Respuesta :
Answer:
39.168g of [tex]O_{2}[/tex]
Explanation:
Step 1: Determine the number of moles of [tex]KClO_{3}[/tex]
[tex]n=\frac{m}{M}[/tex]
where 'n' is the number of moles, m is the mass of compound and M is the molar mass of compound
[tex]n_{KClO_{3}}=\frac{m_{KClO_{3}}}{M_{KClO_{3}}}[/tex]
[tex]n_{KClO_{3}}=\frac{100.0}{39+35.5+3(16)}[/tex]
[tex]n_{KClO_{3}}=\frac{100.0}{122.5}[/tex]
[tex]n_{KClO_{3}}=0.816 mol[/tex]
Step 2: Determine number of moles of [tex]O_{2}[/tex] produced per mole of [tex]KClO_{3}[/tex] decomposed
[tex]2KClO_{3} -> 3O_{2} + 2KCl[/tex]
1 mole of [tex]KClO_{3}[/tex] will produce 1.5 moles of [tex]O_{2}[/tex]
[tex]n_{O_{2}} = 1.5 * n_{KClO_{3}}[/tex]
[tex]n_{O_{2}} = 1.5 * 0.816[/tex]
[tex]n_{O_{2}} = 1.224 mol[/tex]
Step 3: Determine mass of [tex]O_{2}[/tex]
[tex]m_{O_{2}}=n_{O_{2}}M_{O_{2}}[/tex]
[tex]m_{O_{2}}=1.224*2(16)[/tex]
[tex]m_{O_{2}}=39.168 g[/tex]
The mass of oxygen produced from the decomposition of 100g of KClO₃ is approximately 39.20 g
Let's represent the decomposition with a balance chemical equation. Therefore,
- 2KClO₃ → 2KCl + 3O₂
molar mass of 2 moles of KClO₃ = 2(39 + 35.5 + 48) = 2(122.5) = 245 g
molar mass of 3 moles of oxygen molecules = 3(32) = 96 g
245 g of potassium chlorate gives 96 g of oxygen
100 g of potassium chlorate will give ? of oxygen
cross multiply
mass of oxygen produced = (96 × 100)/245
mass of oxygen produced = 9600 / 245
mass of oxygen produced = 39.1836734694
mass of oxygen produced ≈ 39.20 g
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