The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result. This is important because the correct reaction would only appear if the right elements are mixed together, the unknown substances on the iron nails can cause a different reaction to happen that is not expected. …show more content…
After a while, a brownish color substance started to form on the three iron nails. We predicted that the brown substance on the nails is copper because the reaction of copper(II) chloride with iron is a single displacement reaction, so copper would be produced. 0.48 grams of iron was used in the reaction because 2.73 grams subtracted by 2.25 grams is 0.48 grams. The 0.48 grams of iron had to be used in the reaction with copper(II) chloride in order to produce copper, according to the reaction equation: CuCl2+FeFeCl2+Cu. 0.52 grams of copper was produced after pouring out the copper(II) chloride solution and the three iron
An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
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
Group 1: All the elements that were tested from group 1 had a pH level of 12. This meant that all the tested elements produce an alkaline solution. Group one elements readily lose their valence electron as they wish to form a full valence shell this gives them all a low electron affinity. The group one elements have different electronegativity going down the group. Electronegativity of the elements decreases with the increasing the atomic radii.
The can be seen when iron is coated in zinc. This process is efficient by comes with the prices of losing the zinc due to the fact that the zinc will oxidizes instead of the iron
Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear.
Properties of Substances Express Lab 1)The purpose of this lab was to compare the physical properties of different types of solids and how the properties of solids are determined by their intermolecular forces and their intramolecular bonds. Then we were to classify each type of solid as either ionic, metallic, non-polar molecular, polar molecular, or network. Paraffin wax classified as a non-polar molecular, Silicon dioxide was classifies as a network, Sodium chloride was classified as ionic, Sucrose was classified as polar molecular and Tin was classified as metallic. (2)The intermolecular forces that are present in Paraffin wax are dispersion forces, because it is non-polar and carries a negative charge. Followed by Sucrose that has
Therefore, as HCl was added, a shift occurred. Additionally, the equilibrium for the reaction was determined to be 92. After iron (III) thiocyanate was formed and separated into four separate test tubes, one control and three with additional components, shifts had occurred in each of the three experimental test tubes. When 0.02 M Fe(NO3)3 was added, the solution changed from a reddish-orange color to a deep, dark red indicating a shift to the right or to the products, while 0.02 M NaSCN was added to another test tube, it simply became about one shade lighter but should have
Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, research of definitions of each relating led to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound forms when two or more nonmetal atoms share valence electrons; covalent compounds are also
Other then being an important aspect in humanity Fe, one of the three magnetic elements, the other two being cobalt and nickel, is also the fourth of Earth’s most abundant mineral, by mass (Royal Society of Chemistry, Iron). The source of this iron comes naturally from ores deep in the earth’s crust in sedimentary crusts, since iron oxidizes remarkably fast on the Earth’s surface. For commercial use, pure Iron can transform into steel or an alloy by adding other impurities and elements, making it an
A standard curve plotted during the analysis was used to extrapolate the concentration of iron in the urine samples (Sandell and Kolthoff, 1937). Reagents and Chemicals- Potassium iodate, Ammonium persulphate, Ceric ammonium sulfate, Arsenic trioxide, Sodium chloride, conc. Sulphuric acid and distilled water. Quantitative method based on
2.5.4. Metal chelating activity Briefly, 2 mM FeCl2 was added to different concentrations of test sample and reaction was initiated by the addition of 5 mM ferrozine. The mixture was vigorously shaken and left to stand at room temperature for 10 min. Absorbance was measured at 562 nm after 10 min.8 % Inhibition = [(AB - AA)/AB] x 100, where AB, absorption of blank sample, AA, absorption of test sample.
Then it was treated with alcohol and the resulting iron free residue was a reddish purple color
Typically, FeCl2.4H2O (4.3 g) and FeCl3.6H2O (11.6 g) were mixed with 350 mL of deionized water under N2 atmosphere. The resulting solution was heated to 80 °C while stirring, vigorously. Then, 20 mL of 25% NH4OH was quickly added into the solution. The resulting suspension was vigorously stirred for 5 min and then, the black precipitates were collected with the help of a magnet and washed repeatedly with deionized water and ethanol, then dried at vacuum