Observations of Reactions of Copper
Dominick Prince
Partner: Ryan Potts
Reactions of Copper
Due: Monday January 14, 2013 Beginning of Class
Block: 5
Purpose / Safety:
Purpose: 1. Observe some chemical reaction of copper and its compounds. 2. Write word and formula equations to represent these reactions.
Safety: 1. Wear goggles and a lab apron or coat. 2. Tie back long hair and secure loose clothing before working with an open flame. 3. Corrosive substance; avoid contact with skin, eyes, and clothing. Do not inhale vapor. 4. Poisonous or noxious vapors. Use the fume hood when directed to do so. Do not inhale vapor.
Equipment and Materials:
* 250 mL beaker * 1.5 g Copper * Scooper * Scale * Goggles * Nitric Acid * Fume Hood * 400 mL beaker * Tap water * Sodium Hydroxide * 25 mL graduated cylinder * Stirring Rod * Distilled Water * Heater * Tong * Sulfuric Acid * 100 mL graduated cylinder * Zinc * Hydrochloric Acid
Observations:
1. Addition of nitric acid to copper: * Solution turns blue * Emits orange gas * Copper Nitrate is formed 2. Addition of sodium hydroxide to copper(II) nitrate: * Blue crystals liquefy * Cloudy appearance 3. Heating copper(II) hydroxide: * Solution turns black upon stirring * Water on top of copper 4. Addition of sulfuric acid to copper(II) oxide: * Solution turns clear blue when stirred 5. Addition of zinc to copper(II) sulfate: * Copper is formed
Data and Calculations:
Initial Mass of Beaker: 107.3g
Initial Mass of Copper: 1.5g
Final Mass of Beaker and Copper: 108.4g
Mass of Copper Recovered: 1.1g
% Y = Final mass of Cu/Initial Mass of Cu x 100
1.1g Copper/1.5g Copper x 100 = 7.33%
Questions / Analysis
1. Classify each of the reactions from the equation section as: synthesis, decomposition, single replacement, or double replacement. Exclude equation 1 only!
Equation 2:
Partner: Ryan Potts
Reactions of Copper
Due: Monday January 14, 2013 Beginning of Class
Block: 5
Purpose / Safety:
Purpose: 1. Observe some chemical reaction of copper and its compounds. 2. Write word and formula equations to represent these reactions.
Safety: 1. Wear goggles and a lab apron or coat. 2. Tie back long hair and secure loose clothing before working with an open flame. 3. Corrosive substance; avoid contact with skin, eyes, and clothing. Do not inhale vapor. 4. Poisonous or noxious vapors. Use the fume hood when directed to do so. Do not inhale vapor.
Equipment and Materials:
* 250 mL beaker * 1.5 g Copper * Scooper * Scale * Goggles * Nitric Acid * Fume Hood * 400 mL beaker * Tap water * Sodium Hydroxide * 25 mL graduated cylinder * Stirring Rod * Distilled Water * Heater * Tong * Sulfuric Acid * 100 mL graduated cylinder * Zinc * Hydrochloric Acid
Observations:
1. Addition of nitric acid to copper: * Solution turns blue * Emits orange gas * Copper Nitrate is formed 2. Addition of sodium hydroxide to copper(II) nitrate: * Blue crystals liquefy * Cloudy appearance 3. Heating copper(II) hydroxide: * Solution turns black upon stirring * Water on top of copper 4. Addition of sulfuric acid to copper(II) oxide: * Solution turns clear blue when stirred 5. Addition of zinc to copper(II) sulfate: * Copper is formed
Data and Calculations:
Initial Mass of Beaker: 107.3g
Initial Mass of Copper: 1.5g
Final Mass of Beaker and Copper: 108.4g
Mass of Copper Recovered: 1.1g
% Y = Final mass of Cu/Initial Mass of Cu x 100
1.1g Copper/1.5g Copper x 100 = 7.33%
Questions / Analysis
1. Classify each of the reactions from the equation section as: synthesis, decomposition, single replacement, or double replacement. Exclude equation 1 only!
Equation 2: