1.5 g of hydrocarbon on combustion in excess of oxygen produces 4.4 g of `CO_(2)` and 2.7 g of `H_(2)O`, the data illustrates

Options

A. Law of conservation of mass
B. Law of multiple proportions
C. Law of constant composition
D. Law of reciprocal proportions.

Explanation

To solve the problem, we need to analyze the combustion of the hydrocarbon and determine the relevant masses of carbon and hydrogen produced in the reaction. Here's a step-by-step breakdown:

### Step 1: Identify the mass of hydrocarbon
The mass of the hydrocarbon is given as 1.5 g.

### Step 2: Calculate the mass of carbon in CO₂
We know that 4.4 g of CO₂ is produced. The molar mass of CO₂ is calculated as follows:
- Molar mass of CO₂ = 12 g/mol (for C) + 16 g/mol × 2 (for O) = 12 + 32 = 44 g/mol.

Now, we can find the mass of carbon in 4.4 g of CO₂:
- Mass of carbon in CO₂ = (mass of CO₂ × mass of C in CO₂) / molar mass of CO₂
- Mass of carbon in CO₂ = (4.4 g × 12 g/mol) / 44 g/mol = 1.2 g.

### Step 3: Calculate the mass of hydrogen in H₂O
Next, we know that 2.7 g of H₂O is produced. The molar mass of H₂O is:
- Molar mass of H₂O = 2 g/mol (for H) + 16 g/mol (for O) = 2 + 16 = 18 g/mol.

Now, we can find the mass of hydrogen in 2.7 g of H₂O:
- Mass of hydrogen in H₂O = (mass of H₂O × mass of H in H₂O) / molar mass of H₂O
- Mass of hydrogen in H₂O = (2.7 g × 2 g/mol) / 18 g/mol = 0.3 g.

### Step 4: Calculate total mass of carbon and hydrogen
Now, we can add the masses of carbon and hydrogen to find the total mass of the products:
- Total mass of carbon and hydrogen = mass of carbon + mass of hydrogen
- Total mass = 1.2 g (C) + 0.3 g (H) = 1.5 g.

### Step 5: Compare the mass of reactants and products
The initial mass of the hydrocarbon is 1.5 g, and the total mass of the products (CO₂ and H₂O) is also 1.5 g. This confirms that the mass of the reactants equals the mass of the products.

### Conclusion
Since the mass of the reactants equals the mass of the products, this illustrates the **law of conservation of mass**.

### Final Answer
The data illustrates the **law of conservation of mass**.

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