Chemical Reaction Lab Report

The mole ratio is found by dividing the number of moles of each element with the number that has a smaller amount of moles.

4. Calculate the ratio of moles of copper produced to moles of iron used. Ratio 2 : 1

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

Determine the mole ratio-the ratio of the number of moles of silver to the number of moles of copper. Note: Round the results to the nearest whole number

In this lab there was a performance of a single replacement chemical reaction. The reactants of the reaction was solid iron metal, and copper (II) sulfate solution. This was a gravimetric lab and therefore it was crucial to begin by massing the reactants individually. The copper (II) sulfate was initially a solid. A procedure was conducted to dissolve the copper (II) solid by heating it in water to create the necessary solution. Once that was complete the following action was to react the solid iron and the copper (II) sulfate solution. The single replacement chemical reaction took place and there was a replacement of copper with iron. The products of the reaction was solid copper metal and an iron (II) sulfate solution. The solid copper was

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

The main purpose in doing this experiment was to figure out how much of the percentage of Copper’s mass is in a brass alloy using a spectrophotometer that is hooked up to the laptop. Another purpose in doing this experiment is to learn how to use the Beer’s Law plots to learn how to use the equation and get the correct concentrations. This is important in everyday context because it is important for people who work doing many different types of jobs. Safety Information: In this lab, we used nitric acid to reactant with copper.

According to the Law of Conservation of Mass, the mass of the products must equal the mass of the reactants, so logically one would expect that if 2 g of copper was used to start the lab, the lab would result in 2 g of copper. Unfortunately, that was not the case in this lab, and the final mass of copper exceeded the initial mass by 4.841g. There were many different sources of error throughout this lab, and I believe that this was the reason for such a significant difference between the initial and final masses and moles of copper that were calculated. The first step of the lab was to measure 2 g of copper and place it in a beaker. Error may have occurred at this step if the balance that was used to weight the copper was not calibrated correctly, or if the amount of

First we have to find the Balanced Equation: Fe2O3 + 3CO yields 2Fe + 3CO2 Then you would need to find your number of moles for Fe, which is 0.07890 Then you would need to find your number of moles for CO, which is 0.34451 So that also helps us because it tells us that 1 singluar mole Fe behaves with 3 mole CO. 0.07890^3 mole of Fe which gives us a total of 0.2367 mole 1 singular mole of Fe behaves with 2 mole of Iron, you would then do 0.07890^2 to get: 0.1578 mol of Iron. Then you would take 55.845 (iron's singular mole) and multiply it by the 0.1578 and that would be the theoretical yield which is 8.812341

Procedure: First you will need to get all the lab equipment and material that is needed to do this experiment. After that fill the 150ml beaker to ¼ full of water. Than you will be provided by a teacher or an instructor who will give copper with an scoopula. Than pour the copper that was provided into the beaker, before you stir

The change in colour of the copper wire from bronze to black signifies that the composition of the copper wire have changed during the heating process. The copper wire, Cu had reacted with oxygen, O2 during heating and forms a new substance that is copper oxide, CuO. As the composition of the copper changes with the presence of oxygen, the chemical properties have also changed and thus this causes the resulting substance, copper oxide, CuO to differ physically and chemically with the original substance, Copper, C. Thus, it can be concluded that the heating of copper wire causes a chemical change to occur. Meanwhile, the change in physical state and colour of the iodine crystals, I2 during heating does not signify that a chemical change has taken place.

In order to calculate the concentration of iron in an unknown substance, many steps had to be taken. First, a stock iron solution was prepared by measuring exactly 0.0135g of ferrous ammonium sulfate [Fe(NH4)2(SO4)2·6H2O], mixing it with approximately 5.2mL of 2.0 M H2SO4, and diluting the solution to 200mL. Following this, a diluted 1,10-phenanthroline solution was prepared by obtaining approximately 50.0mL of 1,10-phenanthroline monohydrate in ethanol solution and diluting it to 200mL with deionized (DI) water. Then 9 200-mL volumetric flasks were cleaned and labeled A-I. Flasks B-F were filled with exactly 2.00, 5.00, 10.00, 25.00, and 50.00 mL of the stock iron solution respectively. Flask A was used as a control and was instead filled with 100mL of DI water. Flasks G,H, and I were filled with exactly 25.00mL of Unknown Iron Solution E0717. Then all flasks A-I received approximately 2.0mL of hydroxylammonium chloride solution,

Millimoles of Fe (II) in each solution = (10.00 mL) x (MB). = 10.00 x 0.000694 = 0.00694 millimoles. Mole ratio ‘n’ = (millimoles of ortho-phenanthroline at intersection)/(millimoles Fe^(2+) in each solution ) =0.0196/(0.00694 )=

In relation to this experiment, the per cent recovery, or “how much of the original pure copper mass recovered at the end of the experiment”ii iii iv v should be 100% because all of the copper should return to elemental form. However, the per cent recovery from this experiment was calculated to be 56.5% recovery, much lower than the anticipated value, and therefore does not appear to support the Law of the Conservation of Mass. One explanation for the per cent recovery being too low would be that some copper was lost while decanting the solution after reaction three. The time constraints also should be taken into consideration, as if the reaction resulting in the precipitation of copper by the aluminium wire was allowed to run longer, more of the copper could have been precipitated out of solution, closing the gap toward the 100% recovery. The product of the reaction was a dark reddish brown colour.

In “Part 3: Preparing Copper (II) solutions of Different Concentrations”, 20.0 mL of a 0.500 M solution was from CuSO4 * 5H2 O was made. The solid was weighted and was added to the 100 mL beaker. About 15 mL of water was added to the same beaker. The mixture was transferred back and forth between the graduated cylinder and a beaker to dissolve all the crystals. The solution was transferred back to the graduated cylinder. The beaker was rinsed well with a small amount of distilled water and the rinsed solution was transferred to the same cylinder containing the dissolved solid. After adding the solution, the total volume in the cylinder was about less than 20 mL. With the use of the Pasteur pipette, the water was added until the volume in the cylinder was 20 mL. This was the first solution.