The thermal dissociation equilibrium of CaCO_ | vedclass

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(B) According to Kirchhoff's law,$\Delta H_{T_2} - \Delta H_{T_1} = \int_{T_1}^{T_2} \Delta C_p \, dT$. Since the heat capacity change $\Delta C_p$ is

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$(A, B, D)$

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(B) According to Kirchhoff's law,$\Delta H_{T_2} - \Delta H_{T_1} = \int_{T_1}^{T_2} \Delta C_p \, dT$. Since the heat capacity change $\Delta C_p$ is generally non-zero,$\Delta H$ depends on temperature $T$.$(B)$ The equilibrium constant $K$ for a heterogeneous reaction depends only on temperature and is independent of the initial amounts of solid reactants or products.$(C)$ $K$ is a constant at a fixed temperature; it does not depend on the partial pressure of $CO_2$. The partial pressure of $CO_2$ at equilibrium is equal to $K_p$,which is fixed for a given $T$.$(D)$ $A$ catalyst provides an alternative pathway with a lower activation energy but does not change the enthalpy of reaction $(\Delta H)$ or the equilibrium constant $(K)$.

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