Sabrina Kate S. Carranza – Chemistry Hour 6
The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.
II. Hypothesis: /3
-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then 2AgNO3 + Cu(s) 2Ag + Cu (NO3) 2
* 1 pair of gloves
* 1 pair of safety glasses
* 1 (10 cm) Copper Wire
* 1 Plastic container
* 1 bottle of 0.50 AgNO3
* 1 bottle of distilled water
* 1 Weighing tray
* 1 square of hard, rough paper (to sand wire)
* 1 electronic balance
* 1 pipet
* 1 pair of forceps
* 1 beaker
* 1 pencil
* 1 marker
* 1 roll of tape
1) Take a 10 cm length of copper wire. Sand it with the hard, rough paper. Coil it around a pencil so it assumes a spiral shape. Remove the pencil.
2) Find the mass of the copper wire with the electronic balance. Record this in the data table. 3) Label a plastic container with your name using the markers provided, and record its mass. Record this in the data table. 4) Wear safety glasses and put on gloves.
5) Pipet 50.00 mL of the 0.50M AgNO3 into the plastic container. 6) Place the coiled wire into the silver nitrate solution.
7) Write down your observations and record in the qualitative data table. DAY TWO:
8) Retrieve your container from DAY ONE and record any changes that have occurred. 9) Shake and remove the crystals from the copper wire. Allow the wire...