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Worksheet about revision for exp of determining the empirical formula of copper oxide | ||
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| Subject: Chemistry | ||
| 10th Grade | ||
| Term 1 | ||
| Year: 2023/2024 | ||
| Size: 595.5KB | ||
| Number of clicks: 58 | ||
| Publish date:November 05, 2023 | ||
| Added by: Eman | ||
| Last download date: 2024-09-03 06:23:29 | ||
| Updated by: Eman9966 on 2023-11-05 13:42:35 | By: theodor chingshuen | |
| File info: The experiment for determining the empirical formula of copper oxide typically involves the reaction of copper metal with oxygen gas to form copper oxide. Students are then tasked with determining the empirical formula of the copper oxide compound based on the mass of copper and oxygen involved in the reaction. Here's a step-by-step revision guide for this experiment:1. Review the concept of empirical formula: Ensure that you understand the definition of empirical formula, which represents the simplest whole number ratio of elements in a compound. 2. Understand the reaction: Familiarize yourself with the balanced chemical equation for the reaction between copper and oxygen to form copper oxide. The equation is typically written as: 2Cu + O2 -> 2CuO. 3. Recall the law of conservation of mass: Remember that in a chemical reaction, mass is conserved. The total mass of reactants is equal to the total mass of products. 4. Determine the mass of copper: Review the experimental procedure for obtaining a known mass of copper metal. This can be done by weighing a clean and dry crucible, adding the copper, and re-weighing the crucible with the copper. 5. Perform the reaction: Follow the experimental procedure to heat the copper metal in the crucible using a Bunsen burner or a heating source. The copper will react with oxygen from the air to form copper oxide. 6. Observe the color change: As the copper reacts with oxygen, it undergoes a chemical change and changes color. Note the color change from the initial metallic copper to the black or reddish-brown color of copper oxide. 7. Determine the mass of copper oxide: Allow the crucible to cool, and then weigh it again, including the copper oxide formed. Calculate the mass of the copper oxide by subtracting the mass of the empty crucible. 8. Calculate the mass of oxygen: Subtract the mass of copper from the total mass of copper oxide to find the mass of oxygen that combined with the copper. 9. Calculate the mole ratio: Convert the mass of copper and oxygen to moles using their molar masses (atomic masses). Divide the number of moles of each element by the smaller value to obtain a simple whole number ratio. 10. Write the empirical formula: Write the empirical formula of copper oxide based on the mole ratio obtained. For example, if the ratio is 1:1, the empirical formula would be CuO. 11. Double-check the calculations: Review your calculations and ensure that you have followed the steps accurately. Check for any errors or inconsistencies. 12. Practice additional problems: To reinforce your understanding, practice additional problems involving the determination of empirical formulas using different reactants and compounds. By following this revision guide, you can refresh your understanding of the experiment for determining the empirical formula of copper oxide. Remember to emphasize the importance of accuracy in measurements and calculations for obtaining reliable results. | ||
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