Mole Ratio Lab Essay Example
Mole Ratios Lab
October 10, 2013
Mrs. Oliver
Noah Kent
AP Chemistry
Block 3/4
Laboratory #4: Mole Ratios
I. Hypothesis: If copper wire is placed in an aqueous solution with silver nitrate, then silver crystals will grow on the wire surface and the solution will gradually take on the color of Copper (II) ions. The relative quantities of reactants and products in this chemical reaction can be determined by measuring the mass of copper wire consumed in the reaction and the mass of silver crystals that result. These measurements can then be used to determine the number of moles of reactants and products in the reaction and calculate their mole ratio.
II. Equipment:
Balance
Labeling
50 ml beaker
100 ml beaker
125 ml Erlenmeyer Flask
Spatula
Stirring rod
Wash bottle and distilled or deionized water
Wooden splint
III. Reagents:
Acetone, CH3COCH3
Copper Wire, Cu
Nitric Acid, HNO3
Silver NItrate, AgNO3
IV. Procedure:
1. Obtain a clean and dry 50-mL beaker. Zero the balance with the beaker on the balance pan and then carefully add 1.4–1.6 g of silver nitrate to the beaker. Caution: Use a spatula to transfer the solid—do not touch the silver nitrate. Carefully clean up any silver nitrate spills in the balance area or on the bench top. 2. Measure and record the exact mass of silver nitrate in the data table. 3. Fill the beaker to the 30-mL mark with distilled water and stir the solution with a stirring rod until all of the solid has dissolved. Rinse the stirring rod with distilled water. 4. Cut a 25-cm piece of copper wire and loosely coil it into the shape shown in Figure 1. 5. Find the initial mass of the copper wire to the nearest 0.01 g and record it in the data table. 6. Use a wooden splint to suspend the copper wire in the silver nitrate solution, as shown in Figure 1. The copper wire should not be touching the bottom or sides of the beaker. 7. Carefully add 3 drops of 3 M nitric acid to the beaker. Do NOT stir the solution. 8.
October 10, 2013
Mrs. Oliver
Noah Kent
AP Chemistry
Block 3/4
Laboratory #4: Mole Ratios
I. Hypothesis: If copper wire is placed in an aqueous solution with silver nitrate, then silver crystals will grow on the wire surface and the solution will gradually take on the color of Copper (II) ions. The relative quantities of reactants and products in this chemical reaction can be determined by measuring the mass of copper wire consumed in the reaction and the mass of silver crystals that result. These measurements can then be used to determine the number of moles of reactants and products in the reaction and calculate their mole ratio.
II. Equipment:
Balance
Labeling
50 ml beaker
100 ml beaker
125 ml Erlenmeyer Flask
Spatula
Stirring rod
Wash bottle and distilled or deionized water
Wooden splint
III. Reagents:
Acetone, CH3COCH3
Copper Wire, Cu
Nitric Acid, HNO3
Silver NItrate, AgNO3
IV. Procedure:
1. Obtain a clean and dry 50-mL beaker. Zero the balance with the beaker on the balance pan and then carefully add 1.4–1.6 g of silver nitrate to the beaker. Caution: Use a spatula to transfer the solid—do not touch the silver nitrate. Carefully clean up any silver nitrate spills in the balance area or on the bench top. 2. Measure and record the exact mass of silver nitrate in the data table. 3. Fill the beaker to the 30-mL mark with distilled water and stir the solution with a stirring rod until all of the solid has dissolved. Rinse the stirring rod with distilled water. 4. Cut a 25-cm piece of copper wire and loosely coil it into the shape shown in Figure 1. 5. Find the initial mass of the copper wire to the nearest 0.01 g and record it in the data table. 6. Use a wooden splint to suspend the copper wire in the silver nitrate solution, as shown in Figure 1. The copper wire should not be touching the bottom or sides of the beaker. 7. Carefully add 3 drops of 3 M nitric acid to the beaker. Do NOT stir the solution. 8.