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- Aug 24, 2005
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Hey guys,
This is a fairly simple question dealing with enthalpy calculation, but I'm stuck on one little part. Here is the question:
"Given the following reactions:
N2 + O2 ==> 2NO enthalpy = +180.7 kJ
N2 + 2O2 ==> 2NO2 enthalpy = +66.4 kJ
Calculate the enthalpy of reaction for
2NO + O2 ==> 2NO2"
1.) I reversed the first reaction so that I would have 2NO ==> N2 + O2. The enthalpy also becomes -180.7 kJ.
2.) I left the second reaction unaltered.
With the changes made, I would now have:
2NO ==> N2 + O2
N2 + 2O2 ==> 2NO2
The N2 elements would cancel out -- I understand that much. However, what would happen with the 2O2 and O2? Would one of the O2 elements cancel out, leaving me with just one O2 (which is what I need to get to the final reaction and calculate the enthalpy)?
This is a fairly simple question dealing with enthalpy calculation, but I'm stuck on one little part. Here is the question:
"Given the following reactions:
N2 + O2 ==> 2NO enthalpy = +180.7 kJ
N2 + 2O2 ==> 2NO2 enthalpy = +66.4 kJ
Calculate the enthalpy of reaction for
2NO + O2 ==> 2NO2"
1.) I reversed the first reaction so that I would have 2NO ==> N2 + O2. The enthalpy also becomes -180.7 kJ.
2.) I left the second reaction unaltered.
With the changes made, I would now have:
2NO ==> N2 + O2
N2 + 2O2 ==> 2NO2
The N2 elements would cancel out -- I understand that much. However, what would happen with the 2O2 and O2? Would one of the O2 elements cancel out, leaving me with just one O2 (which is what I need to get to the final reaction and calculate the enthalpy)?