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%. 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 …show more content…
Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s) + H2O (g) Reaction 4: when a sulphuric acid is added to the solution that contains copper (II) oxide, a double displacement reaction will occur. the copper (II) oxide will react with the sulphuric acid producing copper (II) sulfate and water. The copper and hydrogen gas replace each other. Balanced Chemical Equation: CuO (s) + H2SO4 (aq) —> CuSO4 (aq) + H2O (l) Reaction 5: when zinc is added to the copper (II) sulfate solution, a single displacement reaction will occur. The zinc will form a new compound with the sulfate, and the copper will stay as a metal. Balanced Chemical
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
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.
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
Repeat steps 1-10 for two more trials. Conclusion: 1. I chose to compare temperature and amount of reactants in my experiments. I chose these because I thought they would reveal the the most drastic time differences. I also chose these factors because I had prior knowledge of them before I even started chemistry.
Double Replacement Lab Report Date Completed: October 8, 2015 Objective To analyze and determine if a chemical reaction occurred between two compounds using the concepts we learned in class. Also, if the chemical reaction occurred, to determine if it formed a precipitate or gas. Safety General Safety Precautions: Do not touch the chemicals Use of gloves and coats are recommended, use of goggles should be required Keep the work area clean Dispose of the chemicals properly, DO NOT dispose them in the sink Clean up your work station Wash your hand before and after the lab Make sure all chemicals are labeled correctly NEVER return chemicals to reagent bottles Use the wafting technique to smell the chemical Clean up spills immediately
The unknown compound was first reacted with an acid. To begin, 0.50 grams of KCl was mixed with 5 mL of water. Then, 1 mL of 6 M H2SO4 was added to the solution. Secondly, the unknown compound was reacted with a base. Exactly 0.50 grams of KCl was mixed with 5 mL of water, and 1 mL of 1 M NaOH was added to the solution next.
For this lab the knowledge to tell the difference between a chemical and physical changes was needed. To tell this the knowledge of the five signs of a chemical change was needed. These five signs are color change, odor change, production of bubbles/gas, production of heat/light, and the production of precipitate. Also prior to the lab one question was provided that needed to be answered. This question was what chemical must be present for a color change.
Copper is a chemical element with the symbol Cu and atomic number twenty-nine. It is also a solid at room temperature. Copper was most likely the first element ever manipulated by humans. In fact, humans discovered copper during the Paleolithic era. Copper was also very important during the copper and bronze age.
• N. Dirilgen, 1994, Cobalt-copper and Cobalt-zinc effects on duckweed growth and metal accumulation. Different concentrations of Cobalt2+, Zinc2+ and Copper2+ as well as Co2+Cu2+ and Co2+Zn2+ were added to nutrients given to a species of duckweed, Lemna minor L. the effects of these metals on the growth of the duckweed was recorded. A change in growth was not very noticeable until the concentration of Cobalt (Co) and Copper (Cu) reached 2.00 ppm (parts per million), where the growth of the duckweed was inhibited. It was also discovered that Cu and Co work together to inhibit growth when they are at a certain concentration, and at other concentrations, the one would neutralise the other, creating less of an effect on the growth of the duckweed. The conclusion the I took from this study is that as the
Al(s) wire was placed in the solution from the last step and 5 drops of HCl along with a stir bar was added to the beaker and this was stirred on the hot plate. Cu(s) precipitate formed on the wire and the solution turned from clear to cloudy until it eventually become a brownish red color. When the reaction was complete the Al(s) wire was scraped with the stirring rod to get off any residual Copper product. All of the reactions except for reaction 3 were exothermic. This is because each reaction gave
Abstract In this experiment the separation of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved in a methanol solution and filtered out leaving the sodium chloride behind.
Subsequently, the alloy was cast into copper mold. To homogenize the alloys, the ingots were cold rolled to >90% reduction in thickness and re-melted at 180 °C for 10 minutes and cast into copper mold. Finally, the ingots were again cold rolled to >70% reduction in thickness and preserved for subsequent characterization and
- A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.
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
CHAPTER 3 EXPERIMENTAL PROCEDURE 3.1 Materials & Reagents Adsorption of Cu (II) was studied using Montmorillonite-K 10, procured from Sigma Aldrich. It is a very soft phyllosilicate group of minerals that typically form in microscopic crystals, forming clay. Its Cation Exchange Capacity, CEC was 119 meq/100 g .The elemental composition of this clay was [Al1.47Fe0.29Mg0.23][Al0.076Si3.29]O10(OH)2 as reported by the supplier.