Calculate the mass of iron which will be converted into its oxide (`Fe_3O_4`) by the action of 17g of steam on it. [At mass of Fe=56] `Fe+H_2​O→Fe_3O_4+4H_2` ​

Options

A. 23g
B. 16g
C. 40g
D. 17g

Answer

To solve the problem of calculating the mass of iron that will be converted into its oxide (`Fe_3O_4`) by the action of 17g of steam, we can follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction between iron and steam is:
\[ 3Fe + 4H_2O \rightarrow Fe_3O_4 + 4H_2 \]

### Step 2: Determine the molar masses
- Molar mass of iron (Fe) = 56 g/mol
- Molar mass of water (H₂O) = 18 g/mol

### Step 3: Calculate the total mass of reactants
From the balanced equation, we see that:
- 3 moles of Fe react with 4 moles of H₂O.

Calculating the mass of iron and water:
- Mass of 3 moles of Fe = \(3 \times 56 = 168 \text{ g}\)
- Mass of 4 moles of H₂O = \(4 \times 18 = 72 \text{ g}\)

### Step 4: Establish the ratio of iron to steam
From the balanced equation, we can see that:
- 168 g of Fe reacts with 72 g of H₂O.

### Step 5: Set up a proportion to find the mass of iron for 17 g of steam
Using the ratio we established:
\[ \frac{168 \text{ g Fe}}{72 \text{ g H}_2O} = \frac{x \text{ g Fe}}{17 \text{ g H}_2O} \]

### Step 6: Solve for x (mass of iron)
Cross-multiplying gives:
\[ 168 \times 17 = 72 \times x \]
\[ 2856 = 72x \]
Now, divide both sides by 72:
\[ x = \frac{2856}{72} = 39.6 \text{ g} \]

### Step 7: Round the answer
The mass of iron that will be converted into its oxide by the action of 17g of steam is approximately 40 g.

### Final Answer
The mass of iron converted into its oxide is approximately **40 g**.

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