Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Chemical reactions lab
Chemical reactions lab
Chemistry chemical reactions lab report
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Chemical reactions lab
Conclusion The Purpose of the Chemical Reaction Lab was to examine and measure the chemical reaction of H-C-L, hydrochloric acid and CuCl2, Copper chloride solution to determine different types of reactions, within specific elements and compounds; Aluminum foil, Al aluminum shot, Ammonium hydroxide, Magnesium, Silver nitrate, Sodium carbonate, Sodium bicarbonate, Sodium hydroxide, and Zinc. By completing the trials, the data displayed chemical changes. These changes were observable in changes of substances, such as formation of precipitate, change in color, release of gas, and difference of temperature. During Part A, formation of precipitate, change in color, difference in temperature and gaseous reactions all took place. Release of …show more content…
In A3 the clear silver nitrate became dense and concentrated when hydrochloric acid was added. In A4 the Zinc became cloudy and grey. Bubbles continued to release sporadically. During the Trials in Part A, a difference in temperature was also observed, but not to large extremities. The temperature Increased 1 degree Celsius in A1 and A3 (27 to 28 Degrees Celsius) When conducting Part B, formation of precipitate, change in color, difference in temperature and gaseous reactions all took place. However unlike Part A more responsive results were recorded. Release of Gas was seen in (B1, B2, B3, B4, A6) as bubbling occurred due to the reaction of Copper chloride with: Aluminum shot, Aluminum foil, Zinc, Ammonium hydroxide, and Silver nitrate. Change of Color and Gaseous release was observed in (B1, B2, B3, B4 ) each had cloudiness, and a change in compression. In B1 the bubbling became gradual and eventually turned the Aluminum shot red in color. B2 had a series of bubbling through the experiment, eventually eroding the Aluminum foil. B3 trial was very responsive to the Copper chloride and the Zinc became Black. B4, Ammonium hydroxide had a thick level of blue above the remaining clear
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
For the chloride test, addition of AgNO₃ formed a white precipitate as silver chloride is insoluble, addition of NH₄OH dissolved precipitate as this forms a silver ammine complex which is soluble, finally the addition of HNO₃ neutralizes the ammonia and a white precipitate reforms (silver chloride). For the carbonate test, when H₂SO₄ is added to the solid carbonate fizzing occurs, which indicates that a gas has been made. As the gas reacts with the drop of Ba(OH)₂ suspended above the solution, a white precipitate forms within the drop. This indicates the formation of barium carbonate which is not soluble, therefore, the gas given off by the carbonate must be carbon
In this experiment, the effect of temperature on the time duration between the first and the
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
For part 1 the theoretical yield was predicted to be 2.78g. When the experiment was finished and the precipitate had rested in an incubator for 24 hours, the actual yield turned out to be 2.75g. 98.9% of the theoretical yield was created. For part 2, using stoichiometry the limiting reagent was predicted to be Pb(NO3)2 while the excess reactant was believed to be NaI. After conducting the test, our hypothesis was confirmed; Pb(NO3)2 was indeed the limiting reagent while NaI was the excess reactant. There were little to no anomalies in this lab.
My hypothesis for this experiment is that the heat study tube will turn blue, the cooling study tube will turn green, the dehydration study tube will turn blue, the hydration study tube will turn green, and the common ion effect study tube will turn blue.
Another problem with this experiment was determining at which stage the solution turned completely clear. I had a black piece of card, which I held behind the boiling tube to see when the solution turned clear, however this was not very efficient. I think that it would have been better if I had gotten a white piece of card and wrote a black letter on it, then looked through the solution until I could clearly see the letter.
Results: The purpose of experiment 5a was to determine the molar ratio between copper and silver. It was found that 2 moles of silver nitrate combine with one mole of copper to yield two moles of silver and 1 mole of copper (II)
However, only experiments IV “Effect of Copper Metal” and V “Effect of Temperature” had reasonable results, so copper metal and temperature are the more effective factors. The less effective factors are the changes in concentrations of "H" ^"+" ions and "C" _"2" "O" _"4" "H" _"2" particles. This observation is represented in experiments II “Effect of "H" ^"+ " Ions” and III “Effect of "C" _"2" "O" _"4" "H" _"2" Concentration.” Both runs 2B and 2C had the fastest times of 25 seconds and 86 seconds
Start by measuring 5.00 mL of commercial bleach in a 100 mL volumetric flask. The bleach was then diluted with distilled water until the contents reached the neck of the flask. Two grams of Potassium Iodide was then weighed out. Then, 25 mL of the diluted bleach solution was transferred into an E. flask by pipet. After that, the Potassium Iodide and 25 mL of deionized water was added to the E. Flash. The content of the flask were then swirled in order to properly dissolve the solid Potassium Iodide. The experiment was then moved to the fume hood, where 2 mL of 3 molar hydrochloric add were added to the E. Flask. The flask was then swirled for 2 minutes in the fume hood to ensure that no chlorine gas was produced by accident. The buret was filled
Having two people in the group, we had one person be a timer and a spectrophometer reader, and the other was the data recorder. After recording the time, we then mixed tubes 2 and 3. We then recorded the data of the combined tube and wrote down the results. After this, we mixed tubes 4 and 5 and completed the same procedure as with tubes 2 and 3 (“Biology” 80). We then had to determine the effect of temperature. We found the results of these four temperatures:
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
The purpose of the lab was to show the effect of temperature on the rate of
The purpose of the experiment is to identify and understand reactions under kinetic and thermodynamic control. A reaction under kinetic and thermodynamic control can form two different types of products. A reaction under kinetic control is known to be irreversible and the product is formed quickly. A reaction under thermodynamic control is known to require rigorous conditions. It is also reversible. The final product is more stable than the product made by kinetic control. The chart below shows the two types of reaction coordinates:
Rate of Reactions Gemma Cockle 9F. The Title of the Report: YOUR NAME: Gemma Cockle YOUR PARTNERS NAMES: Grace O’Sullivan and Georgia Rasch YOUR TEACHER’S NAME: Mr Walters CLASS: 9F DATE OF EXPERIMENT: 09/05/14 DUE DATE: 20/05/14. Aim: To investigate what factors affect the rate of a chemical reaction.