass of magnesium metal (0.100 g) and varying volumes of 2.00 M hydrochloric acid added from 2.00 mL to 7.00 mL in progressions of 1.00 mL which in total came out to be six distinctive chemical reactions. Group B used the consistent volume of 2.00 M hydrochloric acid (5.00 mL) and changed the mass of the magnesium metal used from 0.070 g to 0.170 g in growths of 0.020 g which resulted in a total of six different chemical reactions as well. The percent yield for magnesium, according to the data, was 107.3% and the percent yield for hydrochloric acid, according to the data, was 96.0%. Overall, the experiment was fairly successful as observed by the percent yields of both

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