The mass of iron converted into Fe_3O_4 by th | vedclass

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(D) The balanced chemical equation for the reaction of iron with steam is: $3Fe(s) + 4H_2O(g) \rightarrow Fe_3O_4(s) + 4H_2(g)$.From the stoichiometry

Vedclass · Accepted Answer

$42$

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(D) The balanced chemical equation for the reaction of iron with steam is: $3Fe(s) + 4H_2O(g) ightarrow Fe_3O_4(s) + 4H_2(g)$.From the stoichiometry of the reaction, $4$ moles of $H_2O$ react with $3$ moles of $Fe$.The molar mass of $H_2O = (2 	imes 1) + 16 = 18	ext{ g mol}^{-1}$.Thus, $4 	imes 18	ext{ g} = 72	ext{ g}$ of steam reacts with $3 	imes 56	ext{ g} = 168	ext{ g}$ of iron.Using the unitary method, $18	ext{ g}$ of steam will react with: $\frac{168	ext{ g Fe}}{72	ext{ g H}_2	ext{O}} 	imes 18	ext{ g H}_2	ext{O} = \frac{168}{4} = 42	ext{ g}$ of iron.

The mass of iron converted into $Fe_3O_4$ by the action of $18\text{ g}$ of steam is : (Given: Molar mass of $H$, $O$ and Fe are $1$, $16$ and $56\text{ g mol}^{-1}$ respectively). Assume iron is present in excess: (in $\text{ g}$)

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