`0.24 g`of an organic compound gave `0.22 g O_(2)` on complete combustion. If it contains `1.66%` hydrogen, then the percentage of `C` and `O` will be

Options

A. `12.5` and `36.6`
B. `25` and `75`
C. `25` and `36.6`
D. `25` and `80`

Explanation

To find the percentage of carbon (C) and oxygen (O) in the organic compound, we can follow these steps:

### Step 1: Determine the mass of carbon dioxide produced
The mass of oxygen (O₂) produced during combustion is given as 0.22 g. The molecular weight of O₂ is 32 g/mol, and the molecular weight of carbon dioxide (CO₂) is 44 g/mol.

Using the stoichiometry of the combustion reaction, we can find the mass of CO₂ produced from the mass of O₂:
- From the reaction:
\[ C + O_2 \rightarrow CO_2 \]
1 mole of O₂ produces 2 moles of CO₂. Therefore, the mass of CO₂ produced can be calculated as follows:
\[ \text{Mass of CO₂} = \frac{44}{32} \times \text{Mass of O₂} \]
\[ \text{Mass of CO₂} = \frac{44}{32} \times 0.22 \, \text{g} \]

### Step 2: Calculate the mass of carbon in the compound
Next, we need to find the mass of carbon in the CO₂ produced. The mass of carbon in CO₂ can be calculated using the ratio of the molar mass of carbon to the molar mass of CO₂:
- The molar mass of carbon (C) is 12 g/mol.
- The molar mass of CO₂ is 44 g/mol.

Using the formula:
\[ \text{Mass of C} = \left(\frac{12}{44}\right) \times \text{Mass of CO₂} \]

### Step 3: Calculate the percentage of carbon (C)
Now, we can find the percentage of carbon in the organic compound:
\[ \text{Percentage of C} = \left(\frac{\text{Mass of C}}{\text{Mass of compound}}\right) \times 100 \]
Where the mass of the compound is given as 0.24 g.

### Step 4: Calculate the percentage of hydrogen (H)
The percentage of hydrogen in the compound is given as 1.66%.

### Step 5: Calculate the percentage of oxygen (O)
To find the percentage of oxygen, we can use the fact that the total percentage of all elements in the compound must equal 100%. Thus:
\[ \text{Percentage of O} = 100 - (\text{Percentage of C} + \text{Percentage of H}) \]

### Step 6: Final calculations
Now, we can substitute the values and perform the calculations to find the percentages of carbon and oxygen.