Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute the molar delta H (in kJ/mol) for this reaction at 298 K and a pressure of 30 bar. Joule-Thomson coefficients and heat capacities are listed in the table below:
Compound | Cp (cal mol^-1 K^-1) |
Joule-thomson coefficient (K/bar) |
CO | 6.3423 + 0.0018363 T | 1.20 |
O2 | 6.148 + 0.003102 T | 1.15 |
CO2 | 6.369 + 0.0101 T | 1.10 |
CO (g) + 0.5 O2 (g) -> CO2 (g)
Cp of CO = 6.3423 + 0.0018363 T
Cp of CO } at T = 298 K = 6.3423 + 0.0018363 * 298
= 6.8895 Cal /molK
Similarly,
Cp of O2 } at T = 298 K = 6.148 + 0.003102 * 298
= 7.0724 Cal /molK
Cp of CO2 } at T = 298 K = 6.369 + 0.0101 * 298
= 9.3788 Cal /molK
Using Joule thomson Coefficient for the molecules:
Hf of CO = - 6.8895 * 1.20 = - 8.2674 Cal/mol
Hf of O2 = - 7.0724 * 1.15 = - 8.13326 Cal/mol
Hf of CO2 = - 9.3788 * 1.10 = - 10.31668 Cal/mol
Now,
Hrxn = Hf (CO2) - [Hf (CO) + Hf (O2)]
= - 10.31668 - [- 8.2674 + 0.5*(- 8.13326)]
= 2.017 Cal/mol
= 0.008439 kJ/mol
=
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