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. Zinc was able to replace the hydrogen present in hydrochloric acid. This leaves hydrogen to be less active than
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
Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.
Metal cations can be identified based on the colors they emitted off when heated in a flame.1 When atoms of the ions that were tested are excited, their electrons move up to higher levels of energy.2 When the electrons relax and return to the original states, they emit photons of specific energy creating wavelengths of light that produces colors.3 The test wire and Bunsen Burner were used to excite the solution in the crucible. The standard metal cations that were tested and their outcomes are as shown in Table 1.
While the absolute value of slope of the graph for the solution containing only 0.5 mL mitochondrial suspension was 4 x 10-4, the slope of the graph for the solution containing 0.5 mL of mitochondrial suspension, 0.5 mL of 100 mM succinate, and 0.5 mL of 100 mM malonate was 7 x 10-4. Although this change is not large, it does demonstrate that the addition of TCA cycle intermediates has an impact on reaction rate. The decrease in the rate of reaction of the sample containing 0.5 mL of mitochondrial suspension, 0.5 mL of 100 mM succinate, and 0.5 mL of 100 mM malonate as compared to the sample with only 0.5 mL of mitochondrial suspension and 0.5 mL of 100 mM succinate shows that the addition of malonate inhibits the reduction of
The purpose of the lab was to discover the properties and the trends of the alkaline earth metals. In part A, the trend was as the atomic number increase in the alkaline earth metals the elements are more reactive. The alkaline earth metals each have two electrons in their outer shell and because all electrons want to become stable they are ready to give up the two electrons. When they are combined with water, the chemical reaction occurs differently based on each element.
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
In this experiment, the ions that go through gravimetric analysis are the copper and sulfate ions (Grossie and Underwood, 25). Elemental analysis involves determining the amount, which is usually a percent, of an element present in a compound (Blauch, 1). In this experiment, the element going through the elemental process hydrogen, in which the percent of the compound is attempted to be found (Grossie and Underwood, 25). In order to find the amount of copper, copper oxine needs to be formed. To find it, there is a reaction of hydrated copper sulfate and oxine, producing copper (II) oxine (Grossie and Underwood, 25).
The Hydrolysis reaction included an acidic environment and an acidic catalyst to make the reaction occur faster and initiate the reaction as well. The acidic environment is required in order to add the hydrogen and oxygen onto the carbonyl groups in the final product. Dicarboxylic acid is not very soluble in water/acetone which ultimately resulted in larger yield of product. 2.
+ H2O (g) Reaction 4: when a sulphuric acid is added to the solution that contains copper (II) oxide, a double displacement reaction will occur. the copper (II) oxide will react with the sulphuric acid producing copper (II) sulfate and water. The copper and hydrogen gas replace each other. Balanced Chemical Equation: CuO (s) + H2SO4 (aq) —> CuSO4 (aq) + H2O (l) Reaction 5: when zinc is added to the copper (II) sulfate solution, a single displacement reaction will occur.
This classification is based on several characteristics: 1) zinc is a metal essential to hundreds of biological processes 2) zinc is relatively abundant in the natural environment; 3) the recommended daily allowance(RDA) of zinc in the human population is 8 to 15 mg higher than many other essential metals, 4) zinc does not appear to accumulate in the body with age , 5) there are no known genetic abnormalities which result in excessive accumulation of zinc in the body, unlike metals such as copper (Wilson's disease) and iron (hemochromatosis). The US Environmental Protection Agency standard for maximum zinc concentration drinking water is 5
The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.
Lead, when written as a half reaction on the Standard Reduction Potentials table, tends to lose or gain 2e−. Lead is placed towards the bottom of the SRP table, making it a weak oxidizing agent and a strong reducing agent. Therefore, when reacting with entities above it, lead oxidizes (loses electrons). It’s position allows lead to participate in redox reactions with many substances, specifically, oxygen in the process of corrosion. When exposed to oxygen and moisture, lead atoms in an anodic region will each lose 2e−, forming Pb2+ ions.
2.5.4. Metal chelating activity Briefly, 2 mM FeCl2 was added to different concentrations of test sample and reaction was initiated by the addition of 5 mM ferrozine. The mixture was vigorously shaken and left to stand at room temperature for 10 min. Absorbance was measured at 562 nm after 10 min.8 % Inhibition = [(AB - AA)/AB] x 100, where AB, absorption of blank sample, AA, absorption of test sample.
The zinc acts as the anode and the copper acts as the cathode. Copper has a higher electronegativity than zinc, so the bonding electrons in zinc leave and flow into the copper. However, this reaction would not be possible without the lemon in the experiment, which acts as an electrolyte because it contains citric acid in the form of lemon juice. When the zinc comes in contact with the lemon juice, oxidation occurs within the zinc. Oxidation is a process where an element loses electrons in a chemical reaction.