In an experiment, 2.4 g of iron oxide on iron. In another experiment, 2.9 g of iron oxide gave 2.09 g of iron on reduction. Which law is ilustrated from the above data?

Options

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

Answer

To solve the question regarding the law illustrated by the given data about iron oxide and iron, we can follow these steps:

### Step 1: Analyze the Data
We have two experiments:
1. In the first experiment, 2.4 g of iron oxide is used.
2. In the second experiment, 2.9 g of iron oxide gives 2.09 g of iron upon reduction.

### Step 2: Determine the Mass of Iron Produced
From the second experiment, we can see that 2.9 g of iron oxide yields 2.09 g of iron. This indicates that there is a specific mass of iron produced from a specific mass of iron oxide.

### Step 3: Calculate the Ratio of Iron Oxide to Iron
To understand the relationship between the mass of iron oxide and the mass of iron produced, we can calculate the ratio of the mass of iron oxide to the mass of iron produced in the second experiment:
- Mass of iron oxide = 2.9 g
- Mass of iron produced = 2.09 g

The ratio can be calculated as:
\[ \text{Ratio} = \frac{\text{Mass of Iron Oxide}}{\text{Mass of Iron}} = \frac{2.9 \, \text{g}}{2.09 \, \text{g}} \]

### Step 4: Compare with First Experiment
Now, we need to compare this ratio with the first experiment where 2.4 g of iron oxide is used. We can assume that the mass of iron produced from 2.4 g of iron oxide will follow the same ratio.

### Step 5: Identify the Law Illustrated
The consistent ratio of the mass of iron oxide to the mass of iron produced in both experiments illustrates the **Law of Conservation of Mass**. This law states that in a chemical reaction, the mass of the reactants must equal the mass of the products.

### Conclusion
The law illustrated by the data provided is the **Law of Conservation of Mass**.

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