Abstract: The purpose of this lab report is to document what happened to the copper when placed through of series of varying reactions. Reacting copper with varying substances enables a person to enhance their stoichiometry solving abilities and well as differentiate chemical reactions and write balanced equation. The lab was done over the course of five days, with each day catalyzing a new reaction. This resulted in enabling the ability of stoichiometry solving abilities to come easier and quickly identify a reaction, and correctly ending with almost the same of amount of copper at the start of the lab. As a result, we can apply this to the following labs to come. Introduction: The purpose of this lab is to have the ability to observe what occurs during a chemical reaction, as well as being able to write the correct balanced equation for each reaction. While using stoichiometry concepts to also identify the four varying types of common chemical reactions. The four common chemical reactions include synthesis, which when two chemical components unite and become one component. Decomposition, one component becomes divided and Using the electronic balance given, mass the copper wire and record it in the data table. Put the copper into a 150 mL beaker. When placed in the beaker, the Copper needs to be smashed down flat. Place the beaker with the Copper in it, in the fume hood. Proceed to carefully add 12 mL of concentrated Nitric acid ( HNO3 ) into the
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
Repeat for each trial. Rinse volumetric pipette with vinegar and drain into the waste beaker. Weigh and record the mass of each 200mL beaker. Add 10.00mL of vinegar into each beaker and weigh them and record their again. Add 50mL of de-ionized water to the beakers and place them under the drop counter on top of a stir plate, submerging the pH meter into the solution. Place the stir bar into the beaker and carefully turn on the stir plate so that the stir bar spins without splashing or hitting the sides of the beaker or the pH
When the flame was blown out and the glowing wooden splint was placed halfway into the test tube containing H2O2 and MnO2 crystals, the splint reignited and caught flame once again. This demonstrates the decomposition of H2O2 into water and hydrogen. MnO2 is a catalyst that increases the rate at which H2O2 decomposes. Adding oxygen to a fire will cause it to burn faster and hotter and the oxygen rich test tube allowed the splint to reignite.
The purpose of this lab was to to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergo many types of reactions and went through its whole cycle, then returned to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction.
7. Using the stirring wire, stir the mixture until the solute completely dissolves. Turn the heat source off, and allow the solution to cool.
An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases as you move down in the same group. With this in mind, the reactions of the substances involved in this experiment may be hypothesized, observed, and validated.
Rinse your beaker thoroughly to wash any excess powder. 12. Repeat steps 7-11 3 more times for reliability. To make sure the temperature still stays hot by continue heating the water a little bit using the hot plate. 13.
Copper Oxide + Carbon Dioxide (CuCO3 = CuO + CO2) The reactivity series determines how fast this reaction occurs. The reactivity series is the order of metals in the periodic table. The most reactive metals are placed at the top of the reactivity series.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
The Electrolysis of Copper Sulphate Aim Analyse and evaluate the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. Results Voltage across Concentration of solution electrode 0.5M 1.0M 2.0M 2 5.0 10.6 19.5 4 10.5 19.8 40.3 6 14.3 26.0 60.2 8 15.2 40.4 80.3 10 15.0 40.2 99.6 12 15.1 40.0 117.0 Analysing/Conclusion The input variables in this experiment are; concentration of the solution and the voltage across the electrodes. The outcome is the amount of copper gained (measured in grams) at the electrodes. By analyzing the graph, we can see the rapid increase of weight gained for the 2.0 molar concentration as the gradient is steeper.
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
And the symbol equation for it is:. Na2S2O3 + 2HCl, S + SO2 + 2Na + H2O. Before conducting my experiment, I will research into, amongst other things, the factors that affect the rate of a reaction. This is so that I may have enough information to understand the effect of temperature on the rate of a reaction and also gain appropriate understanding to make a suitable prediction as to what the outcome of my experiment will be. Reactions occur when the particles of reactants collide together continuously.
of Copper Sulphate. To do this I plan to work out the amount of water
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and