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0.3g of a compound on combustion gave 0....

0.3g of a compound on combustion gave 0.54g of water and 0.88g of carbon dioxide. Find the percentage of carbon and hydrogen in the compound

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To find the percentage of carbon and hydrogen in the given compound, we can follow these steps: ### Step 1: Write down the given data - Weight of the organic compound = 0.3 g - Weight of carbon dioxide (CO₂) produced = 0.88 g - Weight of water (H₂O) produced = 0.54 g ### Step 2: Calculate the amount of carbon in the compound 1. **Find the moles of CO₂ produced:** - Molar mass of CO₂ = 12 (C) + 16*2 (O) = 44 g/mol - Moles of CO₂ = weight of CO₂ / molar mass of CO₂ \[ \text{Moles of CO₂} = \frac{0.88 \, \text{g}}{44 \, \text{g/mol}} = 0.02 \, \text{mol} \] 2. **Calculate the moles of carbon (C) in CO₂:** - Each mole of CO₂ contains 1 mole of C. \[ \text{Moles of C} = 0.02 \, \text{mol} \] 3. **Convert moles of carbon to grams:** - Molar mass of carbon = 12 g/mol \[ \text{Mass of C} = \text{Moles of C} \times \text{Molar mass of C} = 0.02 \, \text{mol} \times 12 \, \text{g/mol} = 0.24 \, \text{g} \] ### Step 3: Calculate the amount of hydrogen in the compound 1. **Find the moles of H₂O produced:** - Molar mass of H₂O = 2 (H) + 16 (O) = 18 g/mol - Moles of H₂O = weight of H₂O / molar mass of H₂O \[ \text{Moles of H₂O} = \frac{0.54 \, \text{g}}{18 \, \text{g/mol}} = 0.03 \, \text{mol} \] 2. **Calculate the moles of hydrogen (H) in H₂O:** - Each mole of H₂O contains 2 moles of H. \[ \text{Moles of H} = 0.03 \, \text{mol} \times 2 = 0.06 \, \text{mol} \] 3. **Convert moles of hydrogen to grams:** - Molar mass of hydrogen = 1 g/mol \[ \text{Mass of H} = \text{Moles of H} \times \text{Molar mass of H} = 0.06 \, \text{mol} \times 1 \, \text{g/mol} = 0.06 \, \text{g} \] ### Step 4: Calculate the percentage of carbon and hydrogen in the compound 1. **Percentage of carbon:** \[ \text{Percentage of C} = \left( \frac{\text{Mass of C}}{\text{Weight of organic compound}} \right) \times 100 = \left( \frac{0.24 \, \text{g}}{0.3 \, \text{g}} \right) \times 100 = 80\% \] 2. **Percentage of hydrogen:** \[ \text{Percentage of H} = \left( \frac{\text{Mass of H}}{\text{Weight of organic compound}} \right) \times 100 = \left( \frac{0.06 \, \text{g}}{0.3 \, \text{g}} \right) \times 100 = 20\% \] ### Final Result: - Percentage of Carbon (C) = 80% - Percentage of Hydrogen (H) = 20% ---
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