227- $\mathrm{H_2(g)}$ and $\mathrm{Fe_3O_4(s)}$ are introduced into a vessel at a certain temperature and the following reaction is carried out: $$\mathrm{Fe_3O_4(s) + 4H_2(g) \rightleftharpoons 3Fe(s) + 4H_2O(g)}$$ This equilibrium is established. The equilibrium molar concentration of $\mathrm{H_2O(g)}$ is twice the equilibrium molar concentration of $\mathrm{H_2(g)}$. If $0.6$ mol of iron is present in the equilibrium mixture, approximately what percent by mass of the gas mixture is hydrogen gas at equilibrium? (Read the options from right to left, $\mathrm{H=1,\ O=16\ :\ g.mol^{-1}}$) (1) $14.8$ , $8$ (2) $5.76$ , $8$ (3) $14.8$ , $16$ (4) $5.76$ , $16$
\textbf{227-} $\mathrm{H_2(g)}$ and $\mathrm{Fe_3O_4(s)}$ are introduced into a vessel at a certain temperature and the following reaction is carried out:
$$\mathrm{Fe_3O_4(s) + 4H_2(g) \rightleftharpoons 3Fe(s) + 4H_2O(g)}$$
This equilibrium is established. The equilibrium molar concentration of $\mathrm{H_2O(g)}$ is twice the equilibrium molar concentration of $\mathrm{H_2(g)}$. If $0.6$ mol of iron is present in the equilibrium mixture, approximately what percent by mass of the gas mixture is hydrogen gas at equilibrium? (Read the options from right to left, $\mathrm{H=1,\ O=16\ :\ g.mol^{-1}}$)
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(1) $14.8$ , $8$ \qquad (2) $5.76$ , $8$ \qquad (3) $14.8$ , $16$ \qquad (4) $5.76$ , $16$
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