Decomposing a carbonate
By Ronan
Science
8/15/2015
Contents
Background information…..pg2
Aim……pg3
Hypothesis……pg3
Apparatus…..pg4
Method….pg3
Background information
HCI or hydrochloric acid is a powerful mineral acid and is often used in factors and industries. Copper carbonate is a name given to a mineral found in malachite and azurite ores. The reaction between the two elements in its basic form without the heating of copper carbonate. When copper carbonate is placed straight into HCI the reaction makes the HCI become see through and clear but during the process the HCI i become a blue like Colour. The reaction when the copper carbonate is heated and vapour of the chemical is then directed into a chemical called limewater
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(limewater is a diluted version of calcium hydrochloric acid) the chemical turns form its murky white state and turn to a see through Colour. The six types of chemical reaction The first kind of chemical reaction is called combustion. Combustion is where the chemical combines with another chemical. The reaction between the chemical is heat. The chemical reaction called synthesis is where two chemicals combined to make a more complex chemical. The reaction when a complex compound destroy a simple compound is called decomposition. Double displacement is where the anion and the cations that are held by two different elements switch places with each over when this happen it creates two very different compounds. A single displacement is simile to a double displacement but it is where the element changes place with another element. The last reaction is called acid-base the is a rare kind of reaction what happens is the acid base has a reaction with the H+ ion an the acid reacts with the HO ion. When this happens the final concoction is water. What is a decomposing reaction A decomposing reaction is where a compound is divided into two or more compounds.
This only happens if the condition is suitable and are met. Saying this there are two differences there is an ionic a covalent reactions. An ionic bond is where two opposite ions connect to each other. A covalent bond is where two nonmetal atoms share there electron with other atoms and covalent bonds.
Aim
The aim of the experiment is to decompose copper carbonate by heating it.
Hypothesis
If by heating the copper carbonate in a test tube. The Colour of the carbonate will change to a light blue and will being to bubble sending the gases that are released from the copper carbonate into the tube of lime water. The lime water will react by bubbling a producing a gas and the Colour of the liquid will whiten. The reason this will happen is because of the reaction of the gas that the copper carbonate will produce by being heated.
Apparatus
1x Bunsen burner
1x heat mat
1x box matches
1x glass tube
1x rubber stopper
2 x retort clamp
3 x test tube, medium (~150 x 15 mm), borosilicate ("pyrex")
1 x spatula
1 x electronic scales
Copper carbonate (approx. 5g)
50ml lime water
1 x Hydrochloric acrid (10 ml) 1m
1 x 5ml measuring
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cylinder 1 x test tube tongs 1 x plastic pipette 1 x watch glass Method part A 1. Put the first clamp approximately 17-20 cm on top of the base of retort stand. 2. Pick up the watch glass and put it down on the electronic balance 3. Press the “Tare” button to eliminate mass of watch glass 4. Measure 2 grams of copper carbonate using a spatula, place on top of watch glass and add or subtract to the correct amount. 5. Place copper carbonate into test tube with glass funnel 6. Place test tube inside of clamp and tighten accordingly 7. Put delivery tube and stopper on the test tube with the Copper Carbonate inside of it. 8. Measure 15 ml of Limewater into measuring cylinder and put into the second test tube. 9. Place the second test tube into test tube rack. 10. Place the other end of the delivery tube into the test tube just until it is touching the limewater. 11. Turn the match then on turn the gas on for Bunsen burner. 12. Light the Bunsen burner with the match 13. The Bunsen burner must be on a heat mat before turning the Bunsen burner on. 14. The Bunsen burner must be on a safety flame which is when the holes are covered. 15. You must turn the cover to blue flame on the Bunsen burner. 16. Place the Bunsen burner under the Test Tube that has the Copper Carbonate. 17. Twist the cap of the Bunsen burner until the holes are showing and the blue flame has appeared. 18. Record observations. Part B 1. Remove lime water before stopper 2. Measure 5ml of HCL in a measuring cylinder 3. Pour 5ml of HCL into the test tube that contains copper oxide 4.
Measure 2 grams of copper carbonate into a watch glass
5. Use a funnel to put copper carbonate into an empty test tube
6. Measure 5mL HCL in measuring cylinder
7. Add 5mL HCL to test tube that contains copper carbonate
8. Observe results
Results
Results for part A: when the copper carbonate is heated it produced a gas called copper dioxide the gas flows into the limewater. The limewater becomes cloudy and begins to bubble due to this the limewater becomes white and milky the limewater’s test tube also begins to heat up. When lifted up the test tube is clear at the bottom, white and murky at the top.
Results for part B: the copper carbonate is put into the test tube that contains the copper oxide. The affects which follow are that the colour changes from blue to an aqua green colour. the other test with copper carbonate and HCL has the same change but instead of the mixture turning green it become crystal clear.
Discussion
The experiment has gone exactly as planned as was stated in the hypothesis. The colour of the lime water changed due to the reaction that happened when the copper carbonate was heated and the copper oxide is released into the limewater. Along with this the second experiment consisting of placing the HCl in the copper oxide and the mixture turn to a greenish blue
colour. During the experiment in heating the copper carbonate and turning it into copper dioxide. We failed to remove all the oxygen from the copper carbonate. Continuing on with the experiment we attempted to proceed with the experiment because we did not know of our fault until we a poured the HCL inside. This did not affect the experiment. The evidence shown that copper oxide was formed it how the limewater has reacted to the copper oxide. It reacted by becoming murky and white in colour along with bubbling to the vapour. The copper oxide was made when the copper carbonate was heated and the copper oxide left. Evidence that suggests this happened is when the copper carbonate when heated became a light blue colour. The equation for the experiment is CuO (s) + CO2 (g) = CuCO3 (s)
Put 1mL of 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol into a test tube. Then add 1mL of deionized water. Tap the end of the test tube to mix the solution and record the pertinent data in section 2 of the Data Table. Discard the solution in the appropriate container as directed to you by your lab instructor.
