ipl-logo

Single Displacement Reaction Lab

766 Words4 Pages

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

Show More
Related
444 Words | 2 Pages

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

Read More
1316 Words | 6 Pages

For Station 4 , the magnesium and zinc turnings blackened when introduced to Cu(NO3)2 . Copper (II) nitrate, zinc nitrate and magnesium nitrate all changed colour when sodium carbonate was added. b)Magnesium is most reactive (#1). Zinc is second most reactive (#2). Copper is the least reactive (#3).

Read More
840 Words | 4 Pages

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.

Read More
1073 Words | 5 Pages

As the compound was reacting, the aluminum pieces were also dissolving, with only a few pieces left inside. The process of the second reaction included the adding of a new substance which consisted of sulfuric acid. The sulfuric acid along with potassium aluminum hydroxide, was yielded to produce aluminum hydroxide, potassium sulfate, and water. This reaction was both a precipitation reaction and an acid-base reaction. Once the sulfuric acid was added, the reaction became very chunky.

Read More
930 Words | 4 Pages

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

Read More
1047 Words | 5 Pages

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.

Read More
471 Words | 2 Pages

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

Read More
356 Words | 2 Pages

The purpose of this lab was to determine the chemical properties of different metals by observing the color of the flame when it was burned. The dependent variable was the color of the flame and the independent variable was the metal. Thus, the controls were the chlorine (Cl), bunsen burner, deionized water, and cotton swabs used to dip into samples of the metals. Because the bunsen burner was used, goggles were worn and loose clothing or hair was tied back prior to beginning the lab. The first step was to obtain deionized water and 7 q-tips for the 7 metals being examined (Ca, Ba, Cu, Sr, K, Li, Na, and Mg).

Read More
729 Words | 3 Pages

The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.

Read More
377 Words | 2 Pages

George i Whitlatch describes the value of manganese classified into chemical and metallurgical

Read More
792 Words | 4 Pages

How has the extraction of metals changed the course of history? Metal: Magnesium Magnesium is a metal that is both industrially and biologically important. It is the lightest structural metal that is currently available for us.

Read More
578 Words | 3 Pages

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.

Read More
800 Words | 4 Pages

The zinc will form a new compound with the sulfate, and the copper will stay as a metal. Balanced Chemical

Read More
1161 Words | 5 Pages

Empirical Formula of Magnesium Oxide - Lab Report Background Information/Introduction: The aim of this lab is to determine the empirical formula of magnesium oxide by converting magnesium to magnesium oxide. As an alkali earth metal, magnesium reacts violently when heated with oxygen to produce magnesium oxide and magnesium nitride as a byproduct. In order to obtain only magnesium oxide, distilled water was added so that magnesium nitride will react and convert to magnesium hydroxide. Further heating then oxidizes all of the magnesium into magnesium oxide.

Read More
789 Words | 4 Pages

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.

Read More

More about Single Displacement Reaction Lab

Related Topics

Open Document