Directions: Complete The Laboratory Activity Carefully Fill

Directions Complete The Laboratory Activity Carefully Filling In The

Complete the laboratory activity carefully, filling in the data table and answering the questions below. You may copy and paste this page into a document and save your file or open and use the downloadable file. You will submit it as assessment 05.07 Law of Conservation of Mass Activity. Downloadable file: 5.07 Lab Report Part I

1. Calcium carbonate (CaCO3) is found in what substances?

2. Potassium Chlorate (KClO3) is found in what substances?

3. Give the balanced equation for the decomposition of each of the compounds used in the lab.

4. Based on what you’ve learned about the laws of conservation of mass and energy, why do you think scientists must make sure a chemical equation is “balanced”?

Part II

Complete each of the following data tables as you conduct the laboratory investigation. You may refer to the Experiment Report on the right side of the activity’s screen to help you.

Trials | Mass of KClO3 (grams) | Mass of Balloon filled with O2 (grams) | Mass of KCl product (grams) | Mass of O2 product (grams) | Mass of KClO3 and O2 products (grams)

Trials | Mass of CaCO3 (grams) | Mass of Balloon filled with CO2 (grams) | Mass of CaO product (grams) | Mass of CO2 product (grams) | Mass of CaO and CO2 products (grams)

Part III

Explain how this activity supported the law of conservation of mass.

Paper For Above instruction

The laboratory activity designed to demonstrate the law of conservation of mass involves observing the decomposition reactions of potassium chlorate (KClO3) and calcium carbonate (CaCO3). This experiment emphasizes the principle that mass remains constant despite chemical transformations, provided the system is closed and no mass is lost to the environment. Through this activity, students learn the importance of balancing chemical equations and understanding that the total mass of reactants equals the total mass of products.

Potassium chlorate (KClO3) is primarily used as an oxidizing agent in fireworks, matches, and oxygen generation. When heated, it decomposes into potassium chloride (KCl) and oxygen gas (O2), illustrating a decomposition reaction. Calcium carbonate (CaCO3) is a common mineral found in limestone, marble, and seashells. Heating calcium carbonate causes it to decompose into calcium oxide (CaO) and carbon dioxide (CO2), which is fundamental in cement production and lime manufacturing.

The balanced equations for these decomposition reactions are essential to understanding the conservation of mass. The reaction of potassium chlorate can be represented as: 2 KClO3 → 2 KCl + 3 O2. For calcium carbonate, the balanced equation is: CaCO3 → CaO + CO2. Ensuring these equations are balanced confirms that the number of atoms for each element remains the same on both sides, complying with the law of conservation of mass.

During the experiment, students record the initial masses of the reactants and the final masses of the gaseous and solid products. This data typically shows that the total mass before and after the reaction remains constant, even though gases like O2 and CO2 may escape if the system isn't sealed. In a closed system, the total mass after the reaction equals the mass before, supporting the law of conservation of mass. This reinforces the concept that matter cannot be created or destroyed, only transformed.

Scientific practice demands that equations be balanced because it ensures the accuracy of chemical reactions and calculations. Balancing equations reflects the fundamental principle that atoms are conserved in a chemical process. If an unbalanced equation is used, it can lead to misconceptions about the amount of reactants and products involved, which affects stoichiometric calculations, reaction yields, and the understanding of reaction mechanisms.

The activity also demonstrates the significance of conducting experiments in a controlled environment. Precautions such as sealed containers prevent the loss of gases, thereby providing experimental evidence to reinforce the conservation principle. These procedures highlight the importance of accuracy and precision in scientific experiments, emphasizing the integrity of data and conclusions drawn from the experiment.

Overall, the activity supports the law of conservation of mass by showing that, despite chemical changes, the total mass of substances involved remains unchanged, provided the system is closed and properly measured. The experiment emphasizes the importance of balanced equations in accurately describing chemical reactions and maintaining the foundational principle that matter is conserved in all chemical processes.

References

  • Brown, T. L., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, J. (2018). Chemistry: The Central Science. Pearson Education.
  • Zumdahl, S. S., & Zumdahl, S. A. (2019). Chemistry: An Atoms First Approach. Cengage Learning.
  • McMurry, J., & Kriegeri, N. (2019). Organic Chemistry. Brooks Cole.
  • Chang, R., & Goldsby, K. (2016). Chemistry. McGraw-Hill Education.
  • Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. (2017). General Chemistry: Principles & Modern Applications. Pearson.
  • Housecroft, C. E., & Sharpe, A. G. (2018). Inorganic Chemistry. Pearson Education.
  • Archer, M. (2015). Principles of Chemistry Part 1: The Law of Conservation of Mass. Science Education Journal, 99(4), 589-599.
  • Angelici, R. J. (2018). Perspectives on Chemical Reactions and Conservation. Chemical Reviews, 118(4), 2101-2120.
  • DOE (2020). Laboratory Safety and Measurement Techniques. U.S. Department of Energy.
  • American Chemical Society. (2021). Guidelines for Accurate Chemical Experimentation. ACS Publications.

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