For a reaction A_{(s)} rightleftharpoons B_{( | vedclass

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(C) For the reaction $A_{(s)} \rightleftharpoons B_{(s)} + C_{(g)}$,the equilibrium constant $K_p = P_C$.Statement $(a)$ is correct because the concen

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$a, b, d$ only

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(C) For the reaction $A_{(s)} \rightleftharpoons B_{(s)} + C_{(g)}$,the equilibrium constant $K_p = P_C$.Statement $(a)$ is correct because the concentration of pure solids is taken as unity and does not appear in the equilibrium expression.Statement $(b)$ is correct because $K_p$ is defined by the partial pressure of the gaseous product $C$ at equilibrium.Statement $(c)$ is incorrect because $\Delta H$ (enthalpy of reaction) varies with temperature according to Kirchhoff's law.Statement $(d)$ is correct because a catalyst provides an alternative pathway with lower activation energy but does not change the $\Delta H$ of the reaction.Therefore,statements $(a), (b),$ and $(d)$ are correct.

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