226. Considering the reaction: $\mathrm{NiO(s) + CO(g) \rightleftharpoons Ni(s) + CO_2(g)}$, $\Delta H < 0$, which is at equilibrium at a certain temperature, which of the following statements are correct?
The equilibrium constant expression is: $K = \dfrac{[\mathrm{CO_2}]}{[\mathrm{CO}]}$
By decreasing temperature, the equilibrium shifts to establish a larger $K$.
By removing some $\mathrm{Ni(s)}$ from the reaction system, the equilibrium shifts in the forward direction.
By moving to a smaller volume (at constant temperature), the equilibrium establishes a smaller $K$.
(1) 1 (2) 2 (3) 3 (4) 4
\textbf{226.} Considering the reaction: $\mathrm{NiO(s) + CO(g) \rightleftharpoons Ni(s) + CO_2(g)}$, $\Delta H < 0$, which is at equilibrium at a certain temperature, which of the following statements are correct?
\begin{itemize}
\item The equilibrium constant expression is: $K = \dfrac{[\mathrm{CO_2}]}{[\mathrm{CO}]}$
\item By decreasing temperature, the equilibrium shifts to establish a larger $K$.
\item By removing some $\mathrm{Ni(s)}$ from the reaction system, the equilibrium shifts in the forward direction.
\item By moving to a smaller volume (at constant temperature), the equilibrium establishes a smaller $K$.
\end{itemize}
(1) 1 \quad (2) 2 \quad (3) 3 \quad (4) 4