Respuesta :
The difference between the total of the standard enthalpies of formation for the reactant and product is the reaction's ΔHrxn. Hence, ΔHrxn is - 1124.1 KJ/mol.
Using the following standard enthalpy values :
ΔH°f (H2S) = -20.15 kJ/mol;
ΔH°f (O2) = 0 kJ/, mol;
ΔH°f (H2O) = -285.8 kJ/mol;
ΔH°f (SO2) = -296.4 kJ/mol
The ΔHrxn can be calculated thus :
ΔHrxn = ΔHf product - ΔHf reactant
Sum of ΔHf of the product :
2(-285.8) + 2(-296.4) = - 1164.4 KJ/mol
Sum of ΔHf of the reactant :
2(-20.15) + 3(0) = - 40.30 KJ/mol
The ΔHrxn goes thus :
-1164.4 - (-40.30) = -1164.4 + 40.30 = -1124.1 KJ/mol
Therefore, the ΔH for the reaction is -1124.1 kJ/mol
To know more about ΔHrxn refer to: https://brainly.com/question/18533930
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