Given the reaction:

CO(NH2)2(s)+H2O(g)CO2(g)+2NH3(g)KP=1.39at500K

If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be:____(options: more product-favored, more reactant-favored, unchanged)

A flask containing CO₂(g), NH₃(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₃(g) increase. This means that:

The value of K_P for the given reaction at 600 K is:______(options: smaller than 1.39, larger than 1.39, equal to 1.39)

The reaction CO(NH₂)₂(s) + H₂O(g) CO₂(g) + 2 NH₃(g) is:_____ (options: endothermic or exothermic)