Answer:
[tex]\Delta _rH=-1124.14kJ/mol[/tex]
Explanation:
Hello!
In this case, since the standard enthalpy change for a chemical reaction is stood for the enthalpy of reaction, for the given reaction:
[tex]2H_2S(g) +3O_2(g)\rightarrow 2H_2O(l) +2SO_2(g)[/tex]
We set up the enthalpy of reaction considering the enthalpy of formation of each species in the reaction at the specified phase and the stoichiometric coefficient:
[tex]\Delta _rH=2\Delta _fH_{H_2O,liq}+2\Delta _fH_{SO_2,gas}-2\Delta _fH_{H_2S,gas}-3\Delta _fH_{O_2,gas}[/tex]
In such a way, by using the NIST database, we find that:
[tex]\Delta _fH_{H_2O, liq}=-285.83kJ/mol\\\\\Delta _fH_{SO_2, gas}=-296.84kJ/mol\\\\\Delta _fH_{O_2,gas}=0kJ/mol\\\\\Delta _fH_{H_2S,gas}=-20.50kJ/mol[/tex]
Thus, we plug in the enthalpies of formation to obtain:
[tex]\Delta _rH=2(-285.73kJ/mol)+2(-296.84kJ/mol)-2(-20.50kJ/mol)-3(0kJ/mol)\\\\\Delta _rH=-1124.14kJ/mol[/tex]
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