6 g of carbon combines with 32 g of sulphur to form `CS_(2)`. 12 g of C also combine with 32 g of oxygen to form carbon dioxide. 10 g of sulphur combines with 10 g of oxygen to form sulphur dioxide. Which law is illustrated by them?

Options

A. Law of multiple proportions
B. Law of constant composition
C. Law of reciprocal proportions
D. Gay Lussac's law.

Explanation

To determine which law is illustrated by the given reactions, we will analyze the data provided step by step.

### Step 1: Analyze the first reaction
In the first reaction, 6 g of carbon (C) combines with 32 g of sulfur (S) to form carbon disulfide (CS₂).

- The ratio of carbon to sulfur in this reaction is:
\[ \text{Ratio of C to S} = \frac{6 \text{ g}}{32 \text{ g}} = \frac{3}{16} \]

### Step 2: Analyze the second reaction
In the second reaction, 12 g of carbon combines with 32 g of oxygen (O) to form carbon dioxide (CO₂).

- The ratio of carbon to oxygen in this reaction is:
\[ \text{Ratio of C to O} = \frac{12 \text{ g}}{32 \text{ g}} = \frac{3}{8} \]

### Step 3: Analyze the third reaction
In the third reaction, 10 g of sulfur combines with 10 g of oxygen to form sulfur dioxide (SO₂).

- The ratio of sulfur to oxygen in this reaction is:
\[ \text{Ratio of S to O} = \frac{10 \text{ g}}{10 \text{ g}} = 1 \]

### Step 4: Compare the ratios
Now, let's compare the ratios derived from the reactions:

1. From the first reaction (C and S): 3 g of C combines with 16 g of S.
2. From the second reaction (C and O): 6 g of C combines with 16 g of O.
3. From the third reaction (S and O): 10 g of S combines with 10 g of O.

### Step 5: Identify the law
The data shows that when a fixed mass of one element (carbon) is combined with different elements (sulfur and oxygen), they combine in simple whole number ratios. This 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 ratios of small whole numbers.

### Conclusion
The law illustrated by the reactions provided is the **Law of Multiple Proportions**.

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