Question 6 (5 points) (05.05 MC)
The following data was collected when a reaction was performed experimentally in the laboratory

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

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 = 3 × 2 = 6 moles of Al.

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

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

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

In this case, the limiting reactant will be used because all of it is consumed by the reaction.

The limiting reactant is Al and 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 was 5 moles.

thats a little if u want the answer just look it up on google thats what i do haha : )

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be