6-56) Use standard enthalpies of formation to calculate ΔHrxn° for each reaction.
a) 2 H2S(g) + 3 O2(g) ⇒2 H2O(l) + 2 SO2(g)
b) SO2(g) + 12 O2(g) ⇒ SO3(g)
c) C(s) + H2O(g) ⇒ CO(g) + H2(g)
d) N2O4(g) + 4 H2(g) ⇒ N2(g) + 4 H2O(g)
a) 2 H2S(g) + 3 O2(g) ⇒2 H2O(l) + 2 SO2(g)
Hrex = Hf products - Hf reactants
= 2*-296.82 + 2*-285.82 -(2*-20.16) = -1124.96KJ
b) SO2(g) + 12 O2(g) ⇒ SO3(g)
Hrex = Hf products - Hf reactants
= -395.72 -(-296.82 ) = -98.9KJ
c) C(s) + H2O(g) ⇒ CO(g) + H2(g)
Hrex = Hf products - Hf reactants
= (-110.54 + 0) -(1.89-241.8) = 129.37KJ
d) N2O4(g) + 4 H2(g) ⇒ N2(g) + 4 H2O(g)
Hrex = Hf products - Hf reactant
= (4*-241.8 + 0)-(9.16+4*0) = -976.36KJ
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