The oxides of nitrogen contain `63.65%, 46.69%` and `30.46%` of nitrogen respectively. This data illustrate the law of

Options

A. Constant Proportions
B. Multiple Proportions
C. Reciprocal Proportions
D. Conservation of mass

Explanation

To solve the question regarding the oxides of nitrogen and the percentages of nitrogen they contain, we can follow these steps:

### Step 1: Identify the Percentages of Nitrogen
We have three oxides of nitrogen with the following percentages of nitrogen:
1. 63.65%
2. 46.69%
3. 30.46%

### Step 2: Calculate the Mass of Nitrogen and Oxygen for Each Oxide
Assuming we have 100 grams of each oxide, we can calculate the mass of nitrogen and oxygen in each case.

1. **For the first oxide (63.65% N):**
- Mass of nitrogen = 63.65 grams
- Mass of oxygen = 100 - 63.65 = 36.35 grams

2. **For the second oxide (46.69% N):**
- Mass of nitrogen = 46.69 grams
- Mass of oxygen = 100 - 46.69 = 53.31 grams

3. **For the third oxide (30.46% N):**
- Mass of nitrogen = 30.46 grams
- Mass of oxygen = 100 - 30.46 = 69.54 grams

### Step 3: Calculate the Mass Ratio of Oxygen to Nitrogen for Each Oxide
Next, we will find the mass of oxygen that combines with 1 gram of nitrogen for each oxide.

1. **For the first oxide:**
- Ratio of oxygen to nitrogen = 36.35 g O / 63.65 g N = 0.571 g O per g N

2. **For the second oxide:**
- Ratio of oxygen to nitrogen = 53.31 g O / 46.69 g N = 1.141 g O per g N

3. **For the third oxide:**
- Ratio of oxygen to nitrogen = 69.54 g O / 30.46 g N = 2.282 g O per g N

### Step 4: Normalize the Ratios
To find a simple whole number ratio, we will divide all ratios by the second ratio (1.141).

1. **First oxide:**
- 0.571 / 1.141 = 0.5

2. **Second oxide:**
- 1.141 / 1.141 = 1

3. **Third oxide:**
- 2.282 / 1.141 = 2

### Step 5: Write the Ratios
The ratios of oxygen to nitrogen for the three oxides can now be expressed as:
- First oxide: 0.5
- Second oxide: 1
- Third oxide: 2

Expressing these in whole numbers gives us:
- 1 : 2 : 4

### Conclusion
This data illustrates the **Law of Multiple Proportions**, which states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.