Sunday
April 20, 2014

Homework Help: Chemistry

Posted by Stuck on Thursday, April 8, 2010 at 10:54pm.

"Given that the bond enthalpy of the carbon-oxygen bonds in carbon monoxide and carbon dioxide are 1073 kJ/mol and 743 kJ/mol respectively, and that of the bond in the oxygen molecule is 496 kJ/mol, calculate the enthalpy change for the combustion of 1 mole of carbon monoxide."

So I have:

2CO2(g) + O2 (g) -> 2CO2(g)

Delta H = (2 mol)(1073 kJ/mol) + (1 mol)(496 kJ/mol)-[(4 mol)(743 kJ/mol)]

Delta H = -330 kJ/mol

But I know that that is not right. It's part of the correct process...what am I missing?

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