# Let's Get Started with Copper

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• Published : April 16, 2013

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Report Sheet Experiment 1

0 Balance the equations for the three reactions studied. Note, in all reactions the numbers of atoms of each type and the total charge must be equal on each side of the equation.

Equations
1)Cu + 4H+(aq) + 2NO3-(aq)  Cu2+(aq) + 2NO2 + 2H2O 2) Cu2+(aq) + 2-OH(aq)  Cu(OH)2
3)Cu(OH)2 + heat  CuO + H2O (Balanced) 4)CuO + H2SO4  Cu2+(aq) + SO42-(aq) + H2O (Balanced) 5)Cu2+(aq) + Zn  + Cu + Zn2+(aq) (Balanced) Stage 1 Dissolution of Copper

Mass of vial & copper= 3.598g

Mass of vial = 2.504g

Mass of copper = 1.094g

Calculate the moles of copper, this is the mass of copper (in g) divided by the atomic mass of copper, (63.5 g/mol) Moles of copper = mass (g) ÷ (63.5 g/mol)
= 0.017g/mol
Copper description

Solid ribbons, of a reddish-brown metallic appearance.

HNO3 description

Clear transparent aqueous solution with a similar viscosity to water

Notes and observations on the reaction

An exothermic chemical reaction occurred as the 8 M nitric acid solution was dispensed into the copper-containing beaker. Instantly we observed a brown gas dispersing from the solution. A transparent blue homogenous liquid was produced as the copper dissolved into the HNO3 solution. Condensation began forming on the watch glass, concurrently with the increasing temperature of the beaker, which became hot.

Where is the copper?

The copper ribbons were oxidized by the nitric acid, where the newly formed copper ions had bonded with water molecules producing a transparent blue solution. Stage 2 Precipitation of Copper Hydroxide

NaOH solution description

Clear transparent aqueous liquid with a similar viscosity to water

Notes and observations on the reaction

The mixture became gelatinous and the beaker began warming as we added the Sodium...