High School

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1. Obtain a sheet of weighing paper and place it on the balance. Press the TARE button.
2. Add approximately 5.6 g of copper chloride to the weighing paper on the balance.
3. Record the mass of copper chloride (include all digits from the scale).
4. Transfer the solid copper chloride to a 250 mL beaker.
5. Add about 60 mL of distilled water (dH₂O) to the beaker containing the copper chloride solution using a graduated cylinder.
6. Cut about 40–50 cm of aluminum wire, make a flat coil, and place it in the copper chloride solution.
7. Watch the reaction. Wait for the solution to turn clear and stop bubbling, indicating the reaction is complete. This may take 20-30 minutes. Periodically shake off solid copper from the aluminum wire.
8. While the reaction is occurring, set up the Buchner funnel and the Erlenmeyer flask to filter and collect the solid copper.
9. Weigh a clean piece of filter paper.
10. Using the Buchner Funnel Apparatus, collect all copper from the beaker.
11. Dry the copper under a heat lamp, rinse with acetone, and let it dry.
12. Weigh the copper on the filter paper.
13. Subtract the weight of the filter paper to get the weight of the copper.
14. Determine the mass of chlorine by subtracting the mass of copper from the mass of copper chloride.
15. Determine moles of copper from grams of Cu (#13): mole Cu = x. Show your work! (5 pts)
16. Determine moles of chlorine from grams of Cl (#14): mole Cl = y. Show your work! (5 pts)
17. Determine the empirical formula of copper chloride (Cu_x Cl_y). Show your work! (5 pts) / Accuracy of empirical formula (10 pts). Cu_x Cl_y: Put in x and y from steps #15 and #16, then divide by the smallest value to get whole numbers for the empirical formula.
18. Calculate %Cu based on data: = [mass copper chloride (#3) / mass copper (#13)] × 100%. Show your work! (5 pts)
19. Calculate the actual %Cu based on the formula CuCl₂ = Actual %Cu. %Cu = [mass CuCl₂ / mass copper] × 100%. Show your work! (5 pts)
20. Speculate on WHY the experimentally determined %Cu (#18) is different than the actual %Cu (#19).

Answer :

Final answer:

The student is carrying out an experiment to determine the empirical formula of copper chloride by weighing the compound before and after a reaction, calculating the amount of copper and chlorine in moles, and comparing the experimentally determined percent copper to the theoretical value.

Explanation:

This question about an experiment involves determining the empirical formula of copper chloride. You are weighing the copper chloride before and after the reaction with aluminum, filtering and drying the copper product, and then weighing it again. The difference in mass will give you the amount of chlorine in the compound.

To convert the grams of copper and chlorine to moles, you would use the molar mass of each element (approximately 63.55 g/mol for Cu and 35.45 g/mol for Cl). Once you have the number of moles for each element, divide each by the smaller value to get whole numbers for the empirical formula.

The percent of copper based on data (%Cu) is given by the formula [ mass copper chloride (#3) / mass copper (#13) ] × 100%. The actual %Cu is a theoretical value determined from the formula [ Mass CuCl2 / mass copper ] × 100%. Any deviation of the determined %Cu from this value could be due to experimental errors like unreacted copper, impurities, or incomplete transfer of materials among other factors.

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Final answer:

The experimentally determined %Cu is different from the actual %Cu because of potential errors in the experimental procedure, such as incomplete reactions, losses during transfers, and impurities in reagents.

Explanation:

The experiment involves the determination of the empirical formula and the percentage of copper in a copper chloride compound. Here's the step-by-step explanation:

1. We start by zeroing the balance using weighing paper (TARE button).

2. Approximately 5.6 g of copper chloride is added to the weighing paper, and its mass is recorded.

3. The copper chloride is transferred to a beaker, and about 60 mL of water (dH2O) is added.

4. A coil of aluminum wire is placed in the copper chloride solution, initiating a reaction that produces copper.

5. The reaction is allowed to complete, indicated by the solution turning clear and no longer bubbling.

6. While the reaction is ongoing, the Buchner funnel apparatus is set up for filtration.

7. A clean piece of filter paper is weighed.

8. The solid copper is collected using the Buchner funnel and is dried, rinsed with acetone, and dried again.

9. The copper on the filter paper is weighed, and the weight of the filter paper is subtracted to determine the mass of copper.

10. The mass of chlorine is determined by subtracting the mass of copper from the mass of copper chloride.

11. The moles of copper and chlorine are calculated using their respective masses and molar masses.

12. The empirical formula of copper chloride (Cu x Cl y) is determined by dividing the moles of each element by the smallest mole value.

13. The experimentally determined %Cu (actual %Cu) is calculated based on the mass of copper chloride and copper.

14. Discrepancies between the experimentally determined %Cu and actual %Cu can arise due to errors, incomplete reactions, or impurities in reagents.

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