Q. 374.0( 2 Votes )

Following data is

Answer :

Given; CaCO3 (s) CaO3 (s) + CO2 (g)

ΔfH [CaO (s)] = -635.1 kJ mol-1


ΔfH [CO2 (g)] = -393.5 kJ mol-1


ΔfH [CaCO3 (s)] = -1206.9 kJ mol-1


We know that,



Where is the standard enthalpy change for the formation of one mole of compound from its elements in their most stable states of aggregation.


= ΔfH [CaO(s)] + ΔfH [CO2(g)]- ΔfH [CaCO3(s)]


= -635.1 -393.5+1206.9


=178.3 kJ mol-1


=positive


i.e. the reaction is exothermic.


Hence according to Le Chatelier’s Principle on increasing the temperature the reaction will shift to forward direction.


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