Answer:
A. 1 mole of Fe.
B. 1.5 moles of CO₂.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
Fe₂O₃ + 3CO —> 2Fe + 3CO₂
From the balanced equation above,
1 mole of Fe₂O₃ reacted with 3 moles of CO to produced 2 moles of Fe and 3 moles of CO₂.
Next, we shall determine the limiting reactant. This can be obtained as follow:
From the balanced equation above,
1 mole of Fe₂O₃ reacted with 3 moles of CO.
Therefore, 3 moles of Fe₂O₃ will react with = 3 × 3 = 9 moles of CO.
From the calculation made above, we can see clearly that it will require a higher amount (i.e 9 moles) of CO than what was given (i.e 1.5 moles) to react completely with 3 moles of Fe₂O₃.
Therefore, CO is the limiting reactant and Fe₂O₃ is the excess reactant.
A. Determination of the number of mole of Fe produced.
NOTE: The limiting reactant is used to obtain the desired result because it will give the maximum yield of the products since all of it is consumed in the reaction.
From the balanced equation above,
3 moles of CO reacted to produced 2 moles of Fe.
Therefore, 1.5 moles of CO will react to produce = (1.5 × 2)/3 = 1 mole of Fe.
Thus, 1 mole of Fe was obtained from the reaction.
B. Determination of the number of mole of CO₂ produced.
From the balanced equation above,
3 moles of CO reacted to produced 3 moles of CO₂.
Therefore, 1.5 moles of CO will also react to produce 1.5 moles of CO₂.
Thus, 1.5 moles of CO₂ were obtained from the reaction.
