The Number Of Copper, Magnesium, Iron, Zinc And Hydrogen In Terms Of Their Reaction

These reactions can be seen from just a little bit of reaction all the way up to a complete change of the entire sample tested. Some samples of those tested in this experiment which showed the chemical reaction were the baking soda/ammonia mixture, the Epson salt and baking soda mixture as well as the food coloring mixed with the baking soda and bleach. 2. Which reactions, if any, do you believe showed no evidence of chemical change? Justify your reasoning.

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

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

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.

I started with elemental copper metal and then reactions occur step by step as follows:

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

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:-

To know if there was a reaction there was seen a color change of the metal of one or multiple of the following a conduction of heat, and fizzing or bubbling. For the reactions that was seen there was (Zn+FeNO3 = Fe+ZnNO3), (Mg+FeNO3 = Fe+MgNO3), (Mg+CuNO3 = Cu+MgNO3), (Mg+PbNO3 = Pb+MgNO3), (Pb+ZnNO3 = Zn+PbNO3), (Pb+CuNO3= Cu+PbNO3). There should have been ten different reactions but the data that was collected was turned up was six, here are the other reactions that should have

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

Table 1 contains corresponding information to figure 1, as already analyzed, despite having the highest concentrated acid solution, zinc has the lowest output of gas compared to aluminum and magnesium. Looking at the trends, aluminum and magnesium have relatively steady increases of mass and corresponding volume (the amount of gas about doubles as the mass is increased by about 0.02 grams). Zinc, on the other hand, increases by almost triple when the mass is tripled, but levels off after and slowly increases in gas production, but is nowhere near magnesium and aluminum. Magnesium and aluminum are much more reactive than zinc in this reaction; the reactivity of both metals can be deducted from their chemical properties on the periodic table;

How do different metals react in different anion solutions? After the experiment was conducted it was very clear on which metal was most reactive in anion solution and which was not with watching the reaction occur. It is clear that zinc and silver nitrate had the slowest reaction as it was creating rust on the metal. The chemical equation for zinc and silver is, Zn+Pb(NO3)-Zn+Pb(NO3)2. Magnesium put in lead creates the quickest reaction. When it had reacted it had a thick layer of lead which brings the magnesium to the bottom. When taken out of the water the magnesium disintegrates. The chemical equation for magnesium and lead is Pb+Mg(NO3)2-Pb+Ag(NO3)2. With using the activity series of metals it helps determine which metal has the highest

LEARNING OBJECTIVES The learning objectives of this experiment are to. . . ! ! determine changes in enthalpy and entropy of the reaction of zinc with copper sulfate using two methods: electrochemistry and calorimetry. compare the enthalpy values obtained by the two methods. BACKGROUND Thermodynamics is concerned with energy changes that occur in chemical and physical process es. The enthalpy and entropy changes of a system undergoing such processes are interrelated by the change in free energy, ªG, according to the equation

The colour of the precipitate was black and were quite small in size, so it was a bit hard to distinguish between the zinc powder present and the copper formed by the displacement reaction because copper formed should be reddish brown is colour – which is also a dark colour and thus two dark colours were hard to be distinguished.

Heavy metals are elements that exhibit metallic properties. It mainly includes the transition metals, basic metals, some metalloids, lanthanides, and actinides. Many different definitions have been proposed—some based on density, some on atomic number or atomic weight, and some on chemical properties or toxicity (Duffus, 2002). Example for some heavy metal are iron (Fe), zinc (Zn), copper (Cu), lead (Pb), mercury (Hg), cadmium (Cd) etc.