The following data was collected when a reaction was performed experimentally in the laboratory. Reaction Data
Reactants Products
Fe2O3 Al Al2O3 Fe
Starting Amount in Reaction 3 moles 5 moles ? ?

Determine the maximum amount of Fe that was produced during the experiment. Explain how you determined this amount.

5 moles of Fe.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

Fe₂O₃ + 2Al —> Al₂O₃ + 2Fe

From the balanced equation above,

1 mole of Fe₂O₃ reacted with 2 moles of Al to produced 2 moles of Fe.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

1 mole of Fe₂O₃ reacted with 2 moles of Al.

Therefore, 3 moles of Fe₂O₃ will react with = 3 × 2 = 6 moles of Fe.

From the calculation made above, we can see clearly that a higher amount (i.e 6 moles) of Al than what was given (i.e 5 moles) is needed to react completely with 3 moles of Fe₂O₃.

Therefore, Al is the limiting reactant and Fe₂O₃ is the excess reactant.

Finally, we shall determine the maximum amount of Fe produced.

This can be obtained by using the limiting reactant as illustrated below.

NOTE: The limiting reactant is Al.

From the balanced equation above,

2 moles of Al reacted to produce 2 moles of Fe.

Therefore, 5 moles of Al will also react to produce 5 moles of Fe.

Thus, 5 moles of Fe were obtained from the reaction.

b

explanation:

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