High School

Calculate the number of moles of [tex]O_2[/tex] and [tex]H_2O[/tex] that are required to react completely with 1.55 mol [tex]Fe[/tex] in the following reaction:

\[ 2Fe(s) + O_2(g) + 2H_2O(l) \rightarrow 2Fe(OH)_2(s) \]

A. 0.775 mol [tex]O_2[/tex] and 1.55 mol [tex]H_2O[/tex]
B. 1.55 mol [tex]O_2[/tex] and 0.775 mol [tex]H_2O[/tex]
C. 3.10 mol [tex]O_2[/tex] and 1.55 mol [tex]H_2O[/tex]
D. 1.55 mol [tex]O_2[/tex] and 3.10 mol [tex]H_2O[/tex]

Answer :

To react completely with 1.55 mol Fe, 0.775 mol O2 and 0.775 mol H2O are required.

To calculate the number of moles of O2 and H2O required to react with 1.55 mol Fe, we need to use the stoichiometry of the reaction. From the balanced equation, we can see that the ratio of Fe to O2 is 2:1, and the ratio of Fe to H2O is also 2:1. Therefore, the number of moles of O2 required will be half of the number of moles of Fe, which is 0.775 mol. Similarly, the number of moles of H2O required will also be 0.775 mol.

Learn more about stoichiometry here:

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