The Reaction Of Zinc And Iron

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

The purpose of this lab is to test substances and to determine the physical and chemical properties of substances.

The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.

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.

In analysis of the graphs created from the magnesium’s reaction pressure released over time, it appears that we may have had a possible source of error. According to our T.A., the powder should have a faster rate of reaction due to its surface area. However, in our experiment, the reaction rates were found to be similar due to the closeness of the slopes. For the first reaction (trial) of each magnesium type, we had used 0.2 grams due to a communication error. For the second reaction (trial) of each magnesium type, we used 0.02 grams. Despite the mass differences, the slopes were very close to one another but with the ribbon reactions appearing to be faster due to their slightly larger slopes. The ribbon reactions were shown to have a slope in

We began this experiment by obtaining and measuring the mass of a 20 x 150 mm test tube and a 22 x 175 mm test tube with boiling stones. We then weighed out 2 grams of zinc and iodine. First, we added the zinc to the 20 x 150 mm and weighed it out. Then we added the iodine to the 20 x 150 mm and weighed it out. This gave us the amount of each element we were working with before the reaction. Next, we made weak acidified water by adding 18 drops of acetic acid to 25 mL of distilled water in a 50 mL beaker. Then we added 5 mL of acidic solution to the 20 x 150 mm test tube. After the solution is added we swirled the test tube until the liquid became colorless. Once colorless, we poured it into the 22 x 175 mm test tube. We repeated mixing the acid with the zinc and iodine two more times. Then we repeated it 3 more times but poured the solution down the drain. Furthermore, we used a bunsen burner to softly dry off the zinc in the 20 x 150 mm test tube. Once, completely dry we let the test tube

In order to complete this lab students must have a well rounded understanding of the science concepts of the phase of gas and the properties of a gas, the experiment apparatus and how it works, the environment of the procedure including standard temperature and pressure and kinetic molecular theory. To complete the calculations students must understand stoichometry and conversion factors. A gas is a phase of matter that has no shape, no set volume, is easily compressed, and is less dense then both solids and liquids. When matter changes its state, gases can be formed. When liquids vaporize and when solids sublimate gases are formed. In the Molar Volume of a Gas Lab the gas is formed when a measured amount of Zinc metal is combined with five milliliters of Hydrochloric Acid the single replacement reaction occurs causing zinc metal to displace the hydrogen and form hydrogen, a gas and zinc chloride, a salt. In this reaction a gas is formed and bubbles of hydrogen are seen. The apparatus needed for this experiment consists of a small tub of water, graduated cylinder

Because in the data above I concluded that Zn is the most reactive then Fe and the finally Ni I know that Zinc will displace Iron and Iron will displace Ni but Ni will not displace Iron. Because of this if we place one piece of each metal in the solution of Iron(II) nitrate which ever one reacts is the Zinc because the Zinc will be displacing the Iron but since the Ni cant displace Iron no reaction will occur when it is placed into the Iron nitrate.

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

Zinc is known as a cofactor for enzymes included in metabolism and also for appropriate two hundred enzymes in human body as well as a direct participator for the RNA. Because zinc plays an essential in human body energy metabolism and in anabolic, lacking of the consumption of zinc will result in some serious issue, one particular problem is blunts growth (Lukaski, 2000). Some elements can restrain the intake of zinc from diet such as phytate. A event occurred in the early 1960s in the Middle East that people ate the diets containing a high number of phytate which contribute the disease of adolescent nutritional dwarfism in this area. The reason may be that the food these people ate containing one being phytate which damages the absorption of zinc and other minerals (Lönnerdal, 2000). It is confirmed that nearly fifty percent of the world’s population is lacking the consumption of zinc(Prasad, 2003).

This experiment was carried out to understand how Gammarus are exposed to Zinc over a duration of 60minutes. The LC50 was calculated to understand if there is lethal concentration to 50% morality of organisms. In this experiment zinc was used as the toxic product and the organism used was Gammarus. LC50 values were at 45 minutes and 60 minutes. The LC50 value for 45 minutes was 36mg/L and the LC50 value for 60 minutes was 20mg/L.

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

When voltage was measured the nail covered with zinc had the highest average voltage of 0.695267 V followed by Magnesium with 0.307733 volts and the controlled iron alloy had the smallest voltage, 0.2572 V. When current was measured zinc produced the highest current (160.2733 A) followed by Magnesium (52.6733 A) and the smallest was again the control (19.27 A). As shown in the above tables 1 and 2 the mean and median were quite similar throughout testing besides magnesium which wasn’t as close as the others. Explain what that means

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