Copper/Silver Lab Essay, Research Paper
Director of Operations
Adkinson Chemical Corporation
Dear Mrs. Adkinson:
A sample of copper has been produced as requested. We are pleased to report that the
most copper has been produced through the most efficient method. But we regrettably to
report that an accident had occurred during the process (which you will not be billed for).
This accident led to a series of investigations to weed out incompetent workers. The
remaining technicians were the best and most capable of producing the highest purity of
copper at the minimum cost. Captain Copper Chemical Corporation supplies
application-specific process chemicals for most of the science industry. The combination
of high technology products and in-depth support, from the technical service team, allows
the customer to maximize productivity and minimize cost. Captain Copper Chemical
Corporation is a technology-driven, not marketing-driven company. We pride ourselves
on our capacity to solve client?s chemical process issues, and will develop custom
products, when required. Captain Copper Corporation is currently both the leading North
American distributor of chemicals and a world leader in manufacturing a variety of
chemical specialties. In locations throughout the world, you?ll find Captain Copper
Chemical Corporation operations upholding standards that keep safety, health and
environmental considerations a top priority. OSHA has deemed the CCCC of using safe
techniques and proper disposal of wastes. CCCC strives to be the most dependable
supplier of high-quality goods and services for our important constituents. CCCC is
dedicated into achieving mutually profitable relationships with our customers and suppliers
by providing quality products and services, on time and consistently, and by remaining
constantly aware of changing customer needs. Captain Chemical Corporation invites you
to share your chemical process problems, and issues, so that we may offer and
demonstrate our capacity to assist you in becoming the leader in your industry.
1.Determine limiting reactant
2. Prepare a data table with the following: mass of- beaker A, beaker B, beaker A +
CuSO4 . 5H2O, beaker B + Fe, CuSO4 . 5H2O , Fe, filter paper, beaker B + filter
paper + Cu, Cu, and observations
3.Clean and dry two 250 mL beakers. Label one A and the other B. Mass each
beaker. Record results in data table
4.Purchase 10g of CuSO4 . 5H2O and 2.22g of Fe (less than needed to make sure all
Fe reacts). Place CuSO4 . 5H2O in beaker A and Fe in beaker B. Mass each
beaker. Record results in data table
5.Dissolve CuSO4 . 5H2O (Dr. Merck informed us that CuSO4 . 5H2O was soluble)
6.Heat beaker A (w/ CuSO4 . 5H2O (aq)). Heat until solution is hot but not boiling.
7.Remove beaker A from hot plate using beaker tongs and pour CuSO4 . 5H2O (aq)
into beaker A and let CuSO4 . 5H2O react with Fe
8.Let the chemicals react. Done for the day.
9.Make observations of solution and precipitate.
10.Setup to filter solution. Set ring stand with funnel. Mass filter paper. Record
results in data table. Fold filter paper and set it up in funnel. Wet filter paper to
remove all space between filter paper and funnel.
11.Decant solution and filter into beaker A using stirring rod. Rinse precipitate (Cu)
with distilled water. Filter solution again. Do this about three times.
12.Dispose of filtrate (FeSO4). Place filter paper into beaker B with precipitate. Dry
beaker B. Done for the day.
13.Make observations of copper. Scrape any remaining copper on filter paper into
beaker. Mass the copper and record results into data table (Dr. Merck
recommends removing all iron impurities with a magnet)
The following calculations were made prior to the lab for limiting reactant determination
to make efficient use of all materials.
molar mass of CuSO4 . 5H2O = 63.5g Cu + 32.1g S + 144.0g O + 10.1g H = 249.7g
molar mass of Fe = 55.8g
molar mass of FeSO4 = 55.8g Fe + 32.1g S + 64.0g O = 151.9g FeSO4
molar mass of Cu = 63.5g Cu
mols of 10g CuSO4 . 5H2O
= 0.040048058 mols of CuSO4 . 5H2O
mols of 10g Fe
mols of Fe needed if 10g CuSO4 . 5H2O
mols of CuSO4 . 5H2O if 10g Fe
mass of Fe needed if 10g of CuSO4 . 5H2O is used:
= 2.234681618g Fe = 2.23g Fe
mass of CuSO4 . 5H2O needed if 10g of Fe is used:
= 44.74910394g CuSO4 = 44.7g
* mass of CuSO4 . 5H2O
CuSO4 . 5H2O is the limiting reactant.
mass of Cu expected to be produced from 2.22g of Fe:
= 2.526344086g Cu = 2.53g Cu
The following calculation was made after the lab for percent yield determination:
2.50g Cu (actual mass)
2.53 g Cu (theoretical mass) x 100 = 98.8142292% = 99%
99% of the theoretical mass of copper to be produced was retrieved.
CuSO4 . 5H2O.5 grams = $.5010g = $10.00
Fe.5 grams = $1.002.22g x 2= $8.88