Lab Report On The Laboratory

Students will place a potato cube into a test tube and add 3 ml of H202 into each tube. Then students will wait one minute and record the height in cm of the bubbles and rate how rapidly the solution bubbles on a scale of 0-5. (0=no reaction, 1=slow,……. 5= very fast.)

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 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

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

To conduct your laboratory exercises, use the Laboratory Manual located under Course Content. Read the introduction and the directions for each exercise/experiment carefully before completing the exercises/experiments and answering the questions.

6. Fe (NO3)3, Ferric nitrate, is much more active than ferrous. It could be identified by its reddish color and when mixed with thiocyanate, it reveals a “bloody” red color.

Instructions: This is a two-part lab. Be sure to follow all steps given in the lab and complete all sections of the lab report before submitting to your instructor.

Seven test tubes were labeled numerically with 2 mL of VO3- and H2SO42- added to each tube. A small pea size portion of solid Na2SO3 was added to the first test tube. Then, 20 drops of distilled water were added to the second test tube. In the third test tube, 20 drops of (.2 M) NaBr were added. Then, to drops of (.2 M) NaNO2 were added into the fourth test tube. A small portion of Fe(NH4)2(SO4)2 * 6H2O was added into the fifth test tube. The sixth test tube had 20 drops of (.2 M) H2Cr2O4 added, where the seventh test tube was the control tube with no additional chemicals added. All the test tubes were left to react for 3 minutes and then heated in a heated bath for approximately 20 minutes.

When the water is so contaminated that you cannot drink it, what could you do to get a pure glass of H2O? Students taking Western Kentucky University (WKU) Dual-Credit “SPAN Chemistry” class at Metcalfe County High School (MCHS) completed a lab investigation of the distillation of contaminated water.

An example of an analogy shown between a water circuit and an electric circuit appears below in Figures – 2 and Figures –

The first lab was to teach us how to use the devices that will be used during this semester. We also learned how to read the data from the data sheets and get important values from the data sheets. Multi-meter and breadboard are used, too. We learned how to use multi-meter to measure voltage, resistance and current and how we build the simple circuit on a breadboard with a NAND gate. We input the voltage and saw the logical voltage out from the

To the above solution 22.3 mg of nonaqueous supporting electrolyte named Tetrabutyl ammonium hexafluorophosphate (Bu4NPF6) was added (approx0.01 M). The Platinum electrode constitutes the working electrode. The Platinum wire and Ag/AgCl (3M KCl) were used as counter and reference electrodes respectively. Differential Pulse Voltammetric measurements were performed at different pulse rates from the potential range of 0.4 to 1.4 V to infer about oxidation and reduction peaks of AMTPAA. The differential pulse voltammogram of AMTPAA showed the reduction peaks at 0.6 V and

A potential set-up was prepared wherein the 25 x 150 mm test tube was filled with K2SO4 (30mL, 0.15 mol) saturated at 0 °C in 5M H2SO4. The test tube was immersed in ice, power supply was adjusted to give the solution a current of ~3.0 amps. Current was read and recorded as accurately a possible, as well as the time over which electrolysis was carried out. K2S2O8 precipitated over a period of 45-50 minutes during which the temperature was maintained close to 0 °C (~8 °C or lower) during electrolysis.

12. The crocodile clips are attached to the copper electrodes of the experimental apparatus and the power supply is turned on. Simultaneously, the stopclock is started. The thermometer is checked every 30s. 13. After 300s the stopclock is stopped and the power supply is turned off. The negative cathode is carefully removed and is dried using a hair dryer. 14. When dry the negative cathode is placed on the electronic milligram balance and its final mass is recorded. 15. The positive anode and negative anode of the experimental apparatus are disposed and the electrolyte is poured out to ensure that the anode slime (impurities) does not contaminate the solution. 16. The electrodes of the experimental apparatus are replaced with new copper strips. 17. Steps 7 to 16 are repeated. However, this time, the rheostat is adjusted using the calibration apparatus until the multimeter shows approximate readings of 0.40 A, 0.60 A, 0.80 A and 1.00 A respectively. 18. Time permitting, the entire experiment is repeated. Safety Copper sulphate may cause irritation and burns if it comes into contact with the eyes. As standard lab procedure, safety goggles and lab coats must be worn at all times. Control of Variables Volume of Electrolyte Used

Concurrent hydrogen (H2) production and phosphorus (P) recovery were investigated in dual chamber microbial electrolysis cells (MECs). The aim of the study was to explore and understand the influence of applied voltage and influent COD concentration on concurrent H2 production and P recovery in MEC. P was efficiently precipitated at the cathode chamber and the precipitated crystals were verified as struvite, using X-ray diffraction and scanning electron microscopy analysis. The maximum P precipitation efficiency achieved by the MEC was 94%, and the maximum H2 production rate was 0.31m3/m3/d.