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Cu reacts to form CuO

2Cu(s) + O(g) --> 2CuO(s)

Stoichiometry

Reaction #1

Mass of copper before heating: 1.04g Cu

1 mol Cu

X

63.55g Cu

= 0.0164 moles Cu

Mass of Oxygen removed from the air: 0.02 g Oxygen

Theoretical Moles of copper oxide formed: 0.0133 mol

Percent of Copper that was oxidized: 7.69%

Theoretical mass of unoxidized and oxidized copper:

Moles of unoxidized (unreacted) copper (based on moles of copper (II) oxide that were formed): 0.0152 mol Cu

Mass of unoxidized (unreacted) copper: 0.966 g Cu

Mass of oxidized copper: 0.0794 g Cu

Total mass of copper recovered during parts II and III:

0.83 g + 0.32 g = 1.15 g

% yield of total amount of copper recovered:

% yield =

"Dillon O'Leary has a work ethic unrivaled by anyone I have ever met and truly is a god among men. I would give my first-born child just to be him for a single day."

-Bergen Thomson, Disciple

Mass of filter paper #2 and recovered, unoxidized copper

Mass of zinc added to the HCl solution

Mass of recovered, unoxidized copper

Reaction Data Table

Mass of Materials in Reaction

Mass of filter paper #2

0.74 g

1.57 g

0.83 g

1.58 g

= 0.024 mol Zn

x 100 = 83%

Moles of zinc added to the HCl solution:

% yield of unoxidixed copper recovered

1 mol

65.41 g Zn

0.83 g

1 g

X

1.58 g Zn

1

% yield =

CuO reacts with HCl to form Cu^2+ ions, Cl^- ions and water

Chemical Equation

CuO + 2HCl --> Cu^2+ + 2Cl^- + 2H_2O

-Zinc becomes black

-Zinc disks break apart

unoxidized copper

-Charcoal like

-Black

Observations

Zinc

Copper Lab Final:

Reaction #3

Reaction #1

  • Reducing the dissolved Cu + ions in the solution back to Cu atoms.

+2

Separating Copper from Copper Oxide

Chemical equation:

By:

Elizabeth Kulus, Bergen Thomson, and Dillon O'Leary

  • Copper is oxidized through heating

Reaction #2

2

Data Table 1:

Mass of crucible: 11.57g

Observations:

Mass of crucible and copper dust (before heating: 12.61g

It turned rainbow at first then grey

Mass of crucible and material (after heating): 12.63g

Production of hydrogen gas:

+ H

2

Zn + 2HCl ---> ZnCl

Reduction of Cu from CuCl :

2

CuCl

+ Zn ---> Cu +ZnCl

2

Purpose of the lab:

The purpose of the Copper Lab is to demonstrate the Law of Conservation of Matter

Mass of filter paper #3:

0.74 g

  • Copper floating on top of acid
  • Some copper left on bottom of beaker
  • Some leftover zinc on bottom of beaker

Mass of filter paper #3 and recovered, oxidized copper:

1.06 g

Mass of recovered, oxidized copper:

0.32 g

2

Mass of magnesium added to the HCl solution:

0.29 g

  • Bubbles coming up
  • Liquid becoming cloudy
  • Mg turning black

Conclusion:

This lab intended to show the Law of Conservation of Matter. The Copper atoms never disappeared, they just rearranged themselves. Although some of the copper was lost due to human error, the lab still did a decent job of showing the Law of Conservation of Matter.

Mass of oxidized copper recovered during part III:

0.32 g

% yield =

Experimental result (3.A.1)

x 100

Theoretical result (1.C.3)

0.32 g

% yield of oxidized copper =

x 100 = 400%

0.0794 g

1.15 g

x 100 = 111%

1.04 g

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