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⭐️ [50 POINTS, BRAINLIEST, ASAP] A chemistry student was asked to calculate the number of moles of iron required to react with 1.20 mol of Oxygen to produce Iron (III) Oxide. His calculation is shown below.

Is the student correct? Use evidence to support your answer.
[tex] 1 \: mole \: o2 \: \times \frac{1\: \: mole \: fe\: }{1 \: mole \: o2} = 1.20 \: mole \: fe[/tex]
Thank you so much!​

Answer :

s1llvrya
hii

the student's calculation is incorrect. The correct number of moles of iron required is 1.60 mol Fe


you have to determine the balanced chemical equation for the reaction between iron and oxygen to produce Iron (III) Oxide:
4Fe+3O 2 →2Fe 2 O 3
​
then calculate the number of moles of iron required to react with 1.20 mol of oxygen using the stoichiometry of the balanced equation:

1.20 mol O 2 × 3 mol O 2 / 4 mol Fe = 1.60 mol Fe

finally compare the student's calculation (1.20 mol Fe) with the correct calculation (1.60 mol Fe).
So The student's calculation of 1.20 mol Fe is incorrect. the correct number of moles of iron required to react with 1.20 mol of oxygen to produce Iron (III) Oxide is 1.60 mol Fe.

hope this helps ^^

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