Magnetite, `Fe_(3)O_(4)`, can be converted into metallic iron by heating with carbon monoxide as represented by this equation:
`Fe_(3)O_(4)(s)+CO(g) rarr Fe(s) +CO_(2)(g)`
The kilograms of `Fe_(3)O_(4)` which must be processed in this way to obtain `5.00 kg` of iron, if the process is `85%` efficient is closest to? `[M: = Fe = 56]`

Options

A. 8.12 kg
B. 4.14 kg
C. 6.94 kg
D. 16.8 kg

Explanation

To determine the amount of magnetite (`Fe3O4`) needed to produce `5.00 kg` of iron with an efficiency of `85%`, we can follow these steps:

### Step 1: Write the balanced chemical equation.
The balanced chemical equation for the reaction is:
\[ \text{Fe}_3\text{O}_4 (s) + 4 \text{CO} (g) \rightarrow 3 \text{Fe} (s) + 4 \text{CO}_2 (g) \]

### Step 2: Calculate the molar masses.
- Molar mass of `Fe3O4`:
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