Bibliography #640,933

Reference Label	Details
Caneiro 1981	A. Caneiro, J. Fouletier, and M. Kleitz, J. Chem. Thermodyn. 13, 823-832 (1981) Determination of Standard Gibbs Energy Change for CO + 1/2 O2 = CO2 using an Electrochemical Pump and Gauge
note COc	Caneiro 1981 give for the equilibrium CO + 1/2 O2 -> CO2 for the range 400 to 2000 K the equation DeltaG/(kJ/mol) = -(283.328 +- 0.335) + (0.08753 +- 0.00029)*T/(K). The standard deviation is 75 J/mol. while the uncertainties in the equation represent the maximum deviations. In a table of comparison to previous results, they give 1173 K as representative of their range. At that temperature they give DeltaG = -180.66 +- 0.075 kJ/mol (one std dev. uncertainty, based on 56 experiments). From the equation one obtains at 1173 K -180.655 +- 0.477 kJ/mol. They also obtain at 298.15 K a third law value for DeltaH of 282.99 +- 0.13 kJ/mol and a second law value of 283.27 +- 0.29 kJ/mol (range 976-1269 K). using the 1173 K value for DeltaG = -180.655 kJ/mol and standard entropies and enthalpy increments results in DeltaH1173 = -282.004 kJ/mol and DeltaH298 = -283.053 kJ/mol. Note that CODATA Key Vals derives DeltaH298 = -283.05 +- 0.5 kJ/mol from a similar third law analysis. The uncertainty +- 0.15 KJ/mol does not include systematic errors.

Reference Label

Details

Caneiro 1981

A. Caneiro, J. Fouletier, and M. Kleitz, J. Chem. Thermodyn. 13, 823-832 (1981)
Determination of Standard Gibbs Energy Change for CO + 1/2 O2 = CO2 using an Electrochemical Pump and Gauge

note COc

Caneiro 1981 give for the equilibrium CO + 1/2 O2 -> CO2 for the range 400 to 2000 K the equation DeltaG/(kJ/mol) = -(283.328 +- 0.335) + (0.08753 +- 0.00029)*T/(K). The standard deviation is 75 J/mol. while the uncertainties in the equation represent the maximum deviations. In a table of comparison to previous results, they give 1173 K as representative of their range. At that temperature they give DeltaG = -180.66 +- 0.075 kJ/mol (one std dev. uncertainty, based on 56 experiments). From the equation one obtains at 1173 K -180.655 +- 0.477 kJ/mol. They also obtain at 298.15 K a third law value for DeltaH of 282.99 +- 0.13 kJ/mol and a second law value of 283.27 +- 0.29 kJ/mol (range 976-1269 K). using the 1173 K value for DeltaG = -180.655 kJ/mol and standard entropies and enthalpy increments results in DeltaH1173 = -282.004 kJ/mol and DeltaH298 = -283.053 kJ/mol. Note that CODATA Key Vals derives DeltaH298 = -283.05 +- 0.5 kJ/mol from a similar third law analysis. The uncertainty +- 0.15 KJ/mol does not include systematic errors.