Abstract Of Cyclic Voltammograms

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

In the United States and in most of the world food dyes are exceedingly common. In addition to this, they have been brought into question as being dangerous for human and environmental health. From general observation and knowledge about this topic I knew that Red #40 dye (Allura Red AC) is at the height of this controversy. After some initial research, I discovered more information on Azo dyes, their effect on the environment, as well as wastewater treatment used to decontaminate water containing these dyes. This led to my interest on the topic of Electrochemical Advanced Oxidation Processes (EAOPs) as a fairly recent solution to environmental issues regarding contaminants in water. I was curious to see how these processes work, as well as

In Part 1 of the lab, a solar cell was created and tested for its capability to conduct electricity. After researching the processes that contribute to the conductive property, it was found that the oxidized substance is the dye, as it donates an excited electron to the titanium oxide. Consequently, titanium oxide is reduced before it donates an electron to the cathode. The electrolyte solution was found to replenish the dye with electrons so it could continue to act as a reducing agent.

Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was

together with the same reactants used before. Thirdly, mix 0.1M Na2SO4 with those reactants. Then, mix 0.1M NaOH with the same reactants used before again.

It’s important for reactions in aqueous solutions to reach equilibrium, meaning that both products and reactants need to be present before continuing to the next reaction or next step. In this experiment, copper was changed through eight different reactions. Throughout the process, qualitative observations were recorded to see what effect each type of acid and decanting has on copper. All of these steps were successfully completed by using different acidic solutions and zinc to take copper through the cycle from copper solid to copper nitrate to copper hydroxide, to copper oxide, to copper II sulfate, and back to copper solid.

The purpose of this experiment was to investigate the chemical reactions involved with oxovanadium ions VO3- and VO2+ to help determine the standard electrode potential for the reaction: VO3− + 4H+ + e− →VO2+ +2H2O. This procedure helped determine the theoretical Eocell.

I also must ensure that the cathode is properly dried before it is weighed so that we can obtain an accurate result. And finally I must make sure that the electrodes are exposed to the same amount of copper sulphate solution so they must be immersed to the same depth and in an equal amount of copper sulphate solution each time.

All the data was fitted satisfactorily using the equivalent circuit shown in Fig. 7. Where, Rs, CPE1 and R1 represent solution resistance, a constant- phase element corresponding to the double layer capacitance and the charge transfer resistance, respectively. CPE2 and R2 were added to account for the electrical elements of the outer layer. The following formula expressed the electrode impedance, Z, as follow:

The higher the gap band energy, the lower the conductivity. The energy (Eg) of cadmium sulfide calculated was 3.92×10-19J which corresponds to 2.45 eV.

Diphenylamine has a lower reduction potential than copper does so it is harder for it to be reduced. Both analytes showed multiple oxidative and reductive potentials. The second reduction potential for diphenylamine was mistakenly not recorded during the experiment. As shown in figure 1, both diphenylamine and copper have coupled current waves. Figure 1 also shows that the peaks for diphenylamine are quasi reversible and the peaks for copper are

In this experiment, a sample of K2S2O8 was prepared by the electrolysis of an aqueous solution of H2SO4 and K2SO4. The peroxodisulfate anion, S2O82-, was also observed for its ability to serve as a counterion for precipitation by preparing a copper (II) complex by reacting hydrated copper (II) sulfate with ammonium peroxodisulfate in the presence of pyridine. This same ability, coupled with its strong oxidizing ability allowed for stabilization of the unusual oxidation state of 2+ for silver which was observed by preparing an analogous silver (II) complex by reacting silver (I) nitrate with ammonium peroxodisulfate in the presence of pyridine. IR spectra for the three products were

In the first reaction, 0.95 g of pure copper was reacted with 4.0 mL of concentrated nitric acid under the fume hood. The solution was swirled until all of the copper had dissolved. The balanced equation for this reaction is as follows:

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

CoO-NiO oxides were prepared as mixed oxide based oxygen carrier, however, the reaction rate was lower than that of its individual oxides due to the formation of a solid solution of NiCoO2. However, carbon deposition was