This reaction is a single Metal replacement reaction. The zinc and copper switch places in our reaction. This is what causes the liquid to become clear and the copper to form at the bottom of the flask. [S2]
This reaction is an exothermic reaction. An exothermic reaction is where the reaction releases more heat energy than it gains, this results in the temperature of the product being lower than the reactants. [S4]
Then we balanced the chemical equation. when you balance an equation you can only change the coefficients and the goal is to make the ratio of the elements on both sides of the yield the same.
Inserting red litmus paper into copper chloride.
Removing litmus paper from copper chloride. Result = red litmus paper remains the same color.
Inserting blue litmus paper into copper chloride.
Removing blue litmus paper from copper chloride. Result = blue litmus paper turned red.
Next we tested our reactants to find out if they were acids or bases. To do this we dipped two different types of litmus paper into the solution.
Blue paper to red = acid. Red paper to Blue = base. [S1]
Our experiment concluded that our solution is an acid.
[Source One] http://www.rsc.org/learn-chemistry/resource/res00000723/the-reaction-between-zinc-and-copper-ii-oxide?cmpid=CMP00006707
[Source 2] http://chemdemos.uoregon.edu/demos/Reaction-of-Zinc-and-CopperII-Ion
[Source 3] http://web.lemoyne.edu/giunta/chm151L/copper.html
[Source 4] http://antoine.frostburg.edu/chem/senese/101/thermo/faq/why-are-metal-displacements-exothermic.shtml
[Source 5] http://www.dictionary.com/browse/chemical-reaction