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I'm looking for the energy required for a 2-step chemical reaction:

CaSO4 + S2 -> CaS + 2SO2

CaS + 3CaSO4 -> 4CaO + 4SO2

This reaction is to happen around 1600 deg. F. I solved for the heat of reaction for these two reactions with the following enthalpy equation: H2=H1+∫CpdT I used the heat capacity correlations from the Perry's Chemical Engineers' Handbook.

I found the overall energy required for these two reactions in terms of H2, but I'm afraid it may be wrong. My final answer for a temperature of 1600 deg. F is 2,818 kJ/mol.

I'm wondering if I went about this calculation correctly. I did not solve for the activation energy with the Arrhenius equation, is that something I should have done instead?

Any insight will be greatly appreciated.