In this lab we demonstrated a series of sequential steps of chemical reactions in an enclosed system, to detect whether the Law of Conservation of Mass applies to the principles abiding by the Copper Cycle. The first reaction was a redox reaction. This utilised Nitric Acid (strong oxidising reagent) to be combined with Metallic Copper, which formed heat from Nitrogen Dioxide (N2), and a dark green colouration (Cu(NO3)2) was observed. Second, was a double displacement where Sodium Hydroxide (NaOH) and Copper (II) Nitrate reacted together to produce blue solution. The third reaction included a black precipitate that decomposed to create Copper (II) Oxide and water, which signifies this is a Decomposition reaction. Next, the black solution transitioned into blue acidic solution. By referring to the solubility chart, SO4 (soluble), and water is the output. Last, a single displacement reaction transpired with zinc additional alongside to the previous solution to generate heat (Hydrogen gas materialises) and solid copper. Though, in the activity series, zinc is above copper, which means that zinc (II) sulphate is made then it begins to decay into another chemical equation. Additionally, it can be stated that, the group …show more content…
In this experimental investigation, the law of conversation of mass is distinctively applicable. Throughout the duration of the entire practical, we conducted a sequence of chemical reactions that comprise of the mass remaining constant with the theoretical/ initial value; albeit, errors eradicated the quantity of copper recovered at completion. Henceforth, the copper cycle is recognised as a biogeochemical cycle that incorporates a chain of reactions that facilitate copper to regenerate to its elemental
An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
Copper is a chemical element with the symbol Cu and atomic number twenty-nine. It is also a solid at room temperature. Copper was most likely the first element ever manipulated by humans. In fact, humans discovered copper during the Paleolithic era. Copper was also very important during the copper and bronze age.
Like silver, the element copper is also oligodynamic. However, unlike silver, copper’s
• N. Dirilgen, 1994, Cobalt-copper and Cobalt-zinc effects on duckweed growth and metal accumulation. Different concentrations of Cobalt2+, Zinc2+ and Copper2+ as well as Co2+Cu2+ and Co2+Zn2+ were added to nutrients given to a species of duckweed, Lemna minor L. the effects of these metals on the growth of the duckweed was recorded. A change in growth was not very noticeable until the concentration of Cobalt (Co) and Copper (Cu) reached 2.00 ppm (parts per million), where the growth of the duckweed was inhibited. It was also discovered that Cu and Co work together to inhibit growth when they are at a certain concentration, and at other concentrations, the one would neutralise the other, creating less of an effect on the growth of the duckweed. The conclusion the I took from this study is that as the
The Single Replacement Lab of Iron Replacing Copper in a Copper (||) Chloride Solution Lab The purpose of this lab was to help the students further their understanding of single-replacement chemical reactions, and to have a hands-on experience with it in order to practice equation writing and stoichiometry functions. In this experiment, an iron nail was placed in a solution of Copper (||) Chloride that was dissolved with water in a baby food jar. Observations were taken over the next three (schools) days.
Copper, magnesium, iron, and zinc were all tested in the same five solution compounds; which included hydrochloric acid, sulfate, magnesium chloride, iron chloride, and zinc chloride. Observations of chemical changes within the reaction were recorded to describe the results of the reaction and each metal's reactivity. An example of a single replacement reaction is the Statue of Liberty, which has copper on the outside and iron as an inner support. As time went by, the copper started to react with air and form a verdigris coat, or a bright bluish-green patina. Meanwhile, a single replacement reaction between iron and verdigris takes place so that Verdigris on the outside is replaced back to copper but the iron support is oxidized and rusted.
ADI Lab: Stoichiometry and Chemical Reactions The guiding question of this ADI lab was, “Which balanced equation best represents the thermal decomposition of sodium bicarbonate?” The goal of this lab was to use our knowledge of stoichiometry with the mole ratio to identify the correct chemical equation for the decomposition of sodium bicarbonate. Information that was given going into this investigation was the definition of the law of conservation of mass and the atomic theory which states that no atoms can be created nor destroyed during a chemical reaction. Also the mole ratio which is used to determine how much of a product will be produced in a chemical reaction using the given chemical equation.
Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s)
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
As the compound was reacting, the aluminum pieces were also dissolving, with only a few pieces left inside. The process of the second reaction included the adding of a new substance which consisted of sulfuric acid. The sulfuric acid along with potassium aluminum hydroxide, was yielded to produce aluminum hydroxide, potassium sulfate, and water. This reaction was both a precipitation reaction and an acid-base reaction. Once the sulfuric acid was added, the reaction became very chunky.
Referencing our data, it can be determined that out of the three metals, Pb, Cu and Zn, it is shown that Lead (Pb) is more active than Copper (Cu) due to single-replacement reaction that took place. Lead had replaced Copper in the solution. Zinc (Zn), however, had replaced Lead thus leaving Copper to be the least active leaving Zinc to be the most active out of the three. In order of activity from least active, to most active, the metals would be lined up as following: Ag, Cu, Pb, Zn, Mg. From this lineup, it was be determined that hydrogen is more active than the elements silver and copper yet less active than zinc and magnesium.
At the conclusion of heating the malachite, the hammer test and the resistance test were performed on the samples of copper to test their physical properties as compared to pure copper metal. The hammer test was performed to see if the sample was malleable since pure copper can change shape easily when force is applied. When the large pieces of malachite were struck with the hammer, they crumbled into smaller pieces and flaked off in layers. The small pieces of copper changed shape readily and were soft in texture. The resistance test was performed to gauge the purity of the copper metal.
Research Question: How does the reactivity of a Metal affect the enthalpy change for a reaction? Aim: To investigate how reactivity’s of various metals (Fe, Mg, Zn, Cu and Mn) affect the enthalpy change of the solution when it reacts with 25cm3 Copper II Sulphate. Theory: Specific heat capacity is the amount of energy needed to raise the temperature of one gram of a substance by 1 degree Celsius. Different materials absorb different amount of heat when their temperature rises by one degree Celsius.
For our mixtures, we placed the metal pieces inside of a small test tube, poured 1-2 mL of the metal ion solution into the tube, waited 30 minutes, and decided if there was a reaction or not. For the second experiment, we dissolved 0.5 g of solid copper(II)nitrate in 20 mL of deionized water and 0.5 g of sodium iodide in a separate 20 mL of deionized water, combined the two solutions, and recorded our observations. Then we combined 2 mL of 0.1 M sodium iodide, 2 mL hexane, and 2 mL of iron(III)chloride in a test tube and recorded our observations. Lastly, we mixed 2 mL of 0.1 M sodium iodide, 2 mL hexane, and 2 mL of 0.1 M tin(IV)chloride in a test tube and recorded our
(-- removed HTML --) . Childs, Peter E. "John Dalton." Chemistry Explained. N.p., n.d. Web. 2 Nov. 2017.