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I am not sure about the answer, can you check out please?
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(iii) Calculate the standard enthalpy change of formation, ∆fH ө, of hydrogen sulfide using the enthalpy change for Reaction 1, and the standard enthalpy changes of combustion below.
Substance ∆cH ө / kJ mol−1
S(s) −296.8
H2(g) −285.8
2H2S(g) + 3O2(g) --> 2SO2(g) + 2H2O(l) ∆rH = –1125 kJ mol−1 Reaction 1
my answer:
S(s) + H2(g) ------------- > H2S(g)
\ /
\ /
> combustion products <
∆fH of H2S = -582.6 + 562.5 = - 20.1 KJmol-1
At first I got -40.2 KJmol-1, unfortunately i don't have the mark scheme.