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tentukan nilai besaran x pada kristal besi (II) sulfat hidrat

Let's work through the problem step by step to determine the value of \( x \) in the hydrated iron (II) sulfate crystal, \( \text{FeSO}_4 \cdot x \text{H}_2\text{O} \).

### Given Data:
- Mass of hydrated iron (II) sulfate crystal, \( \text{FeSO}_4 \cdot x \text{H}_2\text{O} \): 44.8 g
- Mass of anhydrous iron (II) sulfate, \( \text{FeSO}_4 \): 30.4 g
- Molar mass (Mr) of \( \text{FeSO}_4 \): 152 g/mol
- Molar mass (Mr) of \( \text{H}_2\text{O} \): 18 g/mol

### Approach:

1. **Determine the mass of water lost during heating:**
   \[
   \text{Mass of water} = \text{Mass of hydrated crystal} - \text{Mass of anhydrous } \text{FeSO}_4
   \]
   \[
   \text{Mass of water} = 44.8 \, \text{g} - 30.4 \, \text{g} = 14.4 \, \text{g}
   \]

2. **Calculate the moles of anhydrous \( \text{FeSO}_4 \):**
   \[
   \text{Moles of } \text{FeSO}_4 = \frac{\text{Mass of } \text{FeSO}_4}{\text{Molar mass of } \text{FeSO}_4}
   \]
   \[
   \text{Moles of } \text{FeSO}_4 = \frac{30.4 \, \text{g}}{152 \, \text{g/mol}} = 0.2 \, \text{mol}
   \]

3. **Calculate the moles of water lost:**
   \[
   \text{Moles of } \text{H}_2\text{O} = \frac{\text{Mass of water}}{\text{Molar mass of } \text{H}_2\text{O}}
   \]
   \[
   \text{Moles of } \text{H}_2\text{O} = \frac{14.4 \, \text{g}}{18 \, \text{g/mol}} = 0.8 \, \text{mol}
   \]

4. **Determine the value of \( x \):**
   Since \( x \) represents the number of moles of water per mole of \( \text{FeSO}_4 \), we calculate:
   \[
   x = \frac{\text{Moles of } \text{H}_2\text{O}}{\text{Moles of } \text{FeSO}_4}
   \]
   \[
   x = \frac{0.8 \, \text{mol}}{0.2 \, \text{mol}} = 4
   \]

### Conclusion:
The value of \( x \) in the formula \( \text{FeSO}_4 \cdot x \text{H}_2\text{O} \) is **4**.

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Would you like further explanation or more details on this solution? Here are a few related questions:

1. How is the molar mass of a compound calculated?
2. What are the properties of hydrates and why do they lose water upon heating?
3. How do you balance a chemical reaction involving hydrate decomposition?
4. What role does the mole concept play in chemical calculations?
5. Can you provide an example of another hydrate calculation?

**Tip:** When calculating the molar mass of a compound, always ensure to account for each element's atomic mass based on the number of atoms present in the formula.

Tentukan nilai besaran x pada kristal besi (II) sulfat hidrat (FeSO4·xH2O) dengan massa 44,8 gram. Setelah pemanasan, diperoleh 30,4 gram kristal FeSO4 anhidrat. (Mr FeSO4 = 152; Mr H2O = 18).

Solve to find the value of x in the hydrated iron (II) sulfate crystal (FeSO4·xH2O) using stoichiometry and mole concept. This chemistry problem involves calculating mass differences and applying molar ratios. Suitable for high school students in Grades 10-12.

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