Carbon monoxide standard enthalpy

Seif-TeS I 6.13A Gasoline, which contains octane, may burn to carbon monoxide if the air supply is restricted. Determine the standard reaction enthalpy for the incomplete combustion of liquid octane in air to carbon monoxide gas and liquid water from the standard reaction enthalpies for the combustions of octane and carbon monoxide ... 

It is important to note that the energy released by the reaction, CO + Vi 02 — C02, Ah°f2gs = -67.63 kcal/[mol C02], of carbon monoxide and oxygen to form carbon dioxide at 1 atm and the standard temperature is not the standard enthalpy of formation of carbon dioxide, since the reactant, CO, is not a natural element. 

From the enthalpy of formation for CO2 and the following information, calculate the standard enthalpy of formation for carbon monoxide (CO). 

The standard enthalpy of formation, AH, of a substance is the enthalpy change associated with the reaction of the elements of the substance in their standard states to produce the substance in its standard state. Thus the enthalpy of formation of carbon monoxide is the enthalpy change associated with the reaction... 

The standard enthalpies of fonnaDon of leadfll) oxide, carbon monoxide and carbon dioxide are —219, lll uid —394kJmol, reflectively. 

Evaluation of errors and accuracy in combustion calorimetry High-precision combustion calorimetry is considered to be one of the most difficult experimental procedures [37]. The precision required in combustion experiments would have to be 0.01-0.02% in order to have an uncertainty in the enthalpy of formation of approximately 1 kJ mof, which is the precision necessary to obtain reliable thermochemical data. This includes errors in all three different parts of a combustion experiment. In the calorimetric part there are errors in weighing the water in the calorimetric jacket and also in the temperature measurements. In the chemical part there are errors in weighing the sample and in the data for auxiliary materials (benzoic acid, cotton. Vaseline, polythene, etc.), errors in the combustion process caused by production of either carbon monoxide or soot and, in the case of compounds with S or N, errors arising from the production of SO and NO instead of SO2 and NO2. Important errors may arise from sample impurities, water being one of the most important and difficult, because many compounds are hygroscopic. In the third part there are errors in the corrections to the standard state. Thus errors in any part of experiment should be kept imder 0.01%. 

Determine the equilibrium composition that is achieved at 300 bar and 700 K when the initial mole ratio of hydrogen to carbon monoxide is 2. You may use standard enthalpy and Gibbs free energy of formation data. For purposes of this problem you should not neglect the variation of the standard heat of reaction with temperature. You may assume ideal solution behavior but not ideal gas behavior. You may also use a generalized fugacity coefficient chart based on the principle of corresponding states as well as the heat capacity data listed below. 

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