Question

Calculate the grams of oxygen which would be enveloped on eating 5G or potassium triox ochlorate v

Answer 1

To calculate the grams of oxygen produced from the decomposition of potassium trioxochlorate (KClO₃), we can follow these steps:

1. **Chemical Reaction**: The decomposition of potassium trioxochlorate (KClO₃) typically follows the reaction:
\[
2 \text{KClO}_3 (s) \rightarrow 2 \text{KCl} (s) + 3 \text{O}_2 (g)
\]

2. **Molar Mass Calculation**:
- The molar mass of KClO₃ can be calculated as follows:
\[
K: 39.1 \, \text{g/mol} \\
Cl: 35.5 \, \text{g/mol} \\
O: 16.0 \, \text{g/mol} \times 3 = 48.0 \, \text{g/mol} \\
\text{Total}: 39.1 + 35.5 + 48.0 = 122.6 \, \text{g/mol}
\]

3. **Calculate Moles of KClO₃**:
- From 5 g of KClO₃:
\[
\text{Moles of KClO}_3 = \frac{5 \, \text{g}}{122.6 \, \text{g/mol}} \approx 0.0408 \, \text{mol}
\]

4. **Oxygen Produced**:
- From the reaction, 2 moles of KClO₃ produce 3 moles of O₂. Therefore, 1 mole of KClO₃ will produce \(\frac{3}{2}\) moles of O₂. The moles of O₂ produced from 0.0408 moles of KClO₃ can be calculated as follows:
\[
\text{Moles of O}_2 = 0.0408 \, \text{mol KClO}_3 \times \frac{3 \, \text{mol O}_2}{2 \, \text{mol KClO}_3} = 0.0612 \, \text{mol O}_2
\]

5. **Grams of Oxygen**:
- To find the mass of oxygen produced, multiply the number of moles of O₂ by the molar mass of O₂ (32 g/mol):
\[
\text{Mass of O}_2 = 0.0612 \, \text{mol} \times 32 \, \text{g/mol} \approx 1.9584 \, \text{g}
\]

**Final Answer**:
Approximately **1.96 grams** of oxygen would be produced from the decomposition of 5 grams of potassium trioxochlorate (KClO₃).