In this lab experience, students determine the molar relationships between silver and copper and silver nitrate and copper in the single replacement reaction between copper metal and silver nitrate. They see that atoms (and mass) are conserved in a chemical reaction—not created or destroyed but converted from one form to another—which is reflected balanced chemical equation coefficients. Students come to understand that the products of a chemical reaction can be related to the reactants by virtue of mole ratios because chemical reactions must adhere to the law of conservation of mass.
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Safety:
Remind students that nitric acid is a corrosive liquid and a strong oxidizer, and that silver nitrate is a corrosive solid, is toxic by ingestion, and will stain skin and clothes. Reiterate that acetone is a flammable liquid and to avoid contact with flames and other sources of ignition. Students should always avoid contact of all chemicals with eyes, skin, and clothing. Students should wear chemical splash goggles and chemical-resistant gloves and apron, and wash hands thoroughly with soap and water before leaving the laboratory.
Materials Included in Kit
Consumable:
Acetone,250 mL
Copper wire, 457 cm
Nitric acid, 3 M, 10 mL
Silver nitrate, 25 g
Wooden splints, package of 30
Additional Materials Required
Beakers, Borosilicate Glass, 50-mL, 10
Beakers, Borosilicate Glass, 100-mL, 10
Beakers, Borosilicate Glass, 250-mL, 10
Bottles, Washing, Polyethylene, 250-mL, 10
Flask, Erlenmeyer, Borosilicate Glass, 125 mL, 10
Flinn Scientific Electronic Balance, 210 x 0.01-g, 10
Spatulas, Disposable, Box of 300, 1
Stirring Rods, Glass, 10
1-800-452-1261
