In this lab experiment, 0.46 grams of copper went through numerous chemical reactions, including being added to nitric acid for an oxidation-reduction reaction to occur, along with going through a precipitation reaction with sodium hydroxide, a decomposition reaction, and double displacement reaction. Theoretically, if 0.46 grams of copper was at the beginning of the reaction, after going through all of the chemical reactions, 0.46 grams should remain. However, due to some loss of copper through the chemical reactions, such as through decanting, only 0.32 grams of copper remained at the end, leaving a percent recovery of around 69.56%. The purpose of this experiment was to determine how many grams of copper remained after allowing it to
The mixture was poured through a weight filter paper and Sucrose washed with a 5ml of dichloromethane. The resulting solid was left in a breaker to dry for one week, to be measured. Left it in the drawer to dry out for a week and weighted it to find the sucrose amount recovered amount.
My goal in this experiment was to determine the amount of zinc (in grams) on 5 different galvanized nails to see if this specific box was up to standard, as well as how consistent the weight of the zinc is on each nail and do so by measuring the weight of the nail initially, then take the zinc off with the hydrochloric
5. A second test tube was then filled with water and placed in a test
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.).
3. The beaker was filled with water and the metal was placed in the water.
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.
The first part of the experiment was to measure an amount of baking soda to start out with. For the first and second time we performed the experiment we used 1 g of
3. Why are the crucible and lid heated at the beginning of the experiment before being weighed?
Introduction: The purpose of this lab was to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergoes many types of reactions and goes through its whole cycle, then returns 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. 4HNO3(aq) + Cu(s) --> Cu (NO3)2(aq) + 2H2O (l) + 2NO2(g) Oxidation reduction reaction Cu (NO3)2(aq) + 2 NaOH (aq) --> Cu (OH)2(s) + 2 NaNO3(aq) Precipitation Reaction Cu (OH)2(s) + heat --> CuO (s) + H2O (l) Decomposition reaction CuO (s) + H2SO Data Results: (mass of copper recovered / initial mass of copper) x 100 Mass of copper recovered: 0.21 Initial mass of copper: 0.52 (0.21/0.52)x100 =40.38%.
This experiment's purpose is to calculate small values (molecular and atomic size) in different phases, such as a gas, liquid, and solid by using practical methods. If the molar mass is known, one can estimate the atomic size through practical measuring techniques with little experimental error. This experiment consists of measuring a block of a solid element (Copper and Zinc), measuring the volume of the lead pellets, and measuring the amount of carbon dioxide gas in a balloon. These experiments will allow one to estimate the atomic or molecular size by using doable measurements and calculations.
The expected moss of anhydrous copper (II) sulfate should have been .834g instead of .694g. The water lost through the heating should have been .471g instead of the .694g that was actually lost. The water lost was much larger while the mass of the anhydrous copper (II) sulfate was much smaller. If the mass of the water lost was too low than something that could have caused this is that the hydrated copper (II) sulfate was not heated correctly. Not all of the water would have been evaporated if the crucible was taken off the Bunsen burner to soon. If the mass of water lost was too large than something that could have caused this is the loss of copper (II) sulfate during the experiment. This could have occurred through the mixing of the hydrated copper (II) sulfate while it was burning on the Bunsen burner.
The purpose of this experiment is to analyze the efficacy and accuracy in determining mass composition of copper in a penny using two methods: atomic absorption spectroscopy and ultraviolet-visible spectroscopy.
of Copper Sulphate. To do this I plan to work out the amount of water
gained at the cathode, so it can be said if you double the time you
== § 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 = == = =