Moles of iron which can be made from `Fe_(2)O_(3)` by the use of 294 g of carbon monoxide in the reaction :
`Fe_(2)O_(3) + 3 CO to 2Fe + CO_(2)` are:

Explanation

To determine the number of moles of iron (Fe) that can be produced from 294 g of carbon monoxide (CO) in the reaction:

\[ \text{Fe}_2\text{O}_3 + 3 \text{CO} \rightarrow 2 \text{Fe} + \text{CO}_2 \]

we will follow these steps:

### Step 1: Write the balanced chemical equation.
The balanced equation is already provided:

\[ \text{Fe}_2\text{O}_3 + 3 \text{CO} \rightarrow 2 \text{Fe} + \text{CO}_2 \]

### Step 2: Calculate the number of moles of CO.
To find the number of moles of CO, we use the formula:

\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]

The molar mass of CO (Carbon monoxide) is approximately 28 g/mol (12 g/mol for carbon + 16 g/mol for oxygen).

Given mass of CO = 294 g, we calculate:

\[ \text{Number of moles of CO} = \frac{294 \, \text{g}}{28 \, \text{g/mol}} = 10.5 \, \text{moles} \]

### Step 3: Use stoichiometry to find moles of Fe produced.
From the balanced equation, we see that 3 moles of CO produce 2 moles of Fe. Therefore, we can set up a ratio:

\[ \frac{2 \, \text{moles of Fe}}{3 \, \text{moles of CO}} = \frac{x \, \text{moles of Fe}}{10.5 \, \text{moles of CO}} \]

Cross-multiplying gives us:

\[ x = \frac{2}{3} \times 10.5 \]

Calculating this:

\[ x = \frac{21}{3} = 7 \, \text{moles of Fe} \]

### Final Answer:
The number of moles of iron (Fe) that can be produced from 294 g of carbon monoxide (CO) is **7 moles**.

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