Cadet Eric Wiggins Date: 18 September 2014 Course Name: Chem 100 Instructor: Captain Zuniga Section: M3A Identification of a Copper Mineral Intro Minerals are elements or compounds that are created in the Earth by geological processes. The method of isolating metals in a compound mineral is normally conducted through two processes. Roasting is one which was performed in this lab involving the heating of the ore to decompose unstable ions which are bonded to the metal. Smelting is the other process, which uses heat and a chemical reducing agent to decompose a metal oxide into a pure metal. Through this process, which is a redox reaction, the transfer of electrons between the two chemical components takes place. The element that loses an …show more content…
Then more roasting occurred when the crucible was placed into a ceramic triangle for the Bunsen burner to continue its burning for an additional 90 minutes. Once the burning was officially over, the crucible was placed onto a ceramic tile to cool off. Next the charcoal and copper material were poured onto a paper towel and were separated from carefully distinguishing them one from the other. Then comparisons were down through analysis of the copper (II) oxide smelted. Then the mass of the copper metal and the percentage of Cu were obtained and compared throughout different groups and a mean and standard deviation was calculated for the …show more content…
Deductive reasoning was used by determining the identity of an unknown copper mineral by looking at different possible copper minerals in the database with observations that were taken throughout the entire lab. Through roasting, the percentage of mass could be found through the mass of copper contained in an unknown copper containing mineral sample by gravimetric analysis of the copper (II) oxide produced. Through the idea of smelting and spectroscopy the identity of the unknown copper could be found through careful calculations and analysis of the lab. A spectroscopy curve was produced of the acid and the absorbance of the unknown mineral could be obtained in order to find what that unknown copper is. Through these methods there is not preferred method when it comes to finding the percentage of an unknown substance, but which is more effective in accurately depicting what that unknown substance is. Standard deviation plays a major part in this experiment to help balance out and find the mean of the unknown substance to help constitute what it is. Through this the difference between smelting and roasting is that one produces a metal from its ore and the other drices off the carbon to obtain an
The purpose of the lab is to acquire the percent composition of zinc and copper. The procedure included obtaining a post 1983 penny and washing it with soap and water. Using a triangular file, we made an X on the penny. Then, we cleaned the top and bottom of the penny with steel wool until it was shiny. We rinsed the penny in acetone and dried it with paper towel.
Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.
The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.
(i.e., what was the evidence of reaction?) When the piece of magnesium come in contact with the flame, it ignited and emitted an intense bright white light. The light was so intense that it was painful to look at. Furthermore, after the metal was done burning the piece of magnesium changed color and consistency. Before the reaction it was a dull gray, malleable piece of metal.
AP Chemistry Semester 1 Final Review 2016 Basics of Chemistry: Name the following compounds BO3 H2S NaOH OF8 PCl6 HNO3 HgNO2 Write the formula for each compound Pentaboron triselenide Sulfuric Acid Carbon Monoxide Lithium Chloride How many moles are in 58.6 g of AgNO3 How many grams are in 2.5 moles of Cl2
We calculated the density of the metal ball to be 7.83 g/cm3 using methods IV and V and concluded it was iron. C. The density of the plate was calculated to be 2.667 g/cm3 using methods IV and V. Thus we concluded that it was aluminum. 3.
If we were given a random sample of pennies, then we could measure the mass and the volume of the pennies. From these measured values we could calculate the density. Then we could compare our calculated density to the given density value of copper and we could find the the percentage of error between copper and the measured density. Conclusion: If the percentage of error between the copper and the measured density of the pennies was large and the values were not in comparison to the density of copper, then we would know that the density of a penny is not the same as the density of pure copper.
This was achieved by using physical observations, logic, and mathematical calculations. In order to do this efficiently, several answer choices were given for the unknown metals. These choices were Bismuth, Manganese, Copper, Lead, Zinc, Tin, Cobalt, Nickel, Cadmium, and Chromium. For the unknown metal in this case (sample #21), the density was approximately 6.848g/cm3. This alone however, is not enough information to identify the metal.
Hence in the sample only copper (II) chloride will dissolve leaving the sodium chloride behind once filtered through. The copper (II) chloride can then be obtained by evaporating the methanol; which has a boiling point of 65 degrees celsius whilst copper (II) chloride has a boiling point of 993 degrees celsius, thus allowing the methanol to be easily evaporated out of the solution eliminating concerns of the copper (II) chloride evaporating alongside the methanol. Purpose To investigate different methods of separating copper (II) chloride and sodium chloride in order to obtain the original masses of both substances.
Sarah Everett CHEM 316 Monday 12-3:50 February 15, 2017 Analysis of Copper in a Penny by Atomic Absorption Spectroscopy and Ultraviolet-Visible Spectroscopy Introduction: The United States cent coin, also known as the penny, was originally composed of pure copper from 1793 to 1837 and the composition of copper in the penny has been diminishing since. For the next 145 years, the penny’s copper composition wavered between 95% and 88% until 1982 where the copper composition was reduced to 2.5% while the rest of penny was composed of 97.5% zinc.
Copper is soft and malleable and has a reddish-orange color. Copper is used as a conductor of heat and electricity, and a building material. Copper is used by automobiles, light and power lines, telephones and radio, and ammunition. These uses are important for humans, and therefore it is important to mine copper, but it is also dangerous for the environment to mine and can harm the community around these copper mines. The top five places where copper is mined are South Africa, Chile, Western USA, Kazakhstan, and Canada.
Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
The process involved blowing air into molten iron which already contains carbon in it from the ashes of stuff like coal. When the air is blown
The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.