Use the standard molar entropies in Appendix B to calculate the
standard entropy of reaction for the oxidation of graphite to
carbon monooxide:
2C(s)+O2(g)→2CO(g)
ΔSrxn = ∑[ΔSfo(products)] - ∑[ΔSfo(reactants)]
ΔSrxn = ∑[2 x CO] - ∑[(2 x C) + (1 x O2]
ΔSrxn = [2 x 197.7] - [(2 x 5.7) + (1 x 205.1)] = 178.9 J/mol.K
The standard entropy of reaction for the oxidation of graphite to carbon monooxide: ΔSrxn = 178.9 J/mol.K
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Use the standard molar entropies in Appendix B to calculate the standard entropy of reaction for...
Use the standard molar entropies B to calculate the standard entropy of reaction for the oxidation of graphite to carbon monoxide: 2C(s)+O2(g)→2CO(g) C(s) = 5.7 J/K*mol, O2(g) = 205.0 J/K*mol, CO(g)= 197.6 J/K*mol Express your answer using one decimal place and include the appropriate units.
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
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