The reaction that occurred with this step was displacement and metathesis in the form of gas formation. The balanced equation of this step looks as follows: CuSO4aq+Zns→Cus+ZnSO4(aq) Once this step was finished, the remaining copper was retrieved. First, to recover the copper HCl was added to remove all the zinc. When this happened, a yellow tint was observed in the liquid, as well as bubbling as the zinc was broken down. Once the copper dried out, it was weighed and came to a total of 240 mg.
By dehydrating it using fire. The contrast mass between pure solid and solid with water gives the mass of water. 3. What is the formula for copper(II) sulfate? CuSO4 4.
Then weigh the crucible without the hydrate after heating. Record both masses. Next, add CoCl2 ∙6H2O and weigh the crucible. Now place the hydrate and crucible on the hot plate. Observe the color change while it is being heated.
Using Numbers: Calculate the moles of iron used in the reaction. 6. Using Numbers: Determine the whole number ratio of moles of iron to moles of copper. 7. Comparing and Contrasting: Compare the ratio of moles of iron to moles of copper from the balanced chemical equation to the mole ratio calculated using your data.
To ensure that all of the copper is removed from solution, an excess of magnesium will be used. The excess magnesium will be dissolved by the addition of hydrochloric acid. The hydrochloric acid reacts with the magnesium but not the copper. The copper will be filtered, dried, and weighed. As you already know, % Copper = mass of copper X 100% mass of sample This first equation will allow you to determine the percent copper in your sample.
Once the procedure was performed three times, the collected iron fillings mass was obtained by using the digital weighing scale. After removing the iron fillings, the sand was removed next by using the property of sand that the sand was completely insoluble in the water. The iron free solids mixture was dissolved in 15.00 mille liters of distal water and heated by using stove top in a beaker. The solution was mixed for a while the benzoic acid and salt were allowed to dissolve completely and solubility was enhanced by heating the solution. The solution was decanted into another beaker.
The first example is calculating empirical formulas from percent compositions using the percents of the different elements. Empirical formulas of compounds are also determined through quantitative analysis by using the masses of each element in the equation3. Lastly, this experiment uses the method of finding empirical formulas through combustion analysis. The empirical formula of magnesium oxide is found from the combustion of magnesium1. The four chemical equations that result when metal magnesium is heated in a closed crucible that becomes gradually exposed to the oxygen in the air are shown in table
Hydrate Lab The purpose of this lab is to analyze the percent water in a crystalline hydrate and to indentify the hydrate from a list of possible unknowns. The solid hydrate will be heated to remove the water, and the percent can be found by measuring the mass of the solid before and after heating. The hydrate will be indentified by comparing the percent water in the hydrate with the percent water calculated for the possible unknown. Before the lab there are pre-lab questions: 1. Describe the three general safety rules for working with a Bunsen burner.
When the gas comes out of the ground, it comes out wet. The first stage of the refining process involves on-site heating of the gas to 212 degrees to evaporate any non-methane hydrocarbons and fluids that are mixed into the gas. (Arthur, 2008) The condensate that is generated from this process is then vented into the atmosphere. The condensate often contains the same chemical additives that are added to the well during the fracking process, as well as volatile organic compounds that are naturally occurring in the ground where the gas is stored (Witter,
4. Howell iron works purchased came with a furnace which was named Howell Iron works then traditionally pig iron would be worked into wrought iron in finery forges and later putting the furnaces more recently into steel. In these processes, pig Iron is melted and a strong current of air is directed over it while it is being stirred or agitated. This cause the dissolved impurities to be thoroughly oxidized. An intermediate known as refined iron, refined metal, and refined iron.