reaction, g mass of Zn reacted, g filter mass of wax paper, g 0.298 mass of wax paper + Glass dish : 50.572 Moles of Cu: Cu, g after 5 min. on 51.686Büchner funnel, g 51.684 51.674 after additional 5 min. on bench, g after another 5 min. on bench, g mass of Cu produced, g mass of Cl in copper chloride, g moles of Cu in copper chloride, mol moles of Cl in copper chloride, mol empirical formula of copper chloride 0.816 0.814 0.804 0.804g 1.217 g 0.0127 Mass of Cl: 0.804+ (mass of (1) = 2.021g 2.021 0.804 = 1.217g 0.0343 CUC13 0.804 x 63.546 = 0.0127 mol Cv class paper Moles of Cl: 1.2179 * 35.453 = 0.0343 mol c -39- Empirical Formula: 0.0127 0.0127 0.0343 mol Cu 0.0127 mol = 1 (v: 2.7 CI =1Cu: 3C1 -CuC13
reaction, g mass of Zn reacted, g filter mass of wax paper, g 0.298 mass of wax paper + Glass dish : 50.572 Moles of Cu: Cu, g after 5 min. on 51.686Büchner funnel, g 51.684 51.674 after additional 5 min. on bench, g after another 5 min. on bench, g mass of Cu produced, g mass of Cl in copper chloride, g moles of Cu in copper chloride, mol moles of Cl in copper chloride, mol empirical formula of copper chloride 0.816 0.814 0.804 0.804g 1.217 g 0.0127 Mass of Cl: 0.804+ (mass of (1) = 2.021g 2.021 0.804 = 1.217g 0.0343 CUC13 0.804 x 63.546 = 0.0127 mol Cv class paper Moles of Cl: 1.2179 * 35.453 = 0.0343 mol c -39- Empirical Formula: 0.0127 0.0127 0.0343 mol Cu 0.0127 mol = 1 (v: 2.7 CI =1Cu: 3C1 -CuC13
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help with number 1 of the Post Laboratory Questions.
![# Laboratory Experiment Data and Calculations: Copper Chloride Reaction
## Data Collection
### Measurements
- **Mass of Copper Chloride in 25.0 mL of Solution:** 2.021 g
- **Initial Mass of Zinc (Zn):** 1.636 g
- **Mass of Zinc after Reaction:** 0.685 g
- **Mass of Zinc Reacted:**
- **Mass of Filter Wax Paper:** 0.298 g
- **Mass of Wax Paper + Copper (Cu), glass dish:** 50.157 g, 50.872 g
- **Mass after 5 Minutes on Büchner Funnel:** 0.816 g
- **After Additional 5 Minutes on Bench:** 0.814 g
- **After Another 5 Minutes on Bench:** 0.804 g
- **Mass of Copper Produced:** 0.804 g
- **Mass of Chlorine (Cl) in Copper Chloride:** 1.217 g
### Calculations
#### Mass of Copper (Cu)
- Calculation:
\[
0.814 \, \text{g} - 0.804 \, \text{g} = 0.01 \, \text{g} \approx 0.05 \, \text{g}
\]
#### Mass of Chlorine (Cl)
- Calculation:
\[
0.804 \, \text{g} + (\text{mass of Cl}) = 2.021 \, \text{g}
\]
\[
2.021 \, \text{g} - 0.804 \, \text{g} = 1.217 \, \text{g}
\]
#### Moles of Copper (Cu)
- Calculation:
\[
\frac{0.804 \, \text{g}}{63.546} = 0.0127 \, \text{mol Cu}
\]
#### Moles of Chlorine (Cl)
- Calculation:
\[
\frac{1.217 \, \text{g}}{35.453} = 0.0343 \, \text{mol Cl}
\]
### Empirical Formula Calculation
- Moles Ratio:
\[
\frac{0.0127}{0.0127}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1b897147-dac4-49d3-a0b7-87acbe9c344d%2F4470ef17-d0d4-473e-9c89-844f0ab956b9%2Fhcnvdbl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Laboratory Experiment Data and Calculations: Copper Chloride Reaction
## Data Collection
### Measurements
- **Mass of Copper Chloride in 25.0 mL of Solution:** 2.021 g
- **Initial Mass of Zinc (Zn):** 1.636 g
- **Mass of Zinc after Reaction:** 0.685 g
- **Mass of Zinc Reacted:**
- **Mass of Filter Wax Paper:** 0.298 g
- **Mass of Wax Paper + Copper (Cu), glass dish:** 50.157 g, 50.872 g
- **Mass after 5 Minutes on Büchner Funnel:** 0.816 g
- **After Additional 5 Minutes on Bench:** 0.814 g
- **After Another 5 Minutes on Bench:** 0.804 g
- **Mass of Copper Produced:** 0.804 g
- **Mass of Chlorine (Cl) in Copper Chloride:** 1.217 g
### Calculations
#### Mass of Copper (Cu)
- Calculation:
\[
0.814 \, \text{g} - 0.804 \, \text{g} = 0.01 \, \text{g} \approx 0.05 \, \text{g}
\]
#### Mass of Chlorine (Cl)
- Calculation:
\[
0.804 \, \text{g} + (\text{mass of Cl}) = 2.021 \, \text{g}
\]
\[
2.021 \, \text{g} - 0.804 \, \text{g} = 1.217 \, \text{g}
\]
#### Moles of Copper (Cu)
- Calculation:
\[
\frac{0.804 \, \text{g}}{63.546} = 0.0127 \, \text{mol Cu}
\]
#### Moles of Chlorine (Cl)
- Calculation:
\[
\frac{1.217 \, \text{g}}{35.453} = 0.0343 \, \text{mol Cl}
\]
### Empirical Formula Calculation
- Moles Ratio:
\[
\frac{0.0127}{0.0127}
Transcribed Image Text:**Post Laboratory Questions**
1. Based on your data and observation:
a. Which of the reactants in your experiment was the limiting reagent? Briefly explain.
b. Which of the reactants in your experiment was present in excess? Briefly explain.
2. You have reacted copper chloride solution with Zn metal to precipitate out all the Cu in its elemental form.
a. Based on the empirical formula you determined for copper chloride, present the balanced chemical equation for this experiment.
b. Based on the mass of Zn reacted and your equation in 2a, how much Cu do you expect to produce (the theoretical yield)?
Mass of Zn reacted = _______ g
Theoretical yield of Cu = ___________ g
c. Determine the percent yield of Cu from your determination.
*Note: There are no graphs or diagrams included in the image.*
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