Two gaseous sample were analysed. One contained 1.2 g of carbon and 3.2 g of oxygen. The other contained `27.3%` carbon and `72.7%` oxygen. The experimental data are in accordance with

Options

A. Law of conservation of mass
B. Law of definite proportions
C. Law of reciprocal proportion
D. Law of multiple proportions

Explanation

To solve the problem, we need to analyze the two gaseous samples provided and determine the law of chemistry they adhere to based on their composition.

### Step-by-Step Solution:

1. **Identify the Composition of the First Sample:**
- Given:
- Mass of Carbon (C) = 1.2 g
- Mass of Oxygen (O) = 3.2 g
- Total mass of the sample = 1.2 g + 3.2 g = 4.4 g

2. **Calculate the Percentage of Carbon in the First Sample:**
\[ \text{Percentage of Carbon} = \left( \frac{\text{Mass of Carbon}}{\text{Total Mass}} \right) \times 100 = \left( \frac{1.2}{4.4} \right) \times 100 \approx 27.27\% \]

3. **Calculate the Percentage of Oxygen in the First Sample:**
\[ \text{Percentage of Oxygen} = \left( \frac{\text{Mass of Oxygen}}{\text{Total Mass}} \right) \times 100 = \left( \frac{3.2}{4.4} \right) \times 100 \approx 72.73\% \]

4. **Identify the Composition of the Second Sample:**
- Given:
- Percentage of Carbon = 27.3%
- Percentage of Oxygen = 72.7%

5. **Compare the Percentages:**
- From the calculations above, we see that:
- First Sample: Carbon = 27.27%, Oxygen = 72.73%
- Second Sample: Carbon = 27.3%, Oxygen = 72.7%
- The percentages of Carbon and Oxygen in both samples are approximately the same.

6. **Determine the Law of Chemistry:**
- Since both samples have the same percentage composition of Carbon and Oxygen, they are in accordance with the **Law of Definite Proportions**. This law states that a chemical compound always contains its component elements in fixed ratio by mass, regardless of the source or method of preparation.

### Conclusion:
The experimental data are in accordance with the **Law of Definite Proportions**.

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