1. គេដុតថ្មកំបោរ CaCO3 50g នៅពិសោធន៍ គេទទួលបាន កាល់ស្យូមអុកសុីត CaO 21g ។ ចូរគណនា ទិន្នផលជាភាគរយនៃប្រតិកម្មនេះ ។ ( គេឲ្យ Ca= 40g/mol , O= 16g/mol )
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To calculate the percentage yield of the reaction, we need to first determine the theoretical yield of calcium oxide (CaO) from the given amount of calcium carbonate (CaCO₃), and then compare it to the actual yield obtained.

### Step 1: Calculate the Molar Mass of CaCO₃ and CaO
- **Molar mass of CaCO₃**:  
  \( \text{Ca} = 40 \, \text{g/mol} \)  
  \( \text{C} = 12 \, \text{g/mol} \)  
  \( \text{O} = 16 \, \text{g/mol} \times 3 = 48 \, \text{g/mol} \)  
  So, \( \text{Molar mass of CaCO₃} = 40 + 12 + 48 = 100 \, \text{g/mol} \)

- **Molar mass of CaO**:  
  \( \text{Ca} = 40 \, \text{g/mol} \)  
  \( \text{O} = 16 \, \text{g/mol} \)  
  So, \( \text{Molar mass of CaO} = 40 + 16 = 56 \, \text{g/mol} \)

### Step 2: Write the Balanced Chemical Equation
The decomposition of calcium carbonate can be represented as:

\[ \text{CaCO}_3 \rightarrow \text{CaO} + \text{CO}_2 \]

### Step 3: Calculate the Theoretical Yield
- **Mass of CaCO₃ given**: 50 g
- **Moles of CaCO₃**:  
  \( \text{Moles of CaCO₃} = \frac{\text{Mass of CaCO₃}}{\text{Molar mass of CaCO₃}} = \frac{50 \, \text{g}}{100 \, \text{g/mol}} = 0.5 \, \text{mol} \)

- **Theoretical moles of CaO produced**:  
  From the balanced equation, 1 mole of CaCO₃ produces 1 mole of CaO.  
  So, 0.5 moles of CaCO₃ would produce 0.5 moles of CaO.

- **Theoretical mass of CaO**:  
  \( \text{Mass of CaO} = \text{Moles of CaO} \times \text{Molar mass of CaO} = 0.5 \, \text{mol} \times 56 \, \text{g/mol} = 28 \, \text{g} \)

### Step 4: Calculate the Percentage Yield
- **Actual yield of CaO**: 21 g
- **Percentage yield**:

\[
\text{Percentage yield} = \left(\frac{\text{Actual yield}}{\text{Theoretical yield}}\right) \times 100 = \left(\frac{21 \, \text{g}}{28 \, \text{g}}\right) \times 100 \approx 75\%
\]

### Final Answer:
The percentage yield of the reaction is approximately **75%**.

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### Additional Questions:
1. What factors could lead to a lower-than-expected percentage yield?
2. How can impurities affect the yield in a chemical reaction?
3. What is the significance of theoretical yield in chemical experiments?
4. How does one determine the limiting reagent in a chemical reaction?
5. What are common methods to increase the percentage yield in a reaction?
6. How does temperature affect the yield of a reaction?
7. Can you explain the concept of atom economy in green chemistry?
8. How would the yield change if the reaction were performed in a closed system?

**Tip:** Always verify the balanced chemical equation before performing any stoichiometric calculations to avoid errors.

Learn how to calculate the percentage yield of CaO produced from the decomposition of CaCO3. This problem involves stoichiometry and molar mass calculations. Get a step-by-step solution with detailed calculations and formula usage.

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