A Cycle of Copper Reaction Lab
Abstract:
After running an experiment on 0.5 g of Copper, which went through five series of reactions. So
the purpose of the entire experiment was to calculate the amount of copper after the five cycles
of chemical reactions. We did this by taking the mass of the copper dividing it by the initial mass
then multiplying by 100 to get a recovery percentage. The results of the copper reaction lab
ended up having a high percentage recovery of 100.01%, which proves there was a lab error.
Introduction:
The purpose of this experiment is to show the different types of reactions being shown during the
lab experiment. Which are oxidation reduction, redox, acid-base, precipitation forming and gas
reactions. While running through the five cycles of the copper reaction lab, we can see that there
were signs of different reactions such as; redox reaction, a double replacement reaction and
precipitation reaction, while also having decomposition and acid-based reactions occurred.
Reactant #1 A Redox Reaction (oxidation is being reduced)
4 HNO3 (aq) + Cu (s) → Cu(NO3)2 (aq) + 2 H2O (l) + 2 NO2 (g)
This reaction would be considered a redox reaction because copper was being oxidized and the
nitrogen was being reduced.
Reactant #2 A Double Replacement Reaction and Precipitation Reaction
Cu(NO3)2 (aq) + 2 NaOH (aq) → Cu(OH)2 (s) + 2 NaNO3 (aq)
The reaction from Cu(NO3)2 (aq) + 2 NaOH (aq) → Cu(OH)2 (s) + 2 NaNO3 (aq) caused a
double replacement reaction due to the Cu(NO3)2 reacting with the 2 NaOH, which leads to the
nitrate precipitate to be light blue.
Reactant #3 A Decomposition Reaction
Cu(OH)2 (s) + heat → CuO (s) + H2O (l)
The reaction from Cu(OH)2 (s) + heat → CuO (s) + H2O (l) caused a decomposition reaction
because it was breaking down copper(II) hydroxide into two molecules when being heated up at
210° C turning it into a black solid.
Reactant #4 An Acid-Base Reaction
CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)
This reaction was Acid-Based because the black copper (II) oxide reacted with the sulphuric
acid, which is blue. Then it became water and copper(II) sulfate, which caused a neutralized
reaction because metal oxides have similar properties in water.
Abstract:
After running an experiment on 0.5 g of Copper, which went through five series of reactions. So
the purpose of the entire experiment was to calculate the amount of copper after the five cycles
of chemical reactions. We did this by taking the mass of the copper dividing it by the initial mass
then multiplying by 100 to get a recovery percentage. The results of the copper reaction lab
ended up having a high percentage recovery of 100.01%, which proves there was a lab error.
Introduction:
The purpose of this experiment is to show the different types of reactions being shown during the
lab experiment. Which are oxidation reduction, redox, acid-base, precipitation forming and gas
reactions. While running through the five cycles of the copper reaction lab, we can see that there
were signs of different reactions such as; redox reaction, a double replacement reaction and
precipitation reaction, while also having decomposition and acid-based reactions occurred.
Reactant #1 A Redox Reaction (oxidation is being reduced)
4 HNO3 (aq) + Cu (s) → Cu(NO3)2 (aq) + 2 H2O (l) + 2 NO2 (g)
This reaction would be considered a redox reaction because copper was being oxidized and the
nitrogen was being reduced.
Reactant #2 A Double Replacement Reaction and Precipitation Reaction
Cu(NO3)2 (aq) + 2 NaOH (aq) → Cu(OH)2 (s) + 2 NaNO3 (aq)
The reaction from Cu(NO3)2 (aq) + 2 NaOH (aq) → Cu(OH)2 (s) + 2 NaNO3 (aq) caused a
double replacement reaction due to the Cu(NO3)2 reacting with the 2 NaOH, which leads to the
nitrate precipitate to be light blue.
Reactant #3 A Decomposition Reaction
Cu(OH)2 (s) + heat → CuO (s) + H2O (l)
The reaction from Cu(OH)2 (s) + heat → CuO (s) + H2O (l) caused a decomposition reaction
because it was breaking down copper(II) hydroxide into two molecules when being heated up at
210° C turning it into a black solid.
Reactant #4 An Acid-Base Reaction
CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)
This reaction was Acid-Based because the black copper (II) oxide reacted with the sulphuric
acid, which is blue. Then it became water and copper(II) sulfate, which caused a neutralized
reaction because metal oxides have similar properties in water.
