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I see that you've uploaded an image with questions related to chemistry and possibly stoichiometry. Let me break down each question and provide detailed solutions.

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**Questions visible in the image:**

3. **Calculate the mass lost due to heating.**

4. **Calculate the percentage composition (by mass) of water in your sample.**

5. **Given that the correct percentage of water in Copper (II) Sulfate Pentahydrate is 36.1%, what is your percentage error?**

6. **What would happen to your calculated percentage of water if your sample contained moisture? Justify your answer.**

7. **Copper (II) Sulfate, if heated excessively, will decompose into Sulfur Trioxide and Copper (II) Oxide as per the equation given below:**
   
   \[
   \text{CuSO}_4 \, (s) \rightarrow \text{CuO} \, (s) + \text{SO}_3 \, (g)
   \]

   What would happen to your calculated percentage of water if the above reaction happened to a significant extent? Justify your answer.

8. **A student heated a hydrated salt sample with an initial mass of 4.8702 g. After the first heating, the mass had decreased to 3.0662 g. The student determined that the mass lost by the sample was 1.8053 g. What was the percent water in the original hydrated sample?**

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### Let’s address the 8th question first, as it provides a complete dataset:

**Mass of the hydrated salt sample before heating:**  
Initial mass \( m_{\text{initial}} = 4.8702 \, \text{g} \)

**Mass of the sample after heating:**  
Final mass \( m_{\text{final}} = 3.0662 \, \text{g} \)

**Mass lost due to heating:**  
Mass lost \( = m_{\text{initial}} - m_{\text{final}} = 4.8702 \, \text{g} - 3.0662 \, \text{g} = 1.8053 \, \text{g} \)

To find the percentage of water in the original hydrated sample, we use:

\[
\text{Percent water} = \left( \frac{\text{mass of water lost}}{\text{initial mass of sample}} \right) \times 100
\]

\[
\text{Percent water} = \left( \frac{1.8053 \, \text{g}}{4.8702 \, \text{g}} \right) \times 100 = 37.06 \%
\]

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Now, would you like to proceed with any specific question, or should I continue solving the rest? Let me know!

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**Here are 5 related questions that expand on the content:**

1. How would you calculate the mass of an anhydrous salt after heating?
2. Why does heating cause a loss of mass in hydrated compounds?
3. How is percentage error calculated in chemical analysis?
4. What assumptions are made during the calculation of water percentage in hydrates?
5. What effect does excessive heating have on the composition of hydrates?

**Tip:** Always ensure you remove moisture before weighing any chemical sample to avoid errors due to excess water content.

Calculate the mass lost due to heating and the percentage of water in a sample of hydrated salt. Additionally, address percentage error and implications of excessive heating or moisture in Copper (II) Sulfate Pentahydrate.

Learn how to calculate mass loss due to heating and determine the percentage of water in a hydrated salt sample. This guide covers essential concepts like mass loss calculation, percentage water composition, and the impact of excessive heating or moisture. Ideal for chemistry students in Grades 10-12.

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