Electrolysis of Water Lab

•  What is the balanced chemical equation of this experiment?
•  Is there qualitative evidence to support the balanced reaction?
•  Could you collect quantitative data to 'prove' the balanced equation 
•  Can you draw the particle diagram?

      Through a simple and fast procedure, we were able to view the separation of both 

hydrogen and oxygen within a baking soda mixture. In order to examine this separation,we filled two test tubes with the baking soda and water solution. We had a cup with two thumbtacks in which we placed each test tube over, and quickly there after filled the cup with the solution. We then placed the cup on a battery with each thumbtack on the positive and negative side of the battery. The setup and and beginning reaction looked like this:

 In this electrolysis of water lab, the production of hydrogen and oxygen can be represented through  the decomposition reaction equation; 2H2O----> 2H2 + O2. This balanced chemical equation can be supported by the quantitative evidence. Quantitative data in this lab supports the Law of Conservation of mass. In order to record this data one would mass the solution before and after the reaction. This law is proved by the equation produced, and by the particle diagram below.

Qualitative data was also observed in order to prove the balanced equation. This data includes; the examination of bubble production rate within each tube. We observed the rate of bubble production in one tube, which was significantly faster than the other. Thus further proving the separation of the hydrogen and oxygen gases. 

 An indicator was  also added to the substance. This gave us, the observers, another view as to     what was happening with in thee substance. With the addition of the indicator, the colors in the tubes began changing. One tube had more of a yellow tint, while the other had more of a blue color thus indicating a divergence of an acid and a base in the substance.

                                                  

Composition of a Hydrate Lab

        We performed this lab in order to determine whether a hydrate was a pure substance or a mixture. In order to determine the composition of the hydrate, we used a specific and significant technique. This technique was the use of heat to determine whether or not the substance's mass remained the same or varied. If the substance had resulted in a significant loss of mass, with an erratic percent composition of water,  one could conclude that the hydrate was a mixture. This conclusion would be valid because, a mixture is made up of more than one pure substance. Each pure substance's components have different properties. Opposed is a pure substance, which contains only one type molecule. This means that the substance maintains a constant composition. If the hydrate was a pure substance, when it was heated it should have resulted in no loss of mass or a consistent loss of water composition percentage. We used this percent composition in mathematically proving that the hydrate was a pure substance. In order to prove our conclusion valid, the percentage we obtained must have been in range of 48.8%. Our percentage amounted to 47.7%  meaning a minuscule percent error and a valid result.