CO(NH$_2$)$_2$(s) + H$_2$O(g) $\rightleftharpoons$ CO$_2$(g) + 2 NH$_3$(g) K$_p$ = 1.39 at 500 K
If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be
A flask containing CO$_2$(g), NH$_3$(g), CO(NH$_2$)$_2$(s) and H$_2$O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH$_2$)$_2$(s) and H$_2$O(g) decrease and the amounts of CO$_2$(g) and NH$_3$(g) increase. This means that:
The value of K$_p$ for the given reaction at 600 K is
The reaction CO(NH$_2$)$_2$(s) + H$_2$O(g) $\rightarrow$ CO$_2$(g) + 2 NH$_3$(g) is