This experiment will determine the levels of Vitamin C present in each of the different fruit juices selected. The level of Vitamin C will be compared between each fruit juice to determine which one has the highest amount of Vitamin C. Several drops from one fruit juice will be mixed into an iodine solution then repeated with a different fruit juice. With every drop of fruit juice a chemical reaction occurs and the process continues until the solution becomes colorless. The reaction will vary in according to the amount of Vitamin C present in each one of the different fruit juices.
In the second experiment with the green color, I can safely conclude that the color green in this case is very soluble and we would need longer filter paper, perhaps more time to safely separate the different colors that make up the color green.
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.
Rate of Reaction Between Calcium Carbonate and Hydrochloric Acid Plan: In my experiment I will measure the rate of reaction between calcium carbonate and hydrochloric acid. The rate of the reaction is the speed that the reaction takes place so by measuring the rate I will measure the amount of time the reaction takes. Hydrochloric acid is a strong acid that is found in digestive juices in the stomach, it is also used for cleaning metals before they are coated. Calcium carbonate has a few forms including chalk and limestone the main use of these two materials is in the making of concrete, which is used for many things such as buildings. When you put calcium carbonate and hydrochloric acid together they react to form calcium chloride, carbon dioxide and water.
The aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
== = == Hypothesis for the experiment: After I conduct this experiment, I expect and suppose I can recognize and physical changes, identifying the difference these two kinds of changes. Also, I will be able to know some physical and chemical properties of copper (II) sulfate, water, iron, sodium carbonate, hydrochloric acid and magnesium and identify if it is a chemical change or physical change in each part of the experiment.
I have been a snob. It is quite soft, but solid. It reacts with hydrochloric acid. like this 2 CaCO3 + 2 HCl â’ CO2 + CaCl2 + H2O. producing carbon dioxide, which is what we measured in the experiment. There are different factors affecting the rate of this reaction, such.
A cuvette was filled 3/ 4ths of the way and the absorbance measured in a spectrophotometer. The data was compiled as a class and recorded. The Spectrophotometer was blanked using a test tube of distilled water.
This is called copper oxide. The copper carbonate has been decomposed. Copper oxide is made by thermal decomposition of copper carbonate. Carbon dioxide is also made. The formula for this is: Copper Carbonate =
Strong heating of calcium carbonate produces calcium oxide, CaO, and carbon dioxide. tlcQeA from tlcQeA coursewrok tlcQeA work tlcQeA info tlcQeA CaCO3(s) à ƒaO (s) + CO2 (g)coce cer sececew orce cek ince foce ce. Limestone is given the equation CaO, slaked lime is produced when CaO reacts with water, this is where further amount of H2O is added which turns this into a saturated aqueous solution known as limewater. Ca(OH)2 (aq) and is used for tests to show the presence of CO2.
From the Results there is an anomaly which is with the test tubes at 58oC, the results spike from 0.100 to 0.536 and then back down to 0.302, this anomaly may have happened due to the three samples in the test tubes potentially having a higher level pigment in the vacuole than the other
The ingredients that will be included are: dish soap, 30% hydrogen peroxide, potassium iodide, and corn starch. Adding the cornstarch to the mixture has a chemical reaction to the hydrogen peroxide. It will have light and dark patches due to the uneven placement of the cornstarch; it will have an uneven reaction. Which will then make it appear “glowing”. The fourth experiment is very similar when it comes to the ingredients the only thing that changes is that we are no longer using potassium iodide but we are using yeast instead. Also, since yeast is being used, we are adding in fluorescent dye to it so we can shine a UV (ultraviolet) light on it to see the reaction occurring. Using the dye under a light helps us observe the reaction between the dye and cornstarch. I had to replace the potassium iodide with yeast for a slow reaction and also so it is possible to use the dye. In both of these experiments the reaction is a massive production of foam. The hydrogen peroxide will be decomposed into water and by the oxygen by the iodide and/or the yeast. A substance called catalyst speeds up the
== § 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 = == = =
We took pictures of each other’s data once finished with the lab. For the paper chromatography, students began by grinding 5g of spinach along with 2g of anhydrous magnesium sulfate. Students added hexanes and acetone as specified by the lab protocols. Once, the solvent was a dark green color, we placed it in a centrifuge and transfer the liquid portion of the solution into a test tube. Throughout this portion of the experiment, students used weighting paper as a funnel poring the indicated solution as stated by the protocol, for instance pouring silica gel and sand into the column. After, we poured about 3ml of Hexanes into the column, making sure not to let the column dry. We then added, spinach extract to the column—after, we added about 1ml of hexanes. Adding hexanes caused the solution to gain a yellow colored band. We added hexanes until the yellow band reached the bottom of the column, thus began to collect all the yellow pigment into a test tube. Once the elutant become colorless, we once again placed a waste basket under it. Finally, we collected the green pigment into another test tube by a 70%/ 30% mixture and a bit of acetone. Once the two colored bands were collected, we obtained the wavelengths of each colored band using the