Two gaseous samples 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 experiemental data is an accordance with

Answer

To solve the problem step by step, we will analyze the two gaseous samples and determine if they adhere to any specific chemical law.

### Step 1: Analyze the first sample
We have the following data for the first sample:
- Mass of carbon (C) = 1.2 g
- Mass of oxygen (O) = 3.2 g

**Calculation of total mass:**
Total mass = Mass of carbon + Mass of oxygen
Total mass = 1.2 g + 3.2 g = 4.4 g

**Calculation of percentage of carbon:**
Percentage of carbon = (Mass of carbon / Total mass) × 100
Percentage of carbon = (1.2 g / 4.4 g) × 100 ≈ 27.27%

**Calculation of percentage of oxygen:**
Percentage of oxygen = (Mass of oxygen / Total mass) × 100
Percentage of oxygen = (3.2 g / 4.4 g) × 100 ≈ 72.73%

### Step 2: Analyze the second sample
The second sample contains:
- 27.3% carbon
- 72.7% oxygen

### Step 3: Compare the percentages
From the first sample, we calculated:
- Percentage of carbon = 27.27%
- Percentage of oxygen = 72.73%

From the second sample, we have:
- Percentage of carbon = 27.3%
- Percentage of oxygen = 72.7%

### Step 4: Conclusion
The percentages of carbon and oxygen in both samples are very close to each other. This indicates that both samples contain the same ratio of elements, which is consistent with the Law of Definite Proportions. This law states that a chemical compound always contains its component elements in fixed ratio by mass.

### Final Answer
The experimental data is in accordance with the Law of Definite Proportions.

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