Copper (II) Chloride is the compound with a chemical formula of CuCl2. This is a light brown solid, which slowly absorbs moisture to form a blue green dihydrate. Copper (II) Chloride is highly soluble in water and will produce a blue solution. solutioAluminum is the compound that has a chemical formula of Al. This is a silver solid that can be easily formed, machined, or cast. In this lab, we will be finding the limiting reactant between Copper(II) Chloride and Aluminum. The limiting reactant is, reactant is, the reactant in a chemical reactant that limit’s the amount of the product that can be formed. We will also need to find the molarity of Copper (II) Chloride in the solution. The molarity of a solution is, the number of moles dissolved in one liter of solution. Hypothesis:
If copper won’t completely dissolve aluminum, then copper is the limiting reagent.
1) Aluminum- 1.5g
2) Copper (II) Chloride- 100mL
4) Glass rod(stirring stick)
5) Graduated Cylinder
8) Paper Towels
Rinse out the graduated cylinder with water and then dry with a towel Mass the aluminum on a scale- 1.5g
Measure out the amount of copper (II) chloride- 100mL
Pour the 100mL of copper (II) chloride in the beaker, then add the aluminum to the solution. Stir the solution
When the solution is done bubbling, take the aluminum out the solution with tweezers. Rub the copper off the aluminum under running water and let the solution sit. Re mass the aluminum-1g
Observations/ Data collection:
The aluminum is fizzing and bubbleing in the copper (II) chloride, its now breaking apart in the solution. The solution has turned murky and grey, while the aluminum is corroding. Now, the solution is a dark purple, the container also feels slightly warm, there is now a solution at the bottom.
The true molarity of Copper(II) Chloride is 0.25
1) 2Al + 3CuCl2 =...
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