Introduction The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in …show more content…
Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper. 5. Define decant. Decant- to pour off only the liquid from a container that is holding both solid and liquid. DATA Before the reaction: | After the reaction: | Mass of empty, dry beaker ---- 48.88 g | Mass of two iron nails-------------- 4.92 g | Mass of beaker + copper (II)---- 101.62 g | Mass of beaker + copper (dry)---- 0.47 g | Mass of 2 iron nails--------------- 4.92 g | | CONCLUSIONS 1. Find the following masses. a. Mass of iron used in the reaction 0.18 g b. Mass of copper produced 0.49 g 2. Find the number of moles of the following. a. Moles of iron used 0.0011 mol b. Moles of copper produced 0.0077 mol 3. Find the number of atoms of each of the substances involved in the reaction. a. Atoms of iron used 5.478 Fe atoms b. Atoms of copper produced 4.214 Cu atoms 4. Calculate the ratio of moles of copper produced to moles of iron used. Ratio 2 : 1 5. Was there any evidence that some of the copper (II) chloride was left in the beaker? Explain. Yes, because the solution seen was still blue meaning that not all the copper chloride was extracted from the beaker. SYNTHESIS 1. Suppose that you have an unlimited supply of copper (II) sulfate to react with iron. How many moles of copper would be
If 5 moles of P4 reacted with 22 moles Cl2 according to the above reaction, determine:
This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.
Beran, J. A. Laboratory Manual for Principles of General Chemistry. 8th ed. Hoboken, NJ: John Wiley & Sons, Inc.; 2009
After 1 minute, a slight change in the color of the iron strip was noticed. It became somehow darker.
The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu
How many moles of NaOH would be needed to completely react with all of the excess HCl determined in problem 8?
The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as
In your laboratory notebook sum these two reactions to find the stoichiometric factor that relates moles of
In the scenario described in problem 7, what is the amount (in moles) of excess
The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.
Before the synthesis of the Copper Iodine Compound, the identities provided (CuNO3)2 and Nal weighed 1.65 g and 4.7 g, respectively. After being weighed, the (CuNO3)2 exhibited a blue color, while the Nal, through observation, was a white color. However, when both identities were combined, the product turned into a brown and red rocky material. Once 20 mL of deionized water was added, the product quickly turned pale pink paste. After the solution was repeatedly washed with a total of an additional 100 mL of deionized water, the product was powdery and pink with small grains, and was left to air-dry. Once the product was air dried, it was observed to be a pale pink color, while the filter paper was stiff as the product was hard and dry. Therefore, the solid was scraped off onto a recrystallizing dish. However, the mass of an empty recrystallizing dish needed to be recorded in order to compare how much of the synthesized copper iodide was obtained. Within this case, the empty recrystallizing dish used weighed 32.01 g, the product on the empty dish weighed 1.03 g, having a total weight of 33.04 g.
XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.
Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.
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 lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-