The following data was collected when a reaction was performed experimentally in the laboratory. Determine the maximum amount of Fe that was produced during experiment. Explain how you determine this amount. (5 points)

5 moles

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 produce 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 = 2 × 3 = 6 moles of Al.

From the calculation made above, we can see 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 Fe produced from the reaction.

Here, the limiting reactant will be use because all of it is consumed by the reaction.

The limiting reactant is Al and the maximum amount of Fe produced can be obtained as follow:

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, the maximum amount of Fe produced is 5 moles.

b is the correct

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.