An organic compound contains 69% carbon and 4.8% hydrogen, the remainder being oxygen. What will be the masses off carbon dioxide and water produced when 0.20 g of this substance is subjected to complete combustion.

Options

A. 0.40g
B. 0.50g
C. 0.60g
D. 0.70g

Explanation

To solve the problem step by step, we will follow the outlined procedure to find the masses of carbon dioxide (CO2) and water (H2O) produced from the complete combustion of the organic compound.

### Step 1: Determine the composition of the organic compound
Given:
- Percentage of Carbon (C) = 69%
- Percentage of Hydrogen (H) = 4.8%
- Percentage of Oxygen (O) = 100% - (69% + 4.8%) = 26.2%

### Step 2: Calculate the mass of carbon and hydrogen in 0.20 g of the organic compound
- Mass of Carbon in 0.20 g = (69 g C / 100 g compound) × 0.20 g = 0.138 g C
- Mass of Hydrogen in 0.20 g = (4.8 g H / 100 g compound) × 0.20 g = 0.0096 g H

### Step 3: Calculate the moles of carbon and hydrogen
- Moles of Carbon (C):
\[ \text{Moles of C} = \frac{\text{mass of C}}{\text{molar mass of C}} = \frac{0.138 \text{ g}}{12 \text{ g/mol}} = 0.0115 \text{ mol} \]

- Moles of Hydrogen (H):
\[ \text{Moles of H} = \frac{\text{mass of H}}{\text{molar mass of H}} = \frac{0.0096 \text{ g}}{1 \text{ g/mol}} = 0.0096 \text{ mol} \]

### Step 4: Calculate the moles of CO2 produced
From the combustion reaction:
\[ \text{C} + \text{O}_2 \rightarrow \text{CO}_2 \]
1 mole of carbon produces 1 mole of CO2. Therefore, the moles of CO2 produced will be equal to the moles of carbon:
- Moles of CO2 = 0.0115 mol

### Step 5: Calculate the mass of CO2 produced
- Molar mass of CO2 = 12 g/mol (C) + 32 g/mol (O2) = 44 g/mol
- Mass of CO2 produced:
\[ \text{Mass of CO2} = \text{moles of CO2} \times \text{molar mass of CO2} = 0.0115 \text{ mol} \times 44 \text{ g/mol} = 0.506 \text{ g} \]

### Step 6: Calculate the moles of H2O produced
From the combustion reaction:
\[ \text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O} \]
2 moles of hydrogen produce 2 moles of H2O. Therefore, the moles of H2O produced will be equal to the moles of hydrogen divided by 2:
- Moles of H2O = 0.0096 mol / 2 = 0.0048 mol

### Step 7: Calculate the mass of H2O produced
- Molar mass of H2O = 2 g/mol (H2) + 16 g/mol (O) = 18 g/mol
- Mass of H2O produced:
\[ \text{Mass of H2O} = \text{moles of H2O} \times \text{molar mass of H2O} = 0.0048 \text{ mol} \times 18 \text{ g/mol} = 0.0864 \text{ g} \]

### Final Results
- Mass of CO2 produced = 0.506 g
- Mass of H2O produced = 0.0864 g