The reaction between iron(II) oxide and carbon monoxide produces iron and carbon dioxide. How many moles of iron can be obtained when 1.75 mol FeO reacts with an excess of CO?

[tex]\[ \text{FeO} + \text{CO} \longrightarrow \text{Fe} + \text{CO}_2 \][/tex]

Moles of Fe:



Answer :

To determine how many moles of iron (Fe) can be obtained when 1.75 moles of iron(II) oxide (FeO) reacts with an excess of carbon monoxide (CO), let's follow these steps:

1. Understand the balanced chemical equation:

The reaction is:
[tex]\[ \text{FeO} + \text{CO} \longrightarrow \text{Fe} + \text{CO}_2 \][/tex]

2. Identify the molar ratio:

From the balanced chemical equation, we can see that 1 mole of FeO reacts with 1 mole of CO to produce 1 mole of Fe and 1 mole of CO₂. The molar ratio of FeO to Fe is 1:1.

3. Calculate the moles of iron (Fe) produced:

Since the molar ratio of FeO to Fe is 1:1, the number of moles of Fe produced will be the same as the number of moles of FeO that reacted.

Given:
[tex]\[ \text{moles of FeO} = 1.75 \, \text{mol} \][/tex]

Therefore, the moles of Fe produced will also be 1.75 mol.

Thus, when 1.75 moles of FeO reacts with an excess of CO, 1.75 moles of iron (Fe) can be obtained.