Metal Chemistry Experiment
Aim
My aim is to plan and carry out an investigation that will enable me
to put 5 metals in order of reactivity. The 5 metals are zinc,
magnesium, copper, iron and calcium. I am also provided with Copper
(II) Sulphate solution.
Equipment
Zinc, magnesium, copper, iron, calcium, 500 cm3 CuSO4, Polystyrene cup
with lid, thermometer, measuring cylinder, stop watch, spatula and
safety specs.
Safety
In the experiment I am using substances that are irritant and harmful.
Throughout the experiment I will wear safety specs. I will make sure
the chairs are kept in and all loose objects are not around. I will
work carefully with the chemicals, so I do not spill any.
Plan
After making sure everything is safe, I will first start the
experiment with zinc. I will measure out 25 cm3 of CuSO4 in a
measuring tube. Then I will put it into a polystyrene cup with the
lid. I will insert a thermometer through the lid of the cup until it
touches the liquid. Then I will take one spatula of zinc. Before I put
it into the cup I will take the starting temperature of CuSO4. I will
write that down on a table already made. Then I will put the zinc into
the cup, close the lid and start the timer. I will mix the solution by
shaking the cup to increase the surface area.
If I increase the surface area the rate of reaction increases because
there is more chance the particles will react, as there is more
surface area. This will speed up the experiment.
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Every 30 seconds I will take the reading of the temperature. After 2
and ½ minutes I will stop the timer. Then I will empty the solution
into the sink and wash the cup and the thermometer. I will do this two
times for zinc, so that I have an average of results. This experiment
will be carried out with all the metals, a total of 15 experiments.
...ease the speed to medium. Slowly add the remaining sugar to the egg whites and continue to mix.
in 5cm³ of water and add 4cm³ of ethanol. We had tom pour this mixture
Third, grab the left edge of the Kool-Aid packet between your thumb and index finger. With your other hand, begin peeling the upper-left corner until the entire top of the envelope is removed. Next, dump the contents of the envelope into the pitcher. Notice how the powder floats before settling on the bottom of the pitcher. Then, take the measuring cup and scoop two cups of sugar into the pitcher as well. At this point, adding the water is a crucial step. Place the pitcher under the water faucet and slowly turn on the cold water. If the water is turned on too quickly, powder will fly all over when the initial gusts of water hit. After the pitcher is filled within two inches of the top, turn the water off and get prepared to stir. With the wooden spoon submersed three-quarters of the way in the liquid, vigorously stir in a clockwise motion until all of the powder is dissolved.
The experiment we did was Copper Cycle. We reverted the copper to its elemental form after a chain of reactions. We performed a series of reactions, starting with copper metal and nitric acid to form copper (ii) nitrate. Then we reacted copper with sodium hydroxide, sulfuric acid, nitric acid and zinc to form precipitates. In conclusion our percent recovery was 40.38%.
4. Pour about 300mL of tap water into the beaker. Set up a hot-water bath using a hot plate, retort stand, and thermometer clamp. Alternatively, use a Bunsen burner, retort stand, ring clamp, thermometer clamp, and wire gauze.
Set up a ring stand in order to support the separatory funnel and place 100ml of beverage into the separatory funnel.
The expected moss of anhydrous copper (II) sulfate should have been .834g instead of .694g. The water lost through the heating should have been .471g instead of the .694g that was actually lost. The water lost was much larger while the mass of the anhydrous copper (II) sulfate was much smaller. If the mass of the water lost was too low than something that could have caused this is that the hydrated copper (II) sulfate was not heated correctly. Not all of the water would have been evaporated if the crucible was taken off the Bunsen burner to soon. If the mass of water lost was too large than something that could have caused this is the loss of copper (II) sulfate during the experiment. This could have occurred through the mixing of the hydrated copper (II) sulfate while it was burning on the Bunsen burner.
In this lab experiment, 0.46 grams of copper went through numerous chemical reactions, including being added to nitric acid for an oxidation-reduction reaction to occur, along with going through a precipitation reaction with sodium hydroxide, a decomposition reaction, and double displacement reaction. Theoretically, if 0.46 grams of copper was at the beginning of the reaction, after going through all of the chemical reactions, 0.46 grams should remain. However, due to some loss of copper through the chemical reactions, such as through decanting, only 0.32 grams of copper remained at the end, leaving a percent recovery of around 69.56%.
the iron ore to iron. In the other cases of metals the most common way
The procedure is very short. First, I constructed the data table. I then massed one piece of Aluminum foil and record it in the data table. Next, pour 25.0 mL of 0.400 M Cu²+ solution and tear up the massed piece of foil. Drop the torn pieces in the solution and record the observations. Mass the other pieces of Aluminum foil, tear it up, and drop it in 25.0 mL of the 0.200 M Cu²+ solution. Record observations and clean up according to the teachers
Before the experiment, I wrote down a prediction. My hypothesis towards the experiment was that magnesium would have a bigger reaction with the acids. The reactivity of an element depends on its ability to gain or loose electrons which are used for bonding. The more reactive an element, the more easily it will combine with others. From this information, I know that magnesium has a stronger ability to gain or loose electrons which makes the metal more reactive.
2nd step heat the mixture: Make sure the agarose dissolves. Wait until it boils and when you are going to transfer the mixture, wear gloves to avoid getting burnt. Transfer the mixture into a removable gel tray.
Metals possess many unique fundamental properties that make them an ideal material for use in a diverse range of applications. Many common place things know today are made from metals; bridges, utensils, vehicles of all modes of transport, contain some form of metal or metallic compound. Properties such as high tensile strength, high fracture toughness, malleability and availability are just some of the many advantages associated with metals. Metals, accompanied by their many compounds and alloys, similar properties, high and low corrosion levels, and affects, whether negative or positive, are a grand force to be reckoned with.
In a 250ml beaker place 100mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved. After 1 minute measure the temperature and record it, do this for a further 2 minutes (3 minutes in total). Repeat this process for a total of 10 teaspoons.
Metallurgy is the field of materials science and material engineering that studies the physical and chemical behaviour of metallic elements, their microstructure compounds and their mixtures, which are mostly known as alloy. Metallurgy can be refers as the technology of metals where science is applied to the production of metals, and the engineering of metal components for the uses of products for consumers and manufacturers.