In the given reaction,calculate the number of electrons lost by iron:
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$
(8) The balanced chemical equation is: $3Fe + 4H_2O \to Fe_3O_4 + 4H_2$
In the reactant side,the oxidation state of $Fe$ is $0$.
In the product side,$Fe_3O_4$ is a mixed oxide of $FeO$ and $Fe_2O_3$. The oxidation state of $Fe$ in $Fe_3O_4$ is calculated as: $3x + 4(-2) = 0 \implies 3x = 8 \implies x = +8/3$.
Total change in oxidation state for $3$ atoms of $Fe$ is: $3 \times (+8/3 - 0) = 8$.
Therefore,the number of electrons lost by iron is $8$.
In the reactant side,the oxidation state of $Fe$ is $0$.
In the product side,$Fe_3O_4$ is a mixed oxide of $FeO$ and $Fe_2O_3$. The oxidation state of $Fe$ in $Fe_3O_4$ is calculated as: $3x + 4(-2) = 0 \implies 3x = 8 \implies x = +8/3$.
Total change in oxidation state for $3$ atoms of $Fe$ is: $3 \times (+8/3 - 0) = 8$.
Therefore,the number of electrons lost by iron is $8$.
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