will there be change in temperature in :
CaCO3 ------> CaO +CO2
Answers
1st there’s the Gibbs Phase rule which can be rearranged to P = C - F + 2 where P is number of phases, C is the number of components (roughly described as the minimum number of chemical species that are necessary to create all of the species in the system), and F is the number of degrees of freedom. If your system is a solid = solid + gas equilibrium, the system is closed, and either pressure (p) or temperature (T) is fixed, then the other p-T variable will also be fixed at equilibrium so F = 1. The minimum number of components for the system you described is 2 (CaO and CO2) if we assume the conditions are such that no other substances such as CO are being formed. So if you plug those numbers into the equation you’ll get P = 3.
Contrary to one of the other answers, each discrete crystalline solid is a phase (so CaCO3 of whichever crystalline form is present is a phase and CaO is a separate phase). The gas phase is another phase.
I pointed out above that CaCO3 forms different crystalline forms, e.g. calcite, aragonite, and vaterite. Each of those is a different phase since they each have distinct crystalline forms so I suppose that there is a set of p-T conditions where 2 of those CaCO3 forms could be in equilibrium with each other as well as CaO and CO2. In that case, P = 4 and F = 0 (i.e. the system would be invariant = you couldn't change anything in the system without changing the number and identity of the phases)
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Jeferson
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