Purpose To observe the reactions, and appearance of the magnesium strip when it come in contact with two different compounds. Introduction This lab experiment focuses on single displacement reactions which occurs between an ionic compound and a single element. The general chemical equation is: AB + C → CB + A (A = metal, B = non-metal, C = element) As you can see, in this reaction the element C replaces the metal A, and forms a compound with non-metal B. Hypothesis I predict that the zinc chloride will corrode the magnesium metal strip because this substance is known to be ‘mildly corrosive’. Since the zinc chloride is only mildly corrosive, I don’t expect the metal to look brittle, or have many visible marking. Also, ZnCl2 is often …show more content…
I predict that the copper(II) chloride will corrode the magnesium metal strip, and there will be visible markings. Copper(II) chloride is known to corrode aluminum metal, and aluminum is known to be more resistant to corrosion than magnesium. magnesium + copper(II) chloride → magnesium chloride + copper (Mg + CuCl2 → MgCl2 + Cu) I also expect the magnesium to combine with the non-metal, chlorine to form an ionic compound (MgCl2) while copper is left isolated. Materials spotting tray 2 magnesium pieces/ ribbons (Mg) zinc chloride solution …show more content…
When the chemicals came in contact with each other, almost all them had an immediate and visible chemical change. The exception is the combination of sodium chloride and potassium nitrate. I saw a similarity in appearance of the reactions between sodium chloride with silver nitrate and sodium carbonate with calcium chloride. They both appeared translucent and cloudy white after their reaction. Discussion A chemical reaction did occur in every combination, however no signs were shown for combination d) between sodium chloride and potassium nitrate. Indications of a chemical reactions occurring between these two compounds were not present, as in the colour did not change, and gas, heat, light nor sound was produced. In addition, when sodium chloride and potassium nitrate combine they form sodium nitrate and potassium chloride. The products sodium nitrate and potassium chloride are both aqueous, therefore no precipitate was formed either. Word equations and balanced chemical equations: sodium chloride + silver nitrate → sodium nitrate + silver chloride (NaCl + AgNO3 → NaNO3 + AgCl) silver nitrate + potassium iodide → silver nitrate + potassium
An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
The process of filtration can be used seeing as the copper particles will be caught by the filter because they are too large to pass through it, while the aluminum chloride particles are small enough to pass through the filter. In order to filter the products, one needs to obtain a funnel, filter paper, and a clean
Copper/ Red Stuff/ Chemical Reaction The purpose of this experiment was to determine what the red stuff that was produced was. We put aluminum foil in a test tube filled with 100 milliliters of copper chloride. During the experiment, I observed that the aluminum foil was breaking away, the aluminum foil that was breaking away was turning into red stuff. After a while, the once light blue copper chloride was turning into a dull gray, almost clear.
George i Whitlatch describes the value of manganese classified into chemical and metallurgical
In this reaction NaOH was added to the Cu(NO3)2. The solution developed a precipitate which made the clear solution become cloudy and uniform in color (blue). The physical color change was demonstrated through the formation of the precipitate. The third step was the formation of CuO. In this reaction, the Cu(OH)2 product was heated on a hot plate and stirred continuously until the solution became colorless and a dark precipitate formed.
Tayjza Burks Mr. Irwin Physical Science 2 2/21/17 The element I will tell you about toady is Magnesium. Magnesium’s element symbol is Mg and was discovered by Joseph Black. It was discovered in England in 1755.
These color changes indicate a chemical change, which show that a reaction had occurred. In the first step when o-vanillin and p-toludine, imine was formed. The color change from green to orange suggests that imine appears as orange colored. In the second step, the addition of sodium borohydride reduced the imine into another derivative, which was yellowish lime color. The solution turned clear when acids and anhydrides was added, which indicated the precipitate were dissolved.
Solution of .04 grams of sodium thiosulfate pentahydrate in 20 mL of water Solution of .9 grams of potassium iodide in 5 mL of water 4 mL starch solution 71 mL of water Combine the solutions in a flask and stir (hand or magnetic stirrer) until turns dark blue Immediately start timing at the moment that the solutions combine together Observation Table (sample data) Experiment 1: Hydrogen Peroxide (mL) Time (seconds) 1
Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
Universal indicator being green shows that the water is neutral 3. Sodium darting on water shows the reaction was vigorous in nature and this was also due to the fact that the hydrogen was propelling the piece in the water 4. The sodium piece becoming spherical shows that the reaction was exothermic. The heat produced melted the sodium piece and made it spherical as the melting point for sodium is low and the heat produced is sufficient to melt it . 5.
During the experiment, a colourless solution of potassium iodide and a solution of sodium persulfate, starch and thiosulfate will be combined into a beaker to later react into a blue-black complex. The elapsed time from when colourless solutions are combined to the colour change is dependent on the reactant concentrations of sodium persulfate and potassium iodide. Experiments will be conducted by systematically varying the concentrations of persulfate and iodine. The times recorded will be utilised to determine the rate of reaction and
Due to the hydroxide ions, both solutions turn pink and become effervescing with hydrogen gas. Below are the equations of the reactions : Mg(s) + 2H2O(aq) → Mg(OH)2(aq) + H2(aq) Ca(s) + 2H2O(aq) → Ca(OH)2(aq) + H2(aq) Calcium is more reactive than Magnesium. Therefore, Ca(OH)2 changes to pink faster than Mg(OH)2 because Calcium is located below Magnesium in the periodic table. Calcium donates electrons faster than Magnesium.
Research Question: How does the concentration of the nitric acid affect the the time for the magnesium to dissolve or react. Hypothesis: If the concentration of the nitric acid is lower, the magnesium strips will dissolve slower and each time the concentration acid is higher the magnesium strip will dissolve faster. The reason for magnesium strips to dissolve faster when the concentration of the nitric acid is higher is because the reaction of this experiment is exothermic and when more energy is given out the faster the magnesium strips will dissolve. Collision theory is when different reactions collide at different rates, a slow reaction have a low rate of reaction and a fast reaction have a high rate of reaction.
P1 Predict the products that form when solution of electrolysed and molten electrolytes are electrolysed Electrolysis Chemical change which is produced by passing an electric current through a conducting solution or molten salt Electrolyte A substance which is able to ionizes ad conduct electricity In order to predict the product of the electrolysis but before we do that we need to know what it is and how does it work. Electrolysis, it is a method to separate bonded elements and compounds by passing an electric current through them. Electrolyte is a substance which contains free ions, which are carriers of electric current in the electrolyte however, if the ions are not transportable as it is in a solid salt, then electrolysis cannot