Determination of Chemical Formulae
Determination of Chemical Formulae: The Reaction of Zinc and Iodine
By Sarah
Abstract: The main objective of this experiment was to use to the reaction between zinc and iodine to examine the validity of the Law of Conservation of Mass and the Law of Constant Composition. The Law of Constant Composition was tested by determining the mass of each of the reactants, zinc and iodine, and comparing their total to the mass of the zinc iodide product plus the excess zinc. The total mass of the reactants was determined by subtracting the mass of the empty beaker from the mass of the beaker with initial amounts of zinc and iodine in it. The mass of the reactants was 5.266g. The mass of the products was obtained by adding the mass of zinc iodide with the mass of the excess zinc. The mass of zinc iodide was 2.412g. The mass of excess zinc was 2.695g. 2.142g was then added to 2.695g to find the total mass of the products. Since the mass of the reactants is 5.266g and the mass of the products is 5.107g, it can be concluded that the Law of Conservation of Mass is a valid law.
The Law of Constant Composition was verified as well. By looking at Graph 1, it is clear to see there is about a 1:3 ratio (closer to 1:2.75) of the amount of iodine reacted to the mass of zinc reacted. Since the law states that samples of a pure compound always contain the same elements in the same mass proportion, the data from this experiment proves that, regardless of the Synthesis Number used.
Purpose: Known amounts of zinc and iodine were reacted to form zinc iodide. The obtained masses throughout the experiment were used to evaluate the validity of the Law of Mass Conservation and the Law of Constant Composition.
Law of Mass Conservation for this experiment should follow this equation:
MZn + MI2 MZn2I4
Data: Synthesis Number 4
Initial Mass Zinc
3.17g
Initial Mass Iodine
2.162g
Mass of Zn + I in beaker (no beaker mass)
5.266g
Mass of excess zinc granules (after reaction)
2.695g
By Sarah
Abstract: The main objective of this experiment was to use to the reaction between zinc and iodine to examine the validity of the Law of Conservation of Mass and the Law of Constant Composition. The Law of Constant Composition was tested by determining the mass of each of the reactants, zinc and iodine, and comparing their total to the mass of the zinc iodide product plus the excess zinc. The total mass of the reactants was determined by subtracting the mass of the empty beaker from the mass of the beaker with initial amounts of zinc and iodine in it. The mass of the reactants was 5.266g. The mass of the products was obtained by adding the mass of zinc iodide with the mass of the excess zinc. The mass of zinc iodide was 2.412g. The mass of excess zinc was 2.695g. 2.142g was then added to 2.695g to find the total mass of the products. Since the mass of the reactants is 5.266g and the mass of the products is 5.107g, it can be concluded that the Law of Conservation of Mass is a valid law.
The Law of Constant Composition was verified as well. By looking at Graph 1, it is clear to see there is about a 1:3 ratio (closer to 1:2.75) of the amount of iodine reacted to the mass of zinc reacted. Since the law states that samples of a pure compound always contain the same elements in the same mass proportion, the data from this experiment proves that, regardless of the Synthesis Number used.
Purpose: Known amounts of zinc and iodine were reacted to form zinc iodide. The obtained masses throughout the experiment were used to evaluate the validity of the Law of Mass Conservation and the Law of Constant Composition.
Law of Mass Conservation for this experiment should follow this equation:
MZn + MI2 MZn2I4
Data: Synthesis Number 4
Initial Mass Zinc
3.17g
Initial Mass Iodine
2.162g
Mass of Zn + I in beaker (no beaker mass)
5.266g
Mass of excess zinc granules (after reaction)
2.695g