To determine the equilibrium constant, Kp, for the decomposition reaction of the solid compound XY into its gaseous components X and Y, we need to consider the following reaction:
XY (s)⇌X (g)+Y (g)
For a reaction where a solid decomposes into gases, the equilibrium constant Kp is defined in terms of the partial pressures of the gaseous products. Since XY is a solid, its activity is considered to be 1 and does not appear in the equilibrium expression. Hence the expression for Kp is:
Kp=PX⋅PY
Where PX and PY are the partial pressures of the gases X and Y, respectively.
Given that the total pressure at equilibrium is 10 bar, and assuming that X and Y are present in equal amounts due to the stoichiometry of the decomposition reaction (i.e., 1:1), we can write:
PX=PY=210=5bar
Substituting these partial pressures into the expression for Kp gives:
Kp=PX⋅PY=5bar⋅5bar=25bar2
Therefore, the equilibrium constant Kp for this reaction is 25. Thus, the correct answer is:
Option C - 25