('us 0415H₂0 Moles of anhydride used. (Show calculations) = • CuSoy 5H20(s) A (u504(5) + 5#20(g) Hydrate → anhydride Moles of H₂O of hydration (Show calculations)=
('us 0415H₂0 Moles of anhydride used. (Show calculations) = • CuSoy 5H20(s) A (u504(5) + 5#20(g) Hydrate → anhydride Moles of H₂O of hydration (Show calculations)=
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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![**Educational Text Transcription:**
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**Moles of Anhydride Used (Show Calculations):**
\[ \text{CuSO}_4 \cdot 5\text{H}_2\text{O} \xrightarrow{\Delta} \text{CuSO}_4(\text{s}) + 5\text{H}_2\text{O}(\text{g}) \]
\[ \text{1 mole of CuSO}_4 \cdot 5\text{H}_2\text{O} \]
\[ \text{1.5 g CuSO}_4 \cdot 5\text{H}_2\text{O} \times \frac{1 \text{ mole}}{\text{Molar mass}} = \]
---
**Moles of H\(_2\)O of Hydration (Show Calculations):**
\[ \_\_\_\_\_\_\_\_ \]
---
**Ratio of Moles of Water to Moles of Anhydride = \_\_\_\_\_\_\_\_\_\_ \]
(To correct sig. figs. — do not round yet)
---
**Question:**
Based on your data, what is the empirical formula of your hydrate (round your ratio to the closest whole number)? Use the Argumentation Framework (see inside front cover) (Claim - Evidence - Justification) to justify your answer.
---
**Explanation:**
This document appears to be a worksheet or assignment for calculating the empirical formula of a hydrate. It involves converting mass measurements to moles, determining the moles of anhydrous copper(II) sulfate and water, and calculating their ratio. The task includes problem-solving steps, such as applying the concept of molar mass and using proper significant figures. The final goal is to determine the empirical formula of the hydrate using stoichiometry and provide a structured justification using the Argumentation Framework.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ec8f5aa-2346-419c-86c9-3c70e4e8e13c%2Fd9d087c9-23d0-4a96-a1ee-e2cbfedc5306%2Fq0nf8iu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Text Transcription:**
---
**Moles of Anhydride Used (Show Calculations):**
\[ \text{CuSO}_4 \cdot 5\text{H}_2\text{O} \xrightarrow{\Delta} \text{CuSO}_4(\text{s}) + 5\text{H}_2\text{O}(\text{g}) \]
\[ \text{1 mole of CuSO}_4 \cdot 5\text{H}_2\text{O} \]
\[ \text{1.5 g CuSO}_4 \cdot 5\text{H}_2\text{O} \times \frac{1 \text{ mole}}{\text{Molar mass}} = \]
---
**Moles of H\(_2\)O of Hydration (Show Calculations):**
\[ \_\_\_\_\_\_\_\_ \]
---
**Ratio of Moles of Water to Moles of Anhydride = \_\_\_\_\_\_\_\_\_\_ \]
(To correct sig. figs. — do not round yet)
---
**Question:**
Based on your data, what is the empirical formula of your hydrate (round your ratio to the closest whole number)? Use the Argumentation Framework (see inside front cover) (Claim - Evidence - Justification) to justify your answer.
---
**Explanation:**
This document appears to be a worksheet or assignment for calculating the empirical formula of a hydrate. It involves converting mass measurements to moles, determining the moles of anhydrous copper(II) sulfate and water, and calculating their ratio. The task includes problem-solving steps, such as applying the concept of molar mass and using proper significant figures. The final goal is to determine the empirical formula of the hydrate using stoichiometry and provide a structured justification using the Argumentation Framework.
![# Determination of the Formula of Anhydride
### Procedure
1. Conduct the heating using about 1.5 g of hydrate.
### Observations
#### Table 2.1
| Measurement | Trial 1 | Trial 2 |
|-------------------------------------------------|-----------|----------|
| Mass of crucible (g) | 16.5818 | 16.4692 |
| Mass of crucible + hydrate (g) | 18.5315 | 17.9622 |
| Mass of crucible + anhydride (after 1st heating) (g) | 17.9376 | 17.3982 |
| Mass of crucible + anhydride (after 2nd heating) (g) | 17.9158 | 17.3633 |
| Mass of crucible + anhydride (after 3rd heating) (g) | 17.9026 | 17.3465 |
### Data Summary
#### Table 2.2
| Measurement | Trial 1 | Trial 2 |
|---------------------------------|----------|----------|
| Mass of hydrate (g) | 1.9498 | 1.4930 |
| Mass of anhydride (g) | 0.9209 | 0.8793 |
| Mass of water lost on heating (g)| 1.0289 | 0.6137 |
### Calculation
- Molar mass of the anhydride (use 4 significant figures):
\[ \text{Formula: } \text{CuSO}_4 \cdot 5\text{H}_2\text{O} \]
*Note: The data summarizes the mass changes before and after heating to determine the mass of water lost and the anhydride formed. Ensure proper use of significant figures in calculations.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ec8f5aa-2346-419c-86c9-3c70e4e8e13c%2Fd9d087c9-23d0-4a96-a1ee-e2cbfedc5306%2F8vdwy4d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Determination of the Formula of Anhydride
### Procedure
1. Conduct the heating using about 1.5 g of hydrate.
### Observations
#### Table 2.1
| Measurement | Trial 1 | Trial 2 |
|-------------------------------------------------|-----------|----------|
| Mass of crucible (g) | 16.5818 | 16.4692 |
| Mass of crucible + hydrate (g) | 18.5315 | 17.9622 |
| Mass of crucible + anhydride (after 1st heating) (g) | 17.9376 | 17.3982 |
| Mass of crucible + anhydride (after 2nd heating) (g) | 17.9158 | 17.3633 |
| Mass of crucible + anhydride (after 3rd heating) (g) | 17.9026 | 17.3465 |
### Data Summary
#### Table 2.2
| Measurement | Trial 1 | Trial 2 |
|---------------------------------|----------|----------|
| Mass of hydrate (g) | 1.9498 | 1.4930 |
| Mass of anhydride (g) | 0.9209 | 0.8793 |
| Mass of water lost on heating (g)| 1.0289 | 0.6137 |
### Calculation
- Molar mass of the anhydride (use 4 significant figures):
\[ \text{Formula: } \text{CuSO}_4 \cdot 5\text{H}_2\text{O} \]
*Note: The data summarizes the mass changes before and after heating to determine the mass of water lost and the anhydride formed. Ensure proper use of significant figures in calculations.*
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