Asked by Jane
Please help!
Calculate the standard change in enthalpy, ΔH°rxn, for the decomposition of calcium carbonate to calcium oxide
CaCO3 (s) → CaO (s) + CO2 (g) Given that:
ΔH°f CaCO3 (s) = -1206.9 kJ/mol
ΔH°f CaO (s) = -635.1 kJ/mol
ΔH°f CO2 (g) = -393.5 kJ/mol
Calculate the standard change in enthalpy, ΔH°rxn, for the decomposition of calcium carbonate to calcium oxide
CaCO3 (s) → CaO (s) + CO2 (g) Given that:
ΔH°f CaCO3 (s) = -1206.9 kJ/mol
ΔH°f CaO (s) = -635.1 kJ/mol
ΔH°f CO2 (g) = -393.5 kJ/mol
Answers
Answered by
bobpursley
Hess' Law:
Hr=--635.1 kJ-393.5kJ-(-1205.9)kJ
In my head, looks like about it is endothermic (absorbs heat). I bet that is why limestone has to be heated in a furnace to make quick lime.
Hr=--635.1 kJ-393.5kJ-(-1205.9)kJ
In my head, looks like about it is endothermic (absorbs heat). I bet that is why limestone has to be heated in a furnace to make quick lime.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.