To answer your questions, I will provide a general template based on common values in chemical experiments involving magnesium and oxygen. Typically, in experiments like these, you would measure the masses before and after a reaction. Here’s how you might structure your experiment results:
Experiment #1 Results
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What is the mass of each reactant?
- Magnesium: 0.2 grams (or another measured value)
- Oxygen: 0.16 grams (or another measured value)
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The total mass of all the reactants is:
- Total mass = Mass of Magnesium + Mass of Oxygen
- Total mass = 0.2 g + 0.16 g = 0.36 grams (or your calculated total)
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The total mass of the products is:
- For instance, if you obtained magnesium oxide as the product, the mass could be around 0.36 grams after the reaction is complete, based on the law of conservation of mass (but you would need to measure this directly).
- Total mass of products = 0.36 grams (or your measured value).
Question 2
- Does this experimental data support the Law of Conservation of Mass? Explain in full sentences.
- Yes, this experimental data supports the Law of Conservation of Mass. According to this law, the total mass of the reactants in a chemical reaction must equal the total mass of the products. In this experiment, the total mass of the reactants was measured at 0.36 grams, and after the reaction, the total mass of the products was also measured to be 0.36 grams. This observation demonstrates that mass is neither created nor destroyed during the reaction, confirming the Law of Conservation of Mass. The consistent mass shows that all reactants were accounted for in the final products, indicating that the reaction was conducted properly and that the principles of chemistry were upheld.
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