The image displays a section of a worksheet used for calculating various aspects of a hydrate sample in chemistry. It includes sections for showing work in the calculations. Below is a transcription suitable for an educational website: --- ### Calculate Mass of Hydrate in Your Sample 1. **Moles Water Lost, mol** - **Show Work:** [Space for calculations] 2. **Moles of Hydrate in Sample, mol (Eq. 1.3)** - **Show Work:** [Space for calculations] 3. **Mass of Hydrate in Sample, g** - **Show Work:** [Space for calculations] --- This worksheet assists students in performing step-by-step calculations to determine the composition and characteristics of a hydrate sample. Each section provides ample space for detailed calculations, encouraging students to understand the process fully. ### Laboratory Experiment: Determination of Hydrate Mass **Unknown Sample Number: A** **Chemicals in Unknown Mixture:** CuSO₄·5H₂O and SiO₂ **Hydrate Formula:** CuSO₄·5H₂O **Molar Mass of a Hydrate:** 249.55 g/mol #### Experimental Data 1. **Mass of Crucible (After Pre-heating):** - **Measured Mass:** 11.393 g 2. **Mass of Crucible and Unheated Sample:** - **Measured Mass:** 12.845 g - **Note:** The sample is described as *bright blue*. - **Mass of Unheated Sample Calculation:** \[ 12.845\, \text{g} - 11.393\, \text{g} = 1.452\, \text{g} \] 3. **Mass of Crucible and Sample After 1st Heating:** - **Measured Mass:** 12.497 g 4. **Mass of Crucible and Sample After 2nd Heating:** - **Measured Mass:** 12.494 g - **Difference Between 1st and 2nd Heating:** \[ 0.003\, \text{g} \] 5. **Mass of Water Lost (difference from beginning):** - **Calculation:** \[ 12.494\, \text{g} - 11.393\, \text{g} = 1.101\, \text{g} \] \[ 1.452\, \text{g} - 1.101\, \text{g} = 0.351\, \text{g} \] - **Water Loss as Gas:** \[ 0.351\, \text{g} \] --- **Conclusion:** Using these observations, you can calculate the mass of hydrate in your sample via two different methods. The precision in the repeated measurements indicates evaporative consistency, suggesting accurate determination of water loss.

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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The image displays a section of a worksheet used for calculating various aspects of a hydrate sample in chemistry. It includes sections for showing work in the calculations. Below is a transcription suitable for an educational website:

---

### Calculate Mass of Hydrate in Your Sample

1. **Moles Water Lost, mol**
   - **Show Work:** [Space for calculations]

2. **Moles of Hydrate in Sample, mol (Eq. 1.3)**
   - **Show Work:** [Space for calculations]

3. **Mass of Hydrate in Sample, g**
   - **Show Work:** [Space for calculations] 

---

This worksheet assists students in performing step-by-step calculations to determine the composition and characteristics of a hydrate sample. Each section provides ample space for detailed calculations, encouraging students to understand the process fully.
Transcribed Image Text:The image displays a section of a worksheet used for calculating various aspects of a hydrate sample in chemistry. It includes sections for showing work in the calculations. Below is a transcription suitable for an educational website: --- ### Calculate Mass of Hydrate in Your Sample 1. **Moles Water Lost, mol** - **Show Work:** [Space for calculations] 2. **Moles of Hydrate in Sample, mol (Eq. 1.3)** - **Show Work:** [Space for calculations] 3. **Mass of Hydrate in Sample, g** - **Show Work:** [Space for calculations] --- This worksheet assists students in performing step-by-step calculations to determine the composition and characteristics of a hydrate sample. Each section provides ample space for detailed calculations, encouraging students to understand the process fully.
### Laboratory Experiment: Determination of Hydrate Mass

**Unknown Sample Number: A**

**Chemicals in Unknown Mixture:**  
CuSO₄·5H₂O and SiO₂

**Hydrate Formula:** CuSO₄·5H₂O

**Molar Mass of a Hydrate:** 249.55 g/mol

#### Experimental Data

1. **Mass of Crucible (After Pre-heating):**
   - **Measured Mass:** 11.393 g

2. **Mass of Crucible and Unheated Sample:**
   - **Measured Mass:** 12.845 g
   - **Note:** The sample is described as *bright blue*.
   - **Mass of Unheated Sample Calculation:**  
     \[
     12.845\, \text{g} - 11.393\, \text{g} = 1.452\, \text{g}
     \]

3. **Mass of Crucible and Sample After 1st Heating:**
   - **Measured Mass:** 12.497 g

4. **Mass of Crucible and Sample After 2nd Heating:**
   - **Measured Mass:** 12.494 g
   - **Difference Between 1st and 2nd Heating:**  
     \[ 
     0.003\, \text{g}
     \]

5. **Mass of Water Lost (difference from beginning):**
   - **Calculation:**  
     \[
     12.494\, \text{g} - 11.393\, \text{g} = 1.101\, \text{g}
     \]
     \[
     1.452\, \text{g} - 1.101\, \text{g} = 0.351\, \text{g}
     \]
   - **Water Loss as Gas:**  
     \[
     0.351\, \text{g}
     \]

---

**Conclusion:**  
Using these observations, you can calculate the mass of hydrate in your sample via two different methods. The precision in the repeated measurements indicates evaporative consistency, suggesting accurate determination of water loss.
Transcribed Image Text:### Laboratory Experiment: Determination of Hydrate Mass **Unknown Sample Number: A** **Chemicals in Unknown Mixture:** CuSO₄·5H₂O and SiO₂ **Hydrate Formula:** CuSO₄·5H₂O **Molar Mass of a Hydrate:** 249.55 g/mol #### Experimental Data 1. **Mass of Crucible (After Pre-heating):** - **Measured Mass:** 11.393 g 2. **Mass of Crucible and Unheated Sample:** - **Measured Mass:** 12.845 g - **Note:** The sample is described as *bright blue*. - **Mass of Unheated Sample Calculation:** \[ 12.845\, \text{g} - 11.393\, \text{g} = 1.452\, \text{g} \] 3. **Mass of Crucible and Sample After 1st Heating:** - **Measured Mass:** 12.497 g 4. **Mass of Crucible and Sample After 2nd Heating:** - **Measured Mass:** 12.494 g - **Difference Between 1st and 2nd Heating:** \[ 0.003\, \text{g} \] 5. **Mass of Water Lost (difference from beginning):** - **Calculation:** \[ 12.494\, \text{g} - 11.393\, \text{g} = 1.101\, \text{g} \] \[ 1.452\, \text{g} - 1.101\, \text{g} = 0.351\, \text{g} \] - **Water Loss as Gas:** \[ 0.351\, \text{g} \] --- **Conclusion:** Using these observations, you can calculate the mass of hydrate in your sample via two different methods. The precision in the repeated measurements indicates evaporative consistency, suggesting accurate determination of water loss.
Expert Solution
Step 1

(a) To calculate the moles of water lost,

As per the given information,

Mass of water lost is 0.351 g

To calculate the number of moles of water:

Number of moles=Mass lostMolar mass of water=0.351 g18.01 g/mol=0.0194 mol

The number of moles of water lost =0.0194 mol

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