Chemical Reactions Research

Chemical reactions have presented important guidelines in the dimension of variables. They continue to act as tools for the enhancement of instrument competencies as well as seek to provide guidelines on how to find options to problems. Moreover, they support different human activities. With the giant usefulness of chemical reactions, it’s important to understand their nature and types. Generally, there are countless types of chemical reaction, including synthesis, decomposition, combustion, single replacement, double replacement, precipitation amongst others. This paper intends to present a lab report for the statement of different chemical reactions and write their respective chemical equations.

Objectives

1. To examine distinctive types of chemical reactions including synthesis, decomposition, combustion, single replacement, double replacement, and precipitation.
2. To identify the products of the performed chemical reactions include the chemical reactions using balanced equations.

Chemicals:

Sodium, Calcium Carbonate, Alluminium, Nickel Sulphate, Magnesium Sulphate, Lithium Hydroxide, Zinc, Copper Sulphate, Butane, water, and Universal indicator

Apparatus:

Sources of heat and lighting, droppers, test tubes, boiling tubes, Universal indicators, wash bottle with distilled water, scapulas, test tube holder, gas container with butane gas, and beakers.

Procedures:

Synthesis reaction:

1. Placed about 100mm of distilled water into a beaker
2. Scooped a small quantity of sodium metal and deeped it into the water in the beaker.
3. Stirred the solution until all the sodium has dissolved.
4. Using a dropper, I placed three drops of universal indicators and observed the change in color.

Decomposition reaction:

1. Placed 10 grams of calcium carbonate in a boiling tube.
2. Using a Bunsen Burner, I heated the solid in the boiling tube until change in mass is complete.

Single replacement reaction

1. Placed a small piece of Alluminium into a test tube
2. Took a solution of Nickel Sulphate and added it into the test tube
3. Allow the reaction to complete by observing deposits at the bottom of the test tube.

Double replacement reaction:

1. Placed dried Mgso4 on a test tube and added aqueous Lithium Sulphate
2. Shook the mixture for the reaction to occur
3. Tested the solution with universal indicator

Precipitation reaction:

1. Placed about 20 mm of aqueous Copper Sulphate into a beaker and added a 10 grams of Zinc metal
2. Stirred the solution until all the zinc had dissolved

Combustion reaction:

1. Allowed butane gas to flow through a metallic pipe and lit the exposed end with a flame in excess air.
2. Observed the color of the flame
3. Place a beaker with water under the burning flame and measure change in temperature

Results:

Data Table 1. Experimental Data and Observations

Discussion and Conclusion:

The synthesis reaction produced aqueous sodium hydroxide and hydrogen gas. The decomposition reaction produced Calcium Oxide and Carbon (IV) Oxide. The single replacement reaction produced Alluminium Sulphate and Nickel while the double replacement reaction produced Magnesium Hydroxide and Lithium Sulphate. The precipitation and combustion reactions produced Zinc Sulphate plus Copper and Carbon (IV) Oxide plus water respectively (See Table 1 for balanced chemical equations).

Each of these products was identified by a change in either mass or color of reactants. In the synthesis reaction, a lot of energy was released. Also, the new product changed to blue/purple upon addition of universal indicator showing the formation of a new product. There was a lot of fizzling indicating a release of a gas. CaCO3 crumbled with continued heating to form a solid with less mass. In the single replacement reaction, alluminium replaced Nickel and nickel was deposited as a silver-white solid while in the double replacement reaction, MgSO4 exchanged ions with LiOH. In the precipitation reaction, Zinc replaced Cu in the CuSO4 solution, which caused the fading of the blue color of the solution. Finally, Butane burn in excess oxygen to give CO2, H2O and energy, which was evident from the increase in water temperature.

In conclusion, this study was intended to examine different types of chemical reactions, including synthesis, decomposition, combustion, single replacement, double replacement, and precipitation and identify the products of the performed chemical reactions include the chemical reactions using balanced equations. After performing laboratory procedures, all the types of chemical reactions were successful and we were able to identify different products of different reactions.

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References

Martin, R. B. (1999). Replace Double Replacement. Journal of Chemical Education, 76(1), 22903. https://doi.org/10.1021/ed076p133

Rice, S. A. (2001, January 18). Interfering for the good of a chemical reaction. Nature. https://doi.org/10.1038/35053211

Siggia, S. (1974). The significant role of chemical reactions in analytical chemistry. Journal of Chemical Education, 51(2), 98. https://doi.org/10.1021/ed051p98

Timberlake, K. C. (2006). General, Organic, and Biological Chemistry: Structures of Life. London, UK: Pearson Education, Limited. Retrieved from https://books.google.co.uk/books/about/General_Organic_and_Biological_Chemistry.html?id=DCdCT4AGW6QC&pgis=1