Calculate the change in entropy (in J/K) for the following reaction
at 298 K:
C(s) + H2O(g) → CO(g) + H2(g)
Use entropy for graphite (diamond is too expensive).
Notice that the entropy of the solid is much smaller than the
entropy of the gases!
we have:
Sof(C(s,graphite)) = 5.74 J/mol.K
Sof(H2O(g)) = 188.825 J/mol.K
Sof(CO(g)) = 197.674 J/mol.K
Sof(H2(g)) = 130.684 J/mol.K
we have the Balanced chemical equation as:
C(s,graphite) + H2O(g) ---> CO(g) + H2(g)
deltaSo rxn = 1*Sof(CO(g)) + 1*Sof(H2(g)) - 1*Sof( C(s,graphite)) - 1*Sof(H2O(g))
deltaSo rxn = 1*(197.674) + 1*(130.684) - 1*(5.74) - 1*(188.825)
deltaSo rxn = 133.8 J/K
Answer: 133.8 J/K
Get Answers For Free
Most questions answered within 1 hours.