227- 5 mol of $\mathrm{CO(g)}$ with 16g of $\mathrm{H_2(g)}$ in a closed lithium vessel, according to the equation: $$\mathrm{CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)}$$ are introduced and the reaction proceeds. If after half an hour 96g of methanol is produced, and the reaction reaches equilibrium, the average rate of consumption of $\mathrm{H_2(g)}$, in $\mathrm{mol.L^{-1}.s^{-1}}$, and the value of K in units of $\mathrm{L^2.mol^{-2}}$, which is correct? $$(H = 1,\ C = 12,\ O = 16 : \mathrm{g.mol^{-1}})$$ (1) $9/375\ ,\ 6/67\times10^{-4}$ (2) $9/375\ ,\ 2/78\times10^{-4}$ [6pt] (3) $3/75\ ,\ 2/78\times10^{-4}$ (4) $3/75\ ,\ 6/67\times10^{-4}$
\textbf{227-} 5 mol of $\mathrm{CO(g)}$ with 16g of $\mathrm{H_2(g)}$ in a closed lithium vessel, according to the equation:
$$\mathrm{CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)}$$
are introduced and the reaction proceeds. If after half an hour 96g of methanol is produced, and the reaction reaches equilibrium, the average rate of consumption of $\mathrm{H_2(g)}$, in $\mathrm{mol.L^{-1}.s^{-1}}$, and the value of K in units of $\mathrm{L^2.mol^{-2}}$, which is correct?
$$(H = 1,\ C = 12,\ O = 16 : \mathrm{g.mol^{-1}})$$
\begin{center}
(1) $9/375\ ,\ 6/67\times10^{-4}$ \hspace{2cm} (2) $9/375\ ,\ 2/78\times10^{-4}$\\[6pt]
(3) $3/75\ ,\ 2/78\times10^{-4}$ \hspace{2cm} (4) $3/75\ ,\ 6/67\times10^{-4}$
\end{center}